Problem: What is the rate constant for the reaction N2O → N2 + O if the reaction occurs at room temperature (T = 25°C) with a pre-exponential factor of 8:0 x 1012 s-1 and an activation energy of 250 kJ/mol.1. 1.27 x 10-312. 1.62 x 10-303. 7.23 x 10104. 9.07 x 1095. 3.21 x 108

FREE Expert Solution

We’re being asked to determine the rate constant for the reaction if the reaction occurs at room temperature (T = 25°C).

N2O → N2 + O

To calculate the rate constant, we will use the Arrhenius Equation:

$\overline{){\mathbf{k}}{\mathbf{=}}{{\mathbf{Ae}}}^{\mathbf{-}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{RT}}}}$

where k = rate constant
A = pre-exponential factor
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
= temperature (in K)

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Problem Details

What is the rate constant for the reaction N2O → N2 + O if the reaction occurs at room temperature (T = 25°C) with a pre-exponential factor of 8:0 x 1012 s-1 and an activation energy of 250 kJ/mol.

1. 1.27 x 10-31

2. 1.62 x 10-30

3. 7.23 x 1010

4. 9.07 x 109

5. 3.21 x 108