Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Rate Law represents an equation for a chemical reaction that connects the reaction rate with the concentrations or pressures of the reactants and the rate constant. 

Rate Law

When it comes to the rate of a reaction the Rate Law focuses on the reactant concentrations, while ignoring the product concentrations. 

Concept #1: Understanding the Rate Law. 

By focusing on only the reactant concentrations we only care about the forward direction of our chemical reaction. 

Concept #2: The Rate Determining Step. 

If the reaction says it’s a SLOW step or a ONE-STEP MECHANISM then we can simply look at the coefficients of the reactants to determine the reaction orders. 

Example #1: For the following reaction, use the given rate law to determine the best answer for the reaction with respect to each reactant and the overall order.

H2O2 (aq) + 3 I (aq) + 2 H+ (aq)  --->  I3 + 2 H2O (l)  

 

Rate = k [H2O2]2 [I ]

 

a) H2O2 is 1st order, I is 1st order, 2nd order overall.

b) H2O2 is 2nd order, I is 1st order, 3nd order overall.

c) H2O2 is 0th order, I is 1st order, H+ is 1st order, 3rd order overall.

d) H2O2 is 2nd order, I is 1st order, H+ is 0th order, 3rd order overall.

Example #2: Answer each of the following question based on the following chemical reaction:

Calculate the reaction order for reactant A. 

Practice: Calculate the reaction orders for Reactants B and C.

Example #3: Calculate the rate constant and the new rate for the given reaction if the initial concentration of [A] = 0.300 M, [B] = 0.150 M and [C] = 0.150 M.

The Rate Constant k

The Rate Constant k can have a direct impact on the rate of the reaction. In order to determine its units just utilize the equation below, where n is the overall order of the reaction: 

Example #4: A certain chemical reaction has the given rate law:

Rate = k [A]3 [B]2 [C]-1

What are the units of the rate constant for the given reaction?

a) M-2 s-1      b) M2 s-1       c) M-4 s-1      d) M-3 s-1      e) M3 s-1

Example #5: The reaction of 3 A + B ---> 2 C + D, was found to be: Rate = k [A]2 [B]3. How much would the rate increase by if A were tripled while B were increased by half?

a) 0.50              b) 30.38            c) 0.75              d) 20.25            e) 1.125

Practice: If the rate law for the following reaction is found to be the following, what are the units for the rate constant, K?

Cl2 (g) + HCCl3 (g) → HCl (g) + CCl4 (g)

a)          b)           c)           d)           e) 

Reaction Mechanisms

Concept #3: A   Reaction Mechanism   involves a series of elementary reactions that give the overall equation. 

