# 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.

###### FREE Expert Solution
86% (465 ratings)
###### 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).

86% (465 ratings)
###### 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?

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Arrhenius Equation concept. You can view video lessons to learn Arrhenius Equation. Or if you need more Arrhenius Equation practice, you can also practice Arrhenius Equation practice problems.

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Based on our data, we think this problem is relevant for Professor Donat's class at ODU.