Chemical kinetic question doubt

Please explain how option (d) is the answer and not option (b)?

  1. The rate of formation of ammonia by the reaction: N_{2} + 3H_{2} → 2NH_{3} expressed as (d[NH_{3}])/(dt) = 2.5 * 10 ^ 4 * mol * I ^ 1 * s ^ - 1

The rate of consumption expressed in terms of H_{2} as (- d * [H_{2}])/(dt) will be

a) Double

b) Three times

c) Same

d) One and a half time of that expressed in terms of N*H_{3}


You can write 3/2 as one and a half time

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Thank you for the solution