Additional Problems
Consider a reaction with the following rate law Rate = k [C]2[D]3[E]-1 By what factor would the rate of the reaction increase if the concentration of [C] tripled, the concentration of D is increased by half and concentration of [E] doubled? A. 15.2 B. 12.9 C. 9.0 D. 6.5 E. 30.4
 The rate law for a reaction is Rate = k[A][B]2 Which one of the following statements is false? a. The reaction is second order in respect to B.  b. If [B] is doubled, the reaction rate will increase by a factor of 4. c. If [A] is doubled, the reaction rate will increase by a factor of 2. d. The reaction is first order overall. 
Determine the rate law for the reaction 2ClO2 (aq) + 2 OH - (aq) → ClO2- + H2O (l) given the following data. a. Rate = k[ClO2][OH-] b. Rate = k[ClO2]2[OH-] c. Rate = k[ClO2]2[OH-]2 d. Rate = k[ClO2][OH-]2 e. Rate = k[OH-]
Consider the reaction A + B + C → products. It has the rate law rate = k[A]  -1[B]3[C]2 Which of the following statements(s) is/are correct? i. The units of the rate constant are M -3 time-1. ii. The overall order of the reaction is 5. iii. Increasing the concentration of A by a factor of 3, B by a factor of 2 and C by a factor of 4 results in the overall rate increasing by a factor of 42.7. A. i only B. ii only C. iii only D. i and iii E. ii and iii
The rate law for the reaction H2O2 + 2H+ + 2l- → I2 + 2H2O is rate = k [H2O2] [I-]. the overall order of the reaction is (A) five (B) three (C) two (D) one
The reaction of peroxydisulfate ion (S2O8 2- ) with iodide ion (I - ) is: S2O8 2- (aq) + 3I - (aq) → 2SO4 2- (aq) + I3 - (aq) a.) What is the rate law?     b.) What is the rate constant?          
The reaction of peroxydisulfate ion (S2O82‐) with Iodide ion (I1‐) S2O82–+ 3 I –(aq) → 2SO42– + I3 From the data below calculate the rate constant for the reaction, k. A) 0.143 B) 0.0049 C) 0.0115 D) 0.061 E) 0.337  
Consider the reaction A → B The rate of the reaction is 2.0 x 10 ‐2 M/s when the concentration of A is 0.31 M. Calculate the rate constant if the reaction is second order in A,  include the correct units in your answer. A) 0.0645 s‐1 B) 0.208 s‐1 C) 0.0062 s‐1 D) 0.0645 M‐1s‐1 E) 0.208 M‐1s‐1  
Consider this reaction and its rate law. 3A + 2B --> products rate = k[A][B] What is the order with respect to A? What is the order with respect to B? What is the overall reaction order?
Give the characteristic of a first order reaction having only one reactant.  A. The rate of the reaction is not proportional to the concentration of the reactant. B. The rate of the reaction is proportional to the square of the concentration of the reactant. C. The rate of the reaction is proportional to the square root of the concentration of the reactant. D. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.  E. The rate of the reaction is directly proportional to the concentration of the reactant. 
What is the overall order of the following reaction, given the rate law? 2NO(g) + H2(g) → N2(g) + 2H2O(g) Rate = k [NO]2[H2] A. 1st order B. 2nd order C. 3rd order D. 4th order E. 0th order
What are the units of k in the following rate law? A. Rate = k[X][Y]2 A) 1/Ms2 B) 1/M2s C) M2s D) M2/s E) 1/M3s
Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? A. Rate = k[X]2[Y]3 A) The rate of reaction will increase by a factor of 9. B) The rate of reaction will increase by a factor of 2. C) The rate of reaction will increase by a factor of 8. D) The rate of reaction will increase by a factor of 4. E) The rate of reaction will remain unchanged.
Determine the rate law and the value of k for the following reaction using the data providded. CO(g) + Cl2(g) → COCl2(g) [CO]i(M) [Cl2]i(M) Initial Rate (M-1s-1) 0.25         0.40             0.696 0.25         0.80             1.97 0.50         0.80             3.94 A) Rate = 11 M-3/2s-1[CO][Cl2]3/2 B) Rate = 36 M-1.8s-1[CO][Cl2]2.8 C) Rate = 17 M-2s-1[CO][Cl2]2 D) Rate = 4.4 M-1/2s-1[CO][Cl2]1/2 E) Rate = 18 M-3/2s-1[CO]2[Cl2]1/2  
Consult the table and find the rate constant of the reaction. A) 2.1 x 10-2 M-1 s-1 B) 2.1 x 10-1 M-1 s-1 C) 2.3 x 10-2 M-1 s-1 D) 1.4 x 10-1 M-1 s-1 E) 6.9 x 10-2 M-1 s-1
The reaction between ethyl bromide (C2H5Br) and hydroxide ion (OH -) in ethyl alcohol at 330 K is first order each in ethyl bromide and hydroxide ion. C2H5Br(alc) + OH -(alc) → C2H5OH(I) + Br -(alc) How would the rate of ethyl bromide change if the solution were diluted by adding an equal volume of pure ethyl alcohol to the solution.   a) no change b) decrease by a factor of four c) increase by a factor of four d) increase by a factor of two e) decrease by a factor of two
If the rate of a reaction increases by a factor of 9 when the concentration of reactant increases by a factor of 3, the order of the reaction (with respect to this reactant) is a) 2 b) 3 c) 9 d) 4 e) 1 
Given that the rate law for the production of water 2 H2 (g) +  O2 (g) → 2 H2O (l) is rate = k[H2]2[O2] –1, then the overall order of the reaction is  a) 1 b) 2 c) 3 d) –1 e) 0  
For the reaction 2A + B → products determine the rate law for the reaction given the following data:  Initial Concentration M,           Initial Rate, M·s–1   A          B 0.10       0.10                           2.0 x 10   –2 0.20       0.10                           8.0 x 10   –2 0.30       0.10                           1.8 x 10   –1 0.20       0.20                           8.0 x 10   –2 0.30       0.30                           1.8 x 10   –1 a) rate = k [A] b) rate = k [A][B] c) rate = k[A] [B] 0 d) rate = k[A]2 e) rate = k[B]2
When the reaction CH3Cl(g) + H2O(g) → CH3OH(g) + HCl(g) was studied, the tabulated data were obtained. Based on these data, what are the reaction orders? (A) CH3Cl: first order         H 2O: first order (B) CH3Cl: first order         H 2O: second order (C) CH3Cl: second order     H 2O: first order (D) CH3Cl: second order     H 2O: second order
The gas-phase reaction, A2 + B2 → 2AB, proceeds by bimolecular collisions between A2 and B2 molecules. If the concentrations of both A2 and B2 are doubled, the reaction rate will change by a factor of A) 1/2 B) √2 C) 2 D) 4
The following kinetic data was obtained for the reaction 2A + B → Products
Initial rate data for the reaction 2 H2 (g) + Cl2 (g) are given in the table. What is the rate law for this reaction? (A) rate k [Cl2]2 (B) rate = k [Cl2] (C) rate = k [H2] (D) rate = k [H2] [Cl2]
A kinetic study of the reaction 2 ClO2(aq) + 2 OH -(aq) → ClO2- (aq) + ClO3- (aq) +   H2O(l) yielded the data shown on the image. A.  What is the rate of appearance of the ClO3- in experiment 1 (Be sure to inlcude units in this and other answers.)   B. Determine the experimental rate law.   C. Determine the value of the rate constant  based on your answer to Part C. (Inlude units)
If the rate for the following reaction is found to be the following: Rate = k [Cl2]3/2 • [HCCl3]. What are the units for the rate constant, k? Cl2 (g) + HCCl3 (g)       →      HCl (g) + CCl 4 (g)    
A reaction is second order in [A]. What happens to the rate when the concentration of A is doubled? A. The rate remains unchanged B. The rate increases by a factor of two C. The rate increases by a factor of three D. The rate increases by a factor of four E. The rate increases by a factor of nine
Given k = 7.8 x 10  - 2 s -1 for a reaction which is first order in A, what is the initial rate of the reaction (M/s) when the initial concentration of A is 0.0030 M? A. 2.3 x 10 -4 B. 7.9 x 10 -4 C. 9.2 x 10 -4 D. 2.6 x 101 E. 7.7 x 101
Initial rate data have been determined at a certain temperature for the gaseous reaction. The numerical value of the rate constant is: A. 7.5 B. 3.0 x 10 -3 C. 380 D. 0.75 E. 3.0 x 10 -4
The initial rate of a reaction which is first order in A is 1.0 × 10  −6 M/s when the initial concentration is 0.0040 M. What is the first order rate constant (s−1)? A. 4.0 × 10 -9 B. 1.0 × 10 -9 C. 2.5 × 10 -3 D. 1.0 × 10 -4 E. 2.5 × 10 -4
A first order reaction has a rate constant equal to 75 days -1. What is the rate constant in hrs-1?
The reaction A → B + C is known to be zero order in A with a rate constant of 3.0 × 10−2 mol/Ls at 25 °C. An experiment was run at 25 °C where [A] o = 1.0 × 10 -3 M. After 5.0 minutes the rate is? A. 5.0 × 10 -2mol/Ls B. 2.5 × 10 -2mol/Ls C. 1.25 × 10 -2mol/Ls D. 1.0 × 10 -3mol/Ls E. none of these
