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The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production - Chemistry

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The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N2 and H2 if = 2.5 × 10−4 mol−1 L s−1?

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Solution

The decomposition of NH3 on platinum surface is represented by the following equation.

Therefore

`Rate = -1/2 (d[NH_3])/dt = (d[N_2])/dt = 1/3(d[H_2])/dt`

However, it is given that the reaction is of zero order.

Therefore,

`-1/2 (d[NH_3])/dt = (d[N_2])/dt = 1/3 (d[H_2])/dt = k` 

= 2.5 x 10-4 mol L-1 s-1

Therefore, the rate of production of N2 is

`(d[N_2])/dt = 2.5xx10^(-4) mol L^(-1) s^(-1)`

 And, the rate of production of H2 is

`(d[H_2])/dt = 3 x 2.5 xx 10^(-4) mol L^(-1) s^(-1)`

= 7.5 × 10−4 mol L−1 s−1

Concept: Integrated Rate Equations - Zero Order Reactions
  Is there an error in this question or solution?

APPEARS IN

NCERT Class 12 Chemistry
Chapter 4 Chemical Kinetics
Q 3 | Page 117
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