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 decomposition of N2O5 can be described by the equation2N2O5 → 4NO2 + O2Given these data for the reaction at 45 °C in carbon tetrachloride solution, calculate the average rate of reaction for each

Solution: The decomposition of N2O5 can be described by the equation2N2O5 → 4NO2 + O2Given these data for the reaction at 45 °C in carbon tetrachloride solution, calculate the average rate of reaction for each

Problem

The decomposition of N2O5 can be described by the equation

2N2O→ 4NO+ O2

Given these data for the reaction at 45 °C in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval.

t(s)       [N2O5]

0             2.04

135         1.87

536         1.46

795          1.24

i) Reaction rate from 0-135 is ?

ii) Reaction rate from 135-536 is ?

iii) Reaction rate from 536-795 is ?

Solution

Average rate = Δ[ N2O5 ] / 2Δt

Because we lose reactants and gain products, we are losing [N2O5], and our equation becomes: 

Average rate = - Δ[ N2O5 ] / 2Δt     

Also, remember that ΔN2O5 ]  and Δt = final - initial, and that whatever the coefficient we have for the reactant, we will put that number on the bottom!

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