The reaction A + 2B → products has the rate law, rate = k [A][B]3. If the concentration of B is doubled while that of A is unchanged, by what factor will the rate of reaction increase? A) 2 B) 4 C) 6 D) 8 E) 9
For the reaction: 2N2O5(g) → 4NO2(g) + O2(g) the rate constant is k = 2.8×10−3 sec−1. What is the order of the reaction? a) Second b) Zeroth c) Third d) First e) None of the above
The rate law of a reaction is rate = k[D][X]. What are the units of the rate constant? A. mol L-1s-1 B. L mol-1s-1 C. mol2 L-2s-1 D. mol L-1s-2 E. L2 mol -2s-1
The rate law for the reaction: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) is rate = k [Cl2]1/2[CHCl3]3/4. The units for the rate constant are a) M−1/4 sec−1 b) M1/4 sec−1 c) M−5/4 sec−1 d) M−1/2 sec−1 e) M−1 sec-1
A reaction was found to be second order in carbon monoxide concentration. If the concentration of carbon monoxide is tripled, the rate of the reaction a) remains unchanged b) doubles c) triples d) increases by a factor of 9 e) increases by a factor of 4
The following chemical reaction produced this chemical kinetics data. 
What is the overall order of the following reaction, given the rate law? 2NO (g) + H2 (g) ⇌ N2 (g) + 2H2O(g)  Rate = k [NO]2[H2]   A. 3rd order B. 0th order C. 1st order D. 2nd order E. 4th order
Based on your knowledge of rate law determine the answer. 
Based on your knowledge of rate law answer the following question. 
Determine the rate constant for the reaction between SO 2, O2, and H2O from the information given in the table below. a) 6.19x10−3 b) 1.37x10−2 c) 4.12x10−2 d) 3.09x10−4 e) 2.06x10−3    
For a certain reaction, the rate law is Rate = k[A][B] 1/2. What are the units of the rate constant? a) conc−3/2 s−1 b) conc−1/2 s c) conc s−1/2 d) conc1/2 s−1 e) conc−1/2 s−1
If the rate law for a reaction is given by Rate = k[A] 1/2[B]3 what will be the effect on the reaction rate if the concentration of A is increased by a factor of 4 and the concentration of B is lowered by a factor of 2?   a) Increase by a factor of 2 b) Remain unchanged c) Decrease by a factor of 4 d) Decrease by a factor of 21/2 e) Increase by a factor of 4
Determine the rate law for the reaction between I 2 and C3H7Br from the information given in the table below.  a) k[I2]1/2[C3H7Br] b) k[I2]1/2[C3H7Br]2 c) k[I2]1/3[C3H7Br]2 d) k[I2]1/4[ C3H7Br]2 e) k[I2]1/3[C3H7Br]  
The following table shows a series of experiements that were performed to determine the rate of NO2 production from O2 and NO: O2(g) + 2NO(g) → 2NO2(g)    a) What is the order with respect to O 2?        b) What is the order of the reaction with respect to NO?       c) What is the overall order of the reaction?  
For the reaction of chlorine and nitric oxide,  2NO(g) + Cl2(g) → 2NOCl(g) doubling the concentration of chlorine doubles the rate of reaction. Doubling the concentration of both reactants increases the rate of reaction by a factor of eight. The reaction is (A) first order in both NO and Cl 2. (B) first order in NO and second order in Cl 2. (C) second order in NO and first order in Cl 2. (D) second order in both NO and Cl 2.
A plot of 1/concentration of A (M-1) vs time (min) gave a straight line with the following formula: y = 0.20x + 2.0. Which of the following is the correct expression for the rate law? Assume a =1. a) Rate = 0.2 M-1 min-1 b) Rate = 0.2 M-1 min-1 [A] c) Rate = -0.2 M-1 min-1 [A] d) Rate = 0.2 M-1 min-1 [A]2 e) Rate = -0.2 M-1 min-1 [A]2
Many gaseous reactions occur in a car engine and exhaust system. One of these is represented by the following equation: NO2 (g) + CO (g) ⇄ NO (g) + CO2 (g) What is the rate of the reaction if the concentrations of NO2 and CO are 0.25 M and 0.30 M respectively?  For the choices below, what is the order of reaction for NO2?
The reaction below has an initial rate of 0.070 M/s. What will the initial rate be if [A] is halved and [B] is tripled?  A  +  B  →  C  +  D         Rate = k [A][B]  2 a) 0.105 M/s b) 0.000343 M/s c) 0.315 M/s d) 0.210 M/s e) 0.0098 M/s
Using the given data, determine the rate constant of this reaction. A + 2 B → C + D Given Data: Trial       [A](M)     [B](M)       RATE (M/s) 1            0.310      0.340          0.0213 2            0.310      0.680          0.0213 3            0.620      0.340          0.0852  
The reaction between acetone and bromine in acid solution is represented by the equation CH3OCH3(aq) + Br2(aq) + H3O+(aq) → products The tabulated kinetic data were gathered. Based on these data, the experimental rate law is:
A certain chemical reaction has the following rate law Rate = k [A]2[B]3[C]-2[D] What are the units of the rate constant for this reaction? 
If the rate law for the following reaction is found to be the following: Rate = [Cl2]3/2 • [HCCl3].  What are the units for the rate constant, k?  Cl2 (g) + HCCl3 → (g) HCl (g)  +   CCl4 (g)  
Given the initial concentrations in  Kinetics Data Table 1, predict what the rate would be if the initial concentrations were [A] = 0.062 M, [B] = 1.03 M, and [C] = 1.12 M. 2 A + 3 B + C → 2 D + E a. 2.026 M/s b. 0.126 M/s c. 2.086 M/s d. 1.863 M/s e. 0.112 M/s  
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A .What is the order of the reaction with respect to A?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A .Write a rate law for the reaction.
How is the order of a reaction generally determined?
For a reaction with multiple reactants (Rate = k [A]m[B]n), how is the overall order of the reaction defined?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant .What is the order of the reaction with respect to A?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant .Write a rate law for the reaction.
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.Write a rate law for the reaction.
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.What is the overall order of the reaction?
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant A for the reaction A .Estimate the value of k.
The graph below shows a plot of the rate of a reaction versus the concentration of the reactant .Estimate the value of k.
What are the units of k for each of the following?first-order reaction
What are the units of k for each of the following?second-order reaction
What are the units of k for each of the following?zero-order reaction
A reaction in which A was monitored as a function of time and the results are shown below. Time (s) [A] (M) 0 1.000 25 0.914 50 0.829 75 0.744 100 0.659 125 0.573 150 0.488 175 0.403 200 0.318 What is the rate of reaction when [A] = 0.21 M ?
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)?
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.By what factor does the reaction rate change if the concentrations of all three reactants are doubled?
A student says, “The initial concentration of a reactant was doubled, and the rate doubled. Therefore the reaction is second order in that reactant.” Why might the student say that? What is wrong with the statement? What is the actual order with respect to the reactant?
Consider a reaction with the following rate law. Rate = k [X]2[Y]3[Z]-1 What are the units of the rate constant for this reaction? A. M-4 time-1 B. M-3 time-1 C. M time -1 D. M4 time-1 E. M3 time-1
Consider this initial-rate data at a certain temperature for the reaction described by 2NO2(g) + O3(g) → N2O5 (g) +O2 (g) Determine the value and units of the rate constant.
Consider this initial-rate data at a certain temperature for the reaction described by:   N2O3(g) → NO(g) + NO2(g) Determine the value and units of the rate constant.  
Write the rate law for these two elementary reaction equations. (a) 2A(g) + B(g) → C(g) + D(g) (b) X(R) + Y(g) → Z(g) 
Consider the following elementary reaction equation. 2O2(g) + Cl(g) → ClO(g) + O3(g) a) What is the order with respect to O 2. b) What is the overall order of the reaction. c) Classify the reaction as a unimolecular, bimolecular, or termolecular.
For the following rate law rate = k[A] x  determine the value of x ifthe rate doubles when [A] is doubled.x= __________the rate quadruples when [A] is doubled.x=__________
