Then decomposition of formic acid on Gold surface follows first order kinetics if the rate costant at 300K is1.0x10 $^{- 3}$ S $^{- 1}$ and the activation energy E $_{a}$ =11.488KJ ${mol}^{- 1}$ If the rate constant at 200 K is………... $\times 10^{- 5} s^{- 1}$ (Round off to the Nearest Integer).

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Detailed Solution

$\begin{array}{l} T_{1} = 200, T_{2} = 300 \\ K_{1} = ? K_{2} = 10^{- 3} \\ \log (\frac{10^{- 3}}{K_{1}}) = \frac{11.488 \times 10^{3}}{2.303 \times 8.314} (\frac{1}{200} - \frac{1}{300}) \end{array}$

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