Consider the reaction A → 2 B + C , Δ H = − 15 kcal . The energy of activation of backward reaction is 20 kcal mol − 1 . In presence of catalyst, the energy of activation of forward reaction is 3 kcal

Question

Consider the reaction A → 2 B + C , Δ H = − 15 kcal . The energy of activation of backward reaction is 20 kcal mol − 1 . In presence of catalyst, the energy of activation of forward reaction is 3 kcal mol − 1 . At 400 K the catalyst causes the rate of the forward reaction to increase by the number of times equal to

TestHub · Accepted Answer

Given: A → 2 B + C , Δ H = − 15 k c a l m o l − 1 E a ​ ( ba c k w a r d ) = 20 k c a l m o l − 1 For an exothermic reaction: E a ​ ( f or w a r d ) = E a ​ ( ba c k w a r d ) + Δ H = 20 − 15 = 5 k c a l m o l − 1 With catalyst, E a ​ = 3 k c a l m o l − 1 . Using the Arrhenius equation: k u ​ k c ​ ​ = e 2 × 400 ( 5 − 3 ) × 1000 ​ = e 2.5 The ratio is e 2.5 .

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