For the following rate law rate = k[A]x. Determine the value of x if:a) the rate doubles when [A] is doubled.b) no change in rate occurs when [A] is doubled.
CH3Br + NaOH ->CH3OH + NaBrWhen the concentration of CH3Br and NaOH are both 0.100M, the rate of the reaction is 0.0050 M/s. a. What is the rate of the reaction if the concentration of CH3Br is doubled? _____M/s b. What is the rate of the reaction if the concentration of NaOH is halved? _____M/s c. What is the rate of the reaction if the concentrations of CH3Br and NaOH are both increased by a factor of six? ____M/s
Consider the reaction described by the following equation.C2H4Br2(aq) + 3I- (aq) → C2H4(g)+2Br- (aq)+I3-(aq)The rate law israte = k[C2H4Br2] [I-]     where k= 4.91 x 10-3 M-1 • s-1What are the missing entries in the following table?  
Consider this reaction and its rate law. 3A + 2B → products rate = k[A][B] a) What is the order with respect to A? b) What is the order with respect to B? c) What is the overall reaction order?
Consider the reaction 
For the reaction (CH3)3CBr(aq) + OH-(aq) → (CH3)3COH(aq) + Br-(aq), the following data were obtained at 55 °C. What is the rate constant? a) 1.0 x 10-4 s-1 b) 2.0 x 10-2 s-1 c) 2.0 x 10-3 s-1 d) 1.0 x 10-2 s-1 e) 1.0 x 10-1 s-1
The following reaction is a single-step, bimolecular reaction:CH3Br+NaOH → CH3OH+NaBr.When the concentrations of CH3Br and NaOH are both 0.170 M, the rate of the reaction is 0.0090 M/s.a. What is the rate of the reaction if the concentration of CH3Br is doubled?b. What is the rate of the reaction if the concentration of NaOH is halved?c. What is the rate of the reaction if the concentrations of CH3Br and NaOH are both increased by a factor of five? 
For the reaction A(g) + 2B(g) → 2C(g) + 2D(g), the following data was collected at constant temperature. Determine the correct rate law for this reaction. a) Rate = k[A][B] b) Rate = k[A]2[B] c) Rate = k[A][B]2 d) Rate = k[A] e) Rate = k[A]3
For each reaction order, identify the proper units for the rate constant, k. Not all choices will be used.
What are dimensions of rate constant units for third-order reaction, give an example.
Fill in the units for the apparent rate constant for each reaction order given below.
For the reaction A +B+ C → D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: What is the value of the rate constant k for this reaction? Express your answer to two significant figures and include the appropriate units.   
Calculate the initial rate for the formation of C at 25°C, if [A]=0.50M and [B]=0.075M. Express your answer to two significant figures and include the appropriate units. Consider the reaction A+2B → C whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table:   Trial                    [A]                    [B]                    Rate                           (M)                   (M)                    (M/s) 1                       0.20                 0.030                1.4 x 10 - 3   2                       0.20                 0.060                2.9 x 10      - 3 3                       0.40                 0.030                5.8 x 10       - 3    
Nitrogen monoxide gas can react with oxygen to produce nitrogen dioxide gas as represented below 2 NO (g) + O2 (g) → 2 NO2 (g) A rate study of the reaction yielded the data recorded in the table below                                                                                                                       (mol L-1s-1) Experiment     Initial Conc. of NO (molL-1)    Initial conc. of O2      Initial rate of formation of NO2           1                             .0200                                .0300                              8.52 x10 -2       2                             .0200                                .0900                              2.56 x 10-1       3                             .0600                                .0300                              7.67 x 10-1 a) Determine the order of the reaction with respect to each of thefollowing reactants. Give details of your reasoning, clearly explaining or showing how you arrived at your answers. i) NO       ii) O2       b) Write the expression for the rate law of the reaction as determined from the experimental data     c) Determine the value of the rate constant for the reaction, clearly indicating the units
Consider this initial-rate data at a certain temperature for the reaction described by 2NOBr(g) → 2NO(g) + Br 2(g)   [NOBr]0 (M)              Initial rate of formation of Br  2 (M/s) 0.600                        1.01 x 10   2 0.750                        1.58 x 10   2 0.900                         2.27 x 10   2   Determine the value and units of the rate constant k =  
Consider this reaction and its rate law. 4A + 3B → products   rate = k[A] 2 [B]2. a) What is the order with respect to A? b) What is the order with respect to B? c) What is the overall reaction order?
The reaction A + B → C + D             rate = k[A][B]  2 has an initial rate of 0.0110 M/s. What will the initial rate be if [A] is halved and [B] is tripled? _____ M/s What will the initial rate be if [A] is tripled and [B] is halved? _____ M/s
Consider the following elementary reaction equation: H2O2(g) → H2O(g) + O(g)a. What is the order with respect to H 2O2?b. What is the overall order of the reaction?c. Classify the reaction as unimolecular, bimolecular or termolecular
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide describe by:O3(g) + NO(g) → O2(g) + NO2(g)The rate law for this reaction is:rate of reaction = k[O3][NO]a. Given that k = 3.66x10 6 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O 3]0 = 2.25x10-6 M and [NO]0 = 4.37x10-5 M, owing to continuous production from separate sources. (M s-1)b. Calculate the number of moles of NO2(g) produced per hour per liter of air. (mol h -1  L-1) 
Using the given data, calculate the rate constant of this reaction.                                      A+B →  C+D Trial            [A](M)          [B](M)          Rate(M/s)                   k=_____? 1                  0.340           0.200           0.0142                  2                  0.340           0.520           0.0960                  3                  0.476           0.200           0.0199                                       
Using the given data, determine the rate constant of this reaction. A + 2B → C + D  
Consider the reaction described by the following equation. 
Using the given data, determine the rate constant of this reaction. A + 2B → C + D Given Data: Trial         [A](M)           [B](M)        RATE (M/s) 1              .330              .280           0.0236 2              .30                .560           0.0236 3              .660              .280           0.0944 k=? the units are M-1 s-1  
Determine the rate law and the value of k for the following reaction using the data provided.2 NO(g) + O2(g) → 2NO2(g)
The following reaction is a single-step, bimolecular reaction:CH3Br +NaOH → CH3OH +NaBrWhen the concentrations of CH3Br and NaOH are both 0.125 M, the rate of the reaction is 0.0060 M/sa. What is the rate of the reaction if the concentration of CH3Br is doubled?b. What is the rate of the reaction if the concentration of NaOH is halved?c. What is the rate of the reaction if the concentration of CH3Br and NaOH are both increased by a factor of six?
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A]  (M)Initial Rate (M/s)0.1000.0650.2000.1300.3000.195What is the order of the reaction?
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning.
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A]  (M)Initial Rate (M/s)0.1000.0650.2000.1300.3000.195Write a rate law for the reaction.
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions:(b) Write the overall rate law for the reaction.
You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem.Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M) Initial rate (M/s)0.150.0090.300.0190.600.038What is the order of the reaction?
You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem.Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M) Initial rate (M/s)0.150.0090.300.0190.600.038Specify a rate law for the reaction.
