The first order rate constant for the decomposition of ethyl iodide by the reaction: C 2 H 5 I (g) → C 2 H 4 (g) + HI(g) at 600K is 1.60 × 10 –5 s –1 . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 7

Question

The first order rate constant for the decomposition of ethyl iodide by the reaction: C 2 H 5 I (g) → C 2 H 4 (g) + HI(g) at 600K is 1.60 × 10 –5 s –1 . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700K.

Quantrex Academy · Accepted Answer

Correct answer: D. 6.36 × 10 –3 s –1

Correct Option is : (D) 6.36 × 10 –3 s –1

The first order rate constant for the decomposition of ethyl iodide by the reaction: C 2 H 5 I (g) → C 2 H 4 (g) + HI(g) at 600K is 1.60 × 10 –5 s –1 . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700K.

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