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.

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FREE Expert 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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Problem Details

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.


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