The data below were collected for the following reaction: 2NO2(g) + F2(g) → 2 NO2F(g) [NO2] (M)  [F2] (M)  Initial Rate (M/s) 0.1000.1000.0260.2000.1000.0510.2000.2000.1030.4000.4000.411What is the overall order of the reaction?
The data below were collected for the following reaction: 2NO2(g) + F2(g) → 2 NO2F(g) [NO2] (M)  [F2] (M)  Initial Rate (M/s) 0.1000.1000.0260.2000.1000.0510.2000.2000.1030.4000.4000.411Write an expression for the reaction rate law.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)[CH3Cl] (M)[Cl2] (M)Initial Rate (M/s)0.0500.0500.0140.1000.0500.0290.1000.1000.0410.2000.2000.115Write an expression for the reaction rate law.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)[CH3Cl] (M)[Cl2] (M)Initial Rate (M/s)0.0500.0500.0140.1000.0500.0290.1000.1000.0410.2000.2000.115What is the overall order of the reaction?
The reaction2NO (g) + Cl2 (g) → 2NOCl (g)was studied at -10°C. The following results were obtained whereRate = -Δ[Cl2] / Δta. What is the rate law? 
The reaction2I- (aq) + S2O82- (aq) → I2 (aq) + 2SO42- (aq)was studied at 25°C. The following results were obtained wherea. Determine the rate law. 
The decomposition of nitrosyl chloride was studied:2NOCl (g) ⇌ 2NO (g) + Cl2 (g)The following data were obtained wherea. What is the rate law? 
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)b. Determine the rate law. 
The reactionI - (aq) + OCl - (aq) → IO - (aq) + Cl - (aq)was studied, and the following data were obtained:a. What is the rate law? 
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)a. Determine the orders of this reaction with respect to Hb and CO. 
The following reaction was monitored as a function of time: A → B + C. A plot of ln[A] versus time yields a straight line with slope −4.4×10−3 /s. Write the rate law for the reaction.
What is the order of reaction with respect to A and B for a reaction that obeys the rate law rate = k[A]2[B]3?
The rate of the reactionO (g) + NO2 (g) → NO (g) + O2 (g)was studied at a certain temperature.a. In one experiment, NO2 was in large excess, at a concentration of 1.0 x 10 13 molecules/cm3 with the following data collected:What is the order of the reaction with respect to oxygen atoms?
At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction is: CH3CHO(g) → CH4(g) + CO(g). A sample of CH3CHO is heated to 700 K and the pressure is measured as 0.31 atm before any reaction takes place. The kinetics of the reaction are then followed by measurements of total pressure and these data are obtained:t (s)010003000  7000  PTotal (atm)0.31  0.35  0.400.46Find the rate law.
At 400 K oxalic acid decomposes according to the reaction: H2C2O4(g) → CO2(g) + HCOOH(g). In three separate experiments, the initial pressure of oxalic acid and final total pressure after 20,000 s is measured.Experiment123P H2C2O4 at t = 065.8  92.1  111PTotal at t = 20,000 s93.6131158  Find the rate law of the reaction.
You may want to reference (Page 629) Section 14.2 while completing this problem.This plot shows the rate of the decomposition of SO2Cl2 into SO2 and Cl2 as a function of the concentration of SO2Cl2.What is the order of the reaction?
For the reaction A ⟶ B + C, the following data were obtained at 30 °C:(a) What is the order of the reaction with respect to [A], and what is the rate equation?
For the reaction Q ⟶ W + X, the following data were obtained at 30 °C:(a) What is the order of the reaction with respect to [Q], and what is the rate equation?
You may want to reference(Page 630) Section 14.3 while completing this problem.For the reaction 2A + B → C, the initial rate was measured at several different reactant concentrations. From the resulting tabulated data, determine the rate law for the reaction. [A] (M)  [B] (M) Initial Rate (M/s)0.050.050.0350.100.050.0700.200.100.56
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.What is the overall order of the reaction?
You may want to reference (Pages 635 - 641) section 14.4 while completing this problem.The following reaction was monitored as a function of time: AB → A + B.A plot of 1/[AB] versus time yields a straight line with slope 5.6×10−2 (M s)-1.Write the rate law for the reaction.
You may want to reference(Pages 629 - 634) Section 14.3 while completing this problem.Consider the following reaction: CHCl3(g) + Cl2(g) → CCl4(g) + HCl(g)The initial rate of the reaction is measured at several different concentrations of the reactants with the following results:[CHCl3] (M)[Cl2] (M)Initial Rate (M/s)0.0100.0100.00340.0200.0100.00680.0200.0200.00960.0400.0400.027From the data, determine the rate law for the reaction.      
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M)Initial rate(M/s)0.127.92×10−30.161.056×10−20.201.32×10−2What is the order of the reaction?
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M)Initial Rate (M/s m M/s)0.120.0003890.180.0008750.280.00212What is the order of the reaction?
The reactionH2SeO3 (aq) + 6I - (aq) + 4H+ (aq) → Se (s) + 2I 3- (aq) + 3H2O (l)was studied at 0°C, and the following data were obtained:These relationships hold only if there is a very small amount of I  3- present. What is the rate law and the value of the rate constant? (Assume that rate = - Δ[H2SeO3] / Δt)
For the reaction  A + B + C → D + E the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Trial            [A]       [B]        [C]        Initial rate                   (M)      (M)       (M)           (M/s) 1                0.50    0.50       0.50     1.5 x 10   -4 2                0.50    0.50       1.50     4.5 x 10   -4 3               1.00    0.50       0.50     6.0 x 10   -4 4               1.00    1.00       0.50     6.0 x 10   -4 a. Find the reaction order with respect to A. b. Find the reaction order with respect to B. c. Find the reaction order with respect to C.
The reaction A(aq) + B(aq) → products(aq) was studied, and the following data were obtained:What is the order of the reaction with respect to A? What is the order of the reaction with respect to B? What is the value of the rate constant for the reaction?
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3 × 104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 µg (0.15 × 10−6 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g) a. Calculate the value of the rate constant, k. Express your answer using two significant figures. b. What is the overall order of the reaction? Express your answer using two significant figures.
Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A]  (M)Initial Rate (M/s)0.1000.0650.2000.1300.3000.195Estimate the value of the rate constant, k.
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions:(c) Calculate the value of the rate constant, k, for the reaction. Include units.
You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem.Consider the following data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M) Initial rate (M/s)0.150.0090.300.0190.600.038Estimate the value of the rate constant, k.
The data below were collected for the following reaction: 2NO2(g) + F2(g) → 2 NO2F(g) [NO2] (M)  [F2] (M)  Initial Rate (M/s) 0.1000.1000.0260.2000.1000.0510.2000.2000.1030.4000.4000.411Calculate the value of the rate constant, k.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)[CH3Cl] (M)[Cl2] (M)Initial Rate (M/s)0.0500.0500.0140.1000.0500.0290.1000.1000.0410.2000.2000.115Calculate the value of the rate constant, k.
The reaction2NO (g) + Cl2 (g) → 2NOCl (g)was studied at -10°C. The following results were obtained whereRate = -Δ[Cl2] / Δtb. What is the value of the rate constant?
The reaction2I- (aq) + S2O82- (aq) → I2 (aq) + 2SO42- (aq)was studied at 25°C. The following results were obtained whereb. Calculate a value for the rate constant for each experiment and an average value for the rate constant.
The decomposition of nitrosyl chloride was studied:2NOCl (g) ⇌ 2NO (g) + Cl2 (g)The following data were obtained whereb. Calculate the value of the rate constant. 
