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

The decomposition of N2O5 can be described by the equation.

2N2O5 (soln) →  4NO2 (soln) + O2 (g)

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

t(s)                [N2O5] (M)

0                    2.10

195                1.86

556                1.48

825                1.25

i) Interval: 0 s to 195 s

Reaction rate= _____M/s

ii) Interval: 195 s to 556 s

Reaction rate= _____M/s

iii) Interval: 556 s to 825 s

Reaction rate= _____M/s


$Average \ rate = \frac {Δ[ \ ]}{Δt}$

Because we lose reactants and gain products, we are losing $[N_2O_2]$, and our equation becomes: $Average \ rate = \frac{-Δ[ \ ]}{Δt}= \frac{-Δ[N_2O_2 ]}{Δt}$ Also, remember that $Δ= final - initial$, and that whatever the coefficient we have for the reactant, we will put that number on the bottom!

Solution BlurView Complete Written Solution