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

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

Aicharya · Accepted Answer

K 300 = 10 - 3 &#160;&#160; &#160; K 200 = ? E a = 11 . 488 KJ / mole &#160;&#160; R = 8 . 314 &#160; J / mole - K so &#8467; n K 300 &#160; K 200 = E a R 1 200 - 1 300 &#8467; n K 300 &#160; K 200 = 11 . 488 &#215; 1000 &#215; 100 8 . 314 &#215; 200 &#215; 300 = 2 . 303 = &#8467; n 10 so K 300 &#160; K 200 = 10 K 200 = 1 10 &#215; K 300 = 10 - 4 = 10 &#215; 10 - 5 &#160; sec - 1

The decomposition of formic acid on gold surface follows first order kinetics. If the rate constant at 300…

Solution