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g) CH3Cl(M)                Cl 2(M)                Initial Rate(M/s) 0.050                      0.050                         0.014 0.100                      0.050                         0.029 0.100                      0.100                         0.041 0.200                      0.200                         0.115 Calculate the value of the rate constant, k.
The rate law for the reactionCl2 (g) + CHCl3 (g) → HCl (g) + CCl4 (g)is Rate = k[Cl2]1/2[CHCl3]What are the units for k, assuming time in seconds and concentration in mol/L?
The decomposition of nitrosyl chloride was studied:2NOCl (g) ⇌ 2NO (g) + Cl2 (g)The following data were obtained wherec. Calculate the value of the rate constant when concentrations are given in moles per liter.
The reactionI - (aq) + OCl - (aq) → IO - (aq) + Cl - (aq)was studied, and the following data were obtained:b. Calculate the value of the rate constant. 
The following data were obtained for the gas‑phase decomposition of dinitrogen pentoxide,2N2O5 (g) → 4NO2 (g) + O2 (g)Defining the rate as -Δ[N2O5] / Δt, write the rate law and calculate the value of the rate constant.
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)c. Calculate the value of the rate constant. 
The following data were obtained for the reaction2ClO2 (aq) + 2OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (l)wherea. Determine the rate law and the value of the rate constant. 
You and a coworker have developed a molecule that has shown potential as cobra antivenin (AV). This antivenin works by binding to the venom (V), thereby rendering it nontoxic. This reaction can be described by the rate lawRate = k[AV]1 [V]1You have been given the following data from your coworker:[V]0 = 0.20 M[AV]0 = 1.0 x 10 -4 MA plot of ln[AV] versus t (s) gives a straight line with a slope of -0.32 s  -1. What is the value of the rate constant (k) for this reaction?
The following data have been determined for the reaction: I − + OCl− ⟶ IO− + Cl−Determine the rate equation and the rate constant for this reaction.
Alcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 25–30%. Women metabolize alcohol a little more slowly than men:Determine the rate equation, the rate constant, and the overall order for this reaction.
Under certain conditions the decomposition of ammonia on a metal surface gives the following data:Determine the rate equation, the rate constant, and the overall order for this reaction.
Nitrosyl chloride, NOCl, decomposes to NO and Cl2.2NOCl(g) ⟶ 2NO(g) + Cl2 (g)Determine the rate equation, the rate constant, and the overall order for this reaction from the following data:
From the following data, determine the rate equation, the rate constant, and the order with respect to A for the reaction A ⟶ 2C.
Nitrogen monoxide reacts with chlorine according to the equation:2NO(g) + Cl2 (g) ⟶ 2NOCl(g)The following initial rates of reaction have been observed for certain reactant concentrations:What is the rate equation that describes the rate’s dependence on the concentrations of NO and Cl2? What is the rate constant? What are the orders with respect to each reactant?
Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation:H2 (g) + 2NO(g) ⟶ N2O(g) + H2O(g) Determine the rate equation, the rate constant, and the orders with respect to each reactant from the following data:
For the reaction A ⟶ B + C, the following data were obtained at 30 °C:(b) What is the rate constant?
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2(g) → CCl4(g) + 3HCl(g)  [CH3Cl](M)                      [Cl2](M)                       Initial Rate (M/s)    0.050                              0.050                                0.014    0.100                              0.050                                0.029    0.100                              0.100                                0.041    0.200                              0.200                                0.115 a. Calculate the value of the rate constant, k? b. What is the overall order of the reaction?
For the reaction Q ⟶ W + X, the following data were obtained at 30 °C:(b) What is the rate constant?
Using the given data, calculate the rate constant of this reaction.                               A + B → C + D
You may want to reference(Pages 629 - 634) Section 14.3 while completing this problem.Consider the following reaction: CHCl3(g) + Cl2(g) → CCl4(g) + HCl(g)The initial rate of the reaction is measured at several different concentrations of the reactants with the following results:[CHCl3] (M)[Cl2] (M)Initial Rate (M/s)0.0100.0100.00340.0200.0100.00680.0200.0200.00960.0400.0400.027From the data, determine the rate constant (k) for the reaction.        
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M)Initial rate(M/s)0.127.92×10−30.161.056×10−20.201.32×10−2Write a rate law for the reaction including the value of the rate constant, k.
Consider the tabulated data showing the initial rate of a reaction (A → products) at several different concentrations of A.[A] (M)Initial Rate (M/s)0.120.0003890.180.0008750.280.00212Write a rate law for the reaction including the value of the rate constant, k.
Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 x 10-2 mol sulfuryl chloride was heated to 600. K in a 5.00 x 10 -1-L container.Defining the rate as - Δ [SO2Cl2] / Δt,a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K.
Consider this initial-rate data at a certain temperature for the reaction described by 2NOBr(g) → 2NO(g) + Br2(g) Determine the value and units of the rate constant.  
For the reaction- A + B + C → D + E the initial raction rate was measured for various initial concentrations of reactants. The follwoing data were collected: a. What is the reaction order with respect to A? b. What is the reaction order with respect to B? c. What is the reaction order with respect to C? d. What is the value of the rate constant k for this reaction? e. Given the data calculated in Parts A, B, C, and D, determine the initial rate for a reaction that starts with 0.55M of reagent A and 0.70M of reagents B and C?
Experiments were conducted to study the rate of the reaction represented by this equation.[2] 2 NO(g) + 2 H2(g) ⟶ N2(g) + 2 H2O(g) Initial concentrations and rates of reaction are given here.Consider the following questions:(d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H2 had been consumed.
The reactionI - (aq) + OCl - (aq) → IO - (aq) + Cl - (aq)was studied, and the following data were obtained:c. Calculate the initial rate for an experiment where both I  - and OCl - are initially present at 0.15 mol/L.
The reaction2NO (g) + O2 (g) → 2NO2 (g)was studied, and the following data were obtained whereWhat would be the initial rate for an experiment where [NO] 0 = 6.21 x 1018 molecules/cm3 and [O2]0 = 7.36 x 1018 molecules/cm3?
The rate of the reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20°C. The following data were collected with all concentration units in μmol/L. (A hemoglobin concentration of 2.21 μmol/L is equal to 2.21 x 10-6 mol/L.)d. What would be the initial rate for an experiment with [Hb] 0 = 3.36 μmol/L and [CO] 0 = 2.40 μmol/L?
The following data were obtained for the reaction2ClO2 (aq) + 2OH- (aq) → ClO3- (aq) + ClO2- (aq) + H2O (l)whereb. What would be the initial rate for an experiment with [ClO 2]0 = 0.175 mol/L and [OH -]0 = 0.0844 mol/L?
Consider the reactionA + 2B → Cwhose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table:a. What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].b. Calculate the initial rate for the formation of C at 25 °C. if [A] = 0. 50 M and [B] = 0. 075 M. Express your answer to two significant figures and include the appropriate units.
The rate constant for the first-order decomposition at 45 °C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCl3, is 6.2 × 10−4 min−1 . 2 N2O5 ⟶ 4 NO2 + O2What is the rate of the reaction when [N2O5] = 0.40 M?
You may want to reference (Pages 622 - 658) Chapter 14 while completing this problem.Consider the following reaction: 2O3(g) → 3O2(g). The rate law for this reaction is as follows: Rate = k[O3]2/[O2]Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?
