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

**N _{2}O → N_{2} + 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**E _{a}** = activation energy (in J/mol)

What is the rate constant for the reaction N_{2}O → N_{2} + O if the reaction occurs at room temperature (T = 25°C) with a pre-exponential factor of 8:0 x 10^{12} 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 10^{9}

5. 3.21 x 10^{8}

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