We’re being asked to **determine the frequency factor (A)** of a reaction given that the plot of ln k vs. 1/T has a **slope of −1.5275 × 10 ^{4}** and an

We’re given the plot of ln k (y) vs. 1/T (x).

This means we need to use the ** two-point form of the Arrhenius Equation**:

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

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

A series of experiments were performed to determine the rate constant for the reaction

2H_{2}S(g) + 3O_{2}(g) → 2H_{2}O(g) + 2SO_{2}(g)

at different temperatures. A plot of *ln *k against 1/T was a straight line with a slope of −1.5275x10^{4} and intercept of 23.6. What is the frequency factor?

a) 196.2

b) 23.6

c) 1.5275x10^{4}

d) 5.63x10^{−11}

e) 1.78x10^{10}

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