For the first order reaction C 2 H 5 I ( g ) → C 2 H 4 ( g ) + HI ( g ) ; Δ r U = − 20.53 kcal / mole The rate constants of the forward reaction at 600 K and 700 K are 2 × 1 0 − 5 s − 1 and

Question

For the first order reaction C 2 ​ H 5 ​ I ( g ) → C 2 ​ H 4 ​ ( g ) + HI ( g ) ; Δ r ​ U = − 20.53 kcal / mole The rate constants of the forward reaction at 600 K and 700 K are 2 × 1 0 − 5 s − 1 and 6.4 × 1 0 − 4 s − 1 respectively. Find the activation energy of the backward reaction in k c a l / m o l e . ( ln 2 = 0.7 )

TestHub · Accepted Answer

ln k 1 ​ k 2 ​ ​ = R E a f ​ ​ ​ ( T 1 ​ 1 ​ − T 2 ​ 1 ​ ) ln 32 = 2 E a f ​ ​ ​ ( 600 1 ​ − 700 1 ​ ) E a f ​ ​ = 5 × 0.7 × 2 × 600 × 7 = 29400 c a l Δ r ​ H = E a f ​ ​ − E a b ​ ​ − 20.53 = 29.4 − E a b ​ ​ E a b ​ ​ = 49.93 k c a l / m o l e

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