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: Rate constants for the reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) are 1.3 M -1 s-1 at 700 K and 23.0 M -1 s-1 at 800 K. a) What is the value of the activation energy in kJ/mol? b) What is the rate c

Solution: Rate constants for the reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) are 1.3 M -1 s-1 at 700 K and 23.0 M -1 s-1 at 800 K. a) What is the value of the activation energy in kJ/mol? b) What is the rate c

Problem

Rate constants for the reaction 

NO2 (g) + CO (g) → NO (g) + CO2 (g) 

are 1.3 M -1 s-1 at 700 K and 23.0 M -1 s-1 at 800 K. 

a) What is the value of the activation energy in kJ/mol? 

b) What is the rate constant at 730 K? 

Express your answer using two significant figures.


Solution

For the first part of the problem, we’re being asked to determine the activation energy (Ea) of the reaction. 

We’re given the rate constants at two different temperatures. 


This means we need to use the two-point form of the Arrhenius Equation:



where:

k1 = rate constant at T

k2 = rate constant at T

Ea = activation energy (in J/mol) 

R = gas constant (8.314 J/mol•K) 

T1 and T2 = temperature (in K).


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