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**Problem**: The gas-phase reaction of NO with F2 to form NOF and F has an activation energy of Ea = 6.3 kj/mol and a frequency factor of A = 6.0 x 108 M-1 s - 1. The reaction is believed to be bimolecular:NO(g) + F2 (g) → NOF (g) + F(g).Calculate the rate constant at 106 oC.

###### FREE Expert Solution

We will use the following equation to solve this problem:

$\overline{){\mathbf{ln}}{\mathbf{}}{\mathbf{k}}{\mathbf{=}}{\mathbf{-}}\frac{{\mathbf{E}}_{\mathbf{a}}}{\mathbf{R}}{\mathbf{}}\left(\frac{\mathbf{1}}{\mathbf{T}}\right){\mathbf{}}{\mathbf{+}}{\mathbf{}}{\mathbf{ln}}{\mathbf{}}{\mathbf{A}}}$

where:

**k** = rate constant

**E _{a}** = activation energy (in J/mol)

**R** = gas constant (8.314 J/mol • K)

**T** = temperature (in K)

**A** = Arrhenius constant or frequency factor

###### Problem Details

The gas-phase reaction of NO with F_{2} to form NOF and F has an activation energy of E_{a} = 6.3 kj/mol and a frequency factor of A = 6.0 x 10^{8} M^{-1} s^{ - 1}. The reaction is believed to be bimolecular:

NO(g) + F_{2} (g) → NOF (g) + F(g).

Calculate the rate constant at 106 ^{o}C.

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