A B (first reaction) C D (second reaction) Consider the above two first-order reactions. The rate constant for first reaction at 500 K is double of the same at 300 K. At 500 K, 50% of the reaction bec

Question

A B (first reaction) C D (second reaction) Consider the above two first-order reactions. The rate constant for first reaction at 500 K is double of the same at 300 K. At 500 K, 50% of the reaction becomes complete in 2 hour. The activation energy of the second reaction is half of that of first reaction. If the rate constant at 500 K of the second reaction becomes double of the rate constant of first reaction at the same temperature; then rate constant for the second reaction at 300 K is _______ × 10 –1 hour –1 (nearest integer).

Prashant Kotian · Accepted Answer

Correct answer: .. For A K  B ln(2) = a E 1 R 500        a ln2 R 1500 E    2 a a E ln2 R 1500 E 4     (K1)at 500 K = ln2 (K2)at 500 K = ln2 Now for C K  D 2 at 500K 2 at 300K (K ) ln2 R 1500 1 ln (K ) R 500                           (K2)at 300 K = ln2 = 0.49 (K2)at 300 K = 4.9 × 10 –1 Ans is 5.

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