At 473 K, for the elementary reaction 2 NOCl(g) → 2 NO(g) + Cl2(g), k1 = 7.8 x 10-2 L/mol•s and k-1 = 4.7 x 102 L2/mol2•s. A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is found to be 0.36 mol/L. Find the concentration of NO.
At 473 K, for the elementary reaction 2 NOCl(g) → 2 NO(g) + Cl2(g), k1 = 7.8 x 10-2 L/mol•s and k-1 = 4.7 x 102 L2/mol2•s. A sample of NOCl is placed in a container and heated to 473 K. When the system comes to equilibrium, [NOCl] is found to be 0.36 mol/L. Find the concentration of Cl2.
Consider the following reaction: CHCl3(g) + Cl2(g) → CCl4(g) + HCl(g). The reaction is first order in CHCl3 and one-half order in Cl2.Which of the following reaction mixtures would you expect to have the fastest initial rate?
Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces: 1532 P ⟶ 1632S + e− Rate = 4.85×10−2 day−1 [32 P]What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of 0.0033 M?
The rate constant for the radioactive decay of 14C is 1.21 × 10−4 year−1. The products of the decay are nitrogen atoms and electrons (beta particles):614C ⟶ 714N  + e−rate = k[614C]What is the instantaneous rate of production of N atoms in a sample with a carbon-14 content of 6.5 × 10−9 M?
The decomposition of acetaldehyde is a second order reaction with a rate constant of 4.71 × 10−8 L/mol/s. What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of 5.55 × 10−4 M?
The reaction A → B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of A of 0.250 M. What is the initial rate at [A] = 0.850 M?
In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.55 mol . L-1 and its rate constant (k) is 0.0014 mol . L-1 . s-1. Determine the rate of reaction if it follows a zero-order reaction mechanism. Express your answer to two significant figures and include the appropriate units.
Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer.The reaction NO + O3 ⟶ NO2 + O2 is first order with respect to both NO and O3 with a rate constant of 2.20 × 107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO] = 3.3 × 10−6 M and [O3] = 5.9 × 10−7 M?
You may want to reference (Pages 629 - 634) Section 14.3 while completing this problem.The following reaction is first order in N2O5: N2O5(g) → NO3(g) + NO2(g). The rate constant for the reaction at a certain temperature is 0.053/s.Calculate the rate of the reaction when [N2O5] = 5.6×10−2 M .
How do the rate of a reaction and its rate constant differ?
Write the rate laws for the following elementary reactions.b. O3 (g) + NO (g) → O2 (g) + NO2 (g)
Write the rate laws for the following elementary reactions.c. O3 (g) → O2 (g) + O (g)
Write the rate laws for the following elementary reactions.d. O3 (g) + O (g) → 2O2 (g)
Write the rate laws for the following elementary reactions.a. CH3NC (g) → CH3CN (g)
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.Write a rate law for the reaction.
The decomposition of many substances on the surface of a heterogeneous catalyst shows the following behavior:How do you account for the rate law changing from first order to zero order in the concentration of reactant?
Doubling the concentration of a reactant increases the rate of a reaction four times. With this knowledge, answer the following questions: (a) What is the order of the reaction with respect to that reactant?
Doubling the concentration of a reactant increases the rate of a reaction four times. With this knowledge, answer the following questions:(b) Tripling the concentration of a different reactant increases the rate of a reaction three times. What is the order of the reaction with respect to that reactant?
Tripling the concentration of a reactant increases the rate of a reaction nine times. With this knowledge, answer the following questions:(a) What is the order of the reaction with respect to that reactant?
Tripling the concentration of a reactant increases the rate of a reaction nine times. With this knowledge, answer the following questions:(b) Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant?
How much and in what direction will each of the following affect the rate of the reaction:CO(g) + NO2(g) ⟶ CO2(g) + NO(g) if the rate law for the reaction is rate = k[NO2]2?(a) Decreasing the pressure of NO2 from 0.50 atm to 0.250 atm.
How much and in what direction will each of the following affect the rate of the reaction:CO(g) + NO2(g) ⟶ CO2(g) + NO(g) if the rate law for the reaction is rate = k[NO2]2?(b) Increasing the concentration of CO from 0.01 M to 0.03 M
How will each of the following affect the rate of the reaction:CO(g) + NO2(g) ⟶ CO2(g) + NO(g) if the rate law for the reaction is rate = k[NO2][CO] ? (a) Increasing the pressure of NO2 from 0.1 atm to 0.3 atm
How will each of the following affect the rate of the reaction:CO(g) + NO2(g) ⟶ CO2(g) + NO(g) if the rate law for the reaction is rate = k[NO2][CO] ?(b) Increasing the concentration of CO from 0.02 M to 0.06 M.
Consider the following reaction: A + B + C → D. The rate law for this reaction is as follows: Rate = k[A][C]2/[B]1/2large{{ m{Rate}} = kfrac{{[{ m{A}}][{ m{C}}]^2 }}{{[{ m{B}}]^Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.16 × 10−2 M/s.What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled?
Consider a simple reaction in which a reactant A forms products: A → productsWhat is the rate law if the reaction is zero order with respect to A? First order? Second order? For each case, explain how a doubling of the concentration of A would affect the rate of reaction.
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)?
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?
You may want to reference (Pages 629 - 634) section 14.3 while completing this problem.A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C.By what factor does the reaction rate change if the concentrations of all three reactants are doubled?
A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described byO3(g) + NO(g) --> O2(g) + NO2(g)The rate law for this reaction israte of reaction = k[O3] [NO]Given that k = 4.06 x 106 M-1 s-1 at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values [O3] = 7.02 x10-6 M and [NO] = 4.89x10-5 M, owing to continuous production from separate sources.Calculate the number of moles of NO2(g) produced per hour per liter of air.
Using the giving data, calculate the rate constant of this reaction.A + B → C + D
For the reaction, A(g) + B(g) → AB(g), the rate is 0.769 mol/Ls when the initial concentrations of both A and B are 2.00 mol/L. If the reaction is first order in A and second order in B, what is the rate when the initial concentration of A = 2.18 mol/L and that of B = 3.8 mol/L Give answer to 2 decimal places. 
The data below were collected for the following reaction 2NO2 (g) + F2 (g) → 2NO2F (g) Part AWrite an expression for the reaction rate law. (i) Rate = k[NO3][F2] (ii) Rate = k[NO2] (iii) Rate = k[F2] (iv) Rate = k[NO3]2 [F2]
Phosgene is a toxic gas that is prepared by the reaction of carbon monoxide with chlorine: CO(g) + CI2(g) → COCI2(g) The data below was obtained in a kinetics study of its formation: (a). Write the rate law for the formation of phosgene. (b). Calculate the average value of the rate constant.
Consider the following elementary reaction equation.2O2 (g) + Cl (G) → ClO (g) + O3 (g)What is the order with respect to O2? What is the overall order of the reaction? Classify the reaction as unimolecular, bimolecular, or termolecular.
The data in the table below were obtained for the reaction: A + B → P The magnitude of the rate constant is _________________.
Consider the reaction A + 2B ⇌ C whose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table: Part A What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B]. rate =Calculate the initial rate for the formation of C at 25°C, if [A] = 0.50 M and [B] = 0.075 M. Express your answer to two significant figures and include the appropriate units. initial rate = 
Consider the reaction described by the following equation.C2H4Br3 (aq) + 3I- (aq) → C2H4 (g) + 2Br- (aq) + I3- (aq) The rate law is rate = k[C2H4Br2][I-] where k = 4.83 x 10-3 M-1 • s-1 What are the missing entries in the following table?
