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

Solution: The following kinetic data are collected for the initial rates of a reaction 2X + Z →products:Experiment  [X]0  (M)  [Z]0  (M)  Rate  (M/s) 10.250.254.0x101imes {10^{1}}20.500.503.2x102imes {10^{2}}30

Solution: The following kinetic data are collected for the initial rates of a reaction 2X + Z →products:Experiment  [X]0  (M)  [Z]0  (M)  Rate  (M/s) 10.250.254.0x101imes {10^{1}}20.500.503.2x102imes {10^{2}}30

Problem

The following kinetic data are collected for the initial rates of a reaction 2X + Z →products:


Experiment  [X]0  (M)  [Z]0  (M)  Rate  (M/s
10.250.254.0x101
20.500.503.2x102
30.500.757.2x102



What is the value of the rate constant with proper units?

Solution

Recall that the Rate Law (which considers reactants only) for the reaction: 

2X + Z → products is given by the equation:

Where:

k = rate law constant

a, b = reactant orders

X and Z = reactants

Based on the given experimental data, we can determine the rate constant, k by these steps:

  1. Solve reactant orders: a and b 
  2. Solve for the value of k 
  3. Determine correct units for k 
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