The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300 K is 1 . 0 × 10 - 3 s - 1 and the activation energy E a = 11 . 488 kJ mol - 1 , the rate cons

Question

The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at $300 K$ is $1.0 \times 10^{- 3} s^{- 1}$ and the activation energy $E_{a} = 11.488 kJ {mol}^{- 1}$ , the rate constant at $200 K$ is _________ $\times 10^{- 5} s^{- 1}$ . (Round of to the Nearest Integer).

(Given $R = 8.314 J {mol}^{- 1} K^{- 1}$ )

TestHub · Accepted Answer

K 300 = 10 - 3 K 200 = ? E a = 11 . 488 KJ / mole R = 8 . 314 J / mole - K so ℓ n K 300 K 200 = E a R 1 200 - 1 300 ℓ n K 300 K 200 = 11 . 488 × 1000 × 100 8 . 314 × 200 × 300 = 2 . 303 = ℓ n 10 so K 300 K 200 = 10 K 200 = 1 10 × K 300 = 10 - 4 = 10 × 10 - 5 sec - 1

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