For Rate = k[A]2[B]3, determine the order with respect to reactants and determine the overall eaction order. Express your answer numerically Part 1 (1 point) Order with respect to A = Part 2 (1 point) Order with respect to B = Part 3 (1 point) Overall order =
Suppose that the following reaction is first order in [B] and second order overall. 2A + B → 2C Which of the following equations represents the rate law for this reaction? (a) d[C]/dt = k[A]2 (b) -d[B]/dt = k[A][B] (c) -(2)d[A]/dt = k[A][B] (d) (1/2)d[C]/dt = k[A]2[B]
Predict the rate law for the reaction 2BrO (g) → Br2 (g) + O2 (g) if the following conditions hold true: The rate triples when [BrO] triples. When [BrO] is halved, the rate decreases by a factor of 4.The rate is unchanged when [BrO] is tripled. 
The following data were collected for the rate of disappearance of NO in the reaction 2NO(g) + O2(g) → H2NO2(g): D. What is the rate of disappearance of NO when [NO] = 0.132 M and [O 2] = 1.78 times 10-2 M ? E. What is the rate of disappearance of O 2 at the concentrations given in part D?
Using the given data, determine the rate constant of this reaction. A + 2B → C + D
Which of the following would be a reasonable unit for the rate constant of a third order reaction? a. L3/mol3.sec b. mol2/sec.L2 c. mol3/sec.L3 d. L/mol.sec e. L2mol2.sec 
Predict the rate law for the reaction 2BrO(g) → Br2(g) + O2(g)if the following conditions hold true: The rate triples when [BrO] triples. When [BrO] is halved, the rate decreases by a factor of 4. The rate is unchanged when [BrO] is tripled.
Which trials do you use to determine n in the proposed rate law rate = k[N2]m [H2]n? a. 1 and 2 b. 1 and 3 c. 2 and 3 d. 1, 2, and 3
Consider the reaction A + 2B → Cwhose rate at 25°C was measured using three different sets of initial concentrations as listed in the following table: Part AWhat is the rate law for this reaction? Express the rate law symbolically in terms of k, [Al] and [B].
Use the rate laws given below to determine which reaction is most likely to occur in a single step. a. 2NO2 + F2 → 2NO2F           Rate = k[NO2] [F2] b. H2 + Br2 → 2HBr                  Rate = k[H2] [Br]1/2 c. NO + O2 → NO2 + O            Rate = k[NO] [O2] d. NO2 + CO → NO + CO         Rate = k[NO2]2
In the reaction 2NO2 → 2NO + O 2 given that the rate law is v = k [NO 2]2 where v is the reaction rate or reaction velocity, calculate the rate coefficient rate constant), k, for the decomposition of nitrogen dioxide for a 0.039 M solution if the instantaneous rate of reaction is 1.3 x 10-13 mol L-1 s-1. 
Consider this initial-rate data at a certain temperature for the reaction described by SO2Cl2 (g) → SO2 (g) + Cl2 (g) Determine the value and units of the rate constant.
The reactionA + B → C + Drate = k[A][B]2 has an initial rate of 0.0270 M/s.What will the initial rate be if [A]is halved and [B] is tripled?What will the initial rate be if [A]is tripled and [B] is halved?
Consider the reaction with the rate law, Rate = k{BrO3-}{Br-}{H+}2. By what factor does the rate change if the concentration of BrO3- is quadrupled and that of Br- is tripled? Just put in the number as a whole number or fraction. 
Consider this initial-rate data at a certain temperature for the reaction described by 2NOCI (g) → 2NO (g) + Cl2 (g) Determine the value and units of the rate constant.
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.
Nitrogen dioxide (NO2) reacts with ozone (O3) according to the equation: 2NO2 (g) + O3 (g) → N2O5 (g) + O2 (g) If the rate law for this reaction is rate = k[NO2] [O3], what is the overall order of the reaction? (a) zero (b) first (c) second (d) third
For a reaction A + B → products, the following data were collected. Determine the order with respect to each reactant and calculate the rate constant for this reaction. Fill in the order: rate = k[A] __________ [B] ____________rate constant, k ____________
For the reaction A + B + C → D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: What is the value of the rate constant k for this reaction? When entering compound units, indicate multiplication of units explicitly using a multiplication dot (in the menu). For example, M-1 • s-1.Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.
The data below were collected for the following reaction: CH3Cl(g) + 3Cl2 (g) → CCl4 (g) + 3HCl (g) Part A Write an expression for the reaction rate law. Part BCalculate the value of the rate constant, k. Express your answer using two significant figures. Part CWhat is the overall order of the reaction? Express your answer using two significant figures.
Using the given data, determine the rate constant of this reaction. A + 2B → C + D 
For the following of rate lawrate = k[A]xdetermine the value of x if (a) the rate double when [A] is doubled.(b) no change in rate occurs when [A] is doubled.
A certain reaction is first order in N2 and second order in H2. Use this information to complete the table below. Round each of your answers to 3 significant digits.
H2 reacts with I2 in the gas phase according to the following chemical equation: H2 (g) + I2 (g) → 2HI (g) It is observed that, when the concentration of I2 is reduced to 1/2 of its initial value, the rate of the reaction is also reduced to 1/2 of its initial value. When the concentration of H2 is multiplied by 6.46, the rate of the reaction also increases by a factor of 6.46. (a) Write the rate expression for this reaction, and give the units of the rate constant k, assuming concentration is expressed as mol L-1 and time is in seconds. (b) If [H2] were multiplied by 4.27 and [I2] by 4.63, what change in the rate would be observed? The rate would increase by a factor of __________.
For the reaction          4A(g) + 3B(g) → 2C(g) The following data were obtained at constant temperature: Pick the best expression for the rate law for the reaction: Calculate k (using the data from the table), 
Using the given data, calculate the rate constant of this reaction. A + B → C + D
What is the value of m? rate = k[N2]m [H2]n? a. 0 b. 0.5 c. 1 d. 1.5 e. 2
What is the value of n? rate = k[N2]m [H2]n? a. 0 b. 0.5 c. 1 d. 1.5 e. 2
The oxidation of nitrogen monoxide by oxygen at 25°C 2NO + O2 → 2NO2 is second order in NO and third order overall. Complete the rate law for this reaction in the box below.Use the form k[A]m[B]n. If either m or n is -1, don't enter the 1. Omit concentrations to the zero power.
Using the given data, determine the rate constant of this reaction.A + 2B → C + D 
What's the reaction order with respect to A for the reaction, A + B → C + D, which has a rate equation as: rate = k[A]x[B]y(a) x(b) y(c) xy(d) x+y(e) x-y
Using the given data, determine the rate constant of this reaction. A + 2B → C + D
The reaction A + B → C + D                                rate = k[A][B]2 has an initial rate of 0.0910 M/s. What will the initial rate be if [A] is halved and [B] is tripled? What will the initial rate be if [A] is tripled and [B] is halved?
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.
The following are initial rate data for: A + B → C (a) The rate law is: Rate = k[A][B] (b) The rate law is: Rate = k[A][B]2 (c) The rate law is: Rate = k[A]2[B] (d) The rate law is: Rate = k[A]2[B]2 (e) The rate law is: Rate = k[A]
The data below were collected for the following reaction: CH3Cl (g) + 3Cl2 (g) → CCl4 (g) + 3HCl (g) Write an expression for the reaction rate law. (i) Rate = k[CH3Cl][Cl2](ii) Rate = k[CH3Cl] [Cl2]1/2(iii) Rate = k[CH3Cl]1/2 [Cl2] (iv) Rate = k[CH3Cl]
Using the given data, calculate the rate constant of this reaction. A + B → C + D 
The reaction A + B yields C + D rate = k[A][B] 2 has an intial rate of 0.0220 M/s.a) What will the initial rate be if [A] is halved and [B] is tripled? Answer must be in M/s.b) What will the intial rate be if [A] is tripled and [B] is halved? Answer must be in M/s.
The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 4.67 x 10-10 cm3 x molecule-1 x s-1 at 298 K.Convert the rate constant to units of M -1 s-1Convert the rate constant to units of Torr -1 s-1What is the order of this reaction?
Consider this initial-rate data at a certain temperature for the reaction described by2 NOBr (g) => 2 NO (g) + Br2 (g)Determine the value and units of the rate constant k =?