Chemistry - Chemical Kinetics Question with Solution | TestHub

The decomposition of ammonia gas on a hot platinum surface is a zero-order reaction at high pressure.

For a zero-order reaction, the rate law is given by Rate = $k[{\text{NH}}_3{]}^0=k$.

Since the rate is equal to the rate constant $k$, the rate of reaction is independent of the concentration of ammonia, and the unit of the rate constant is the same as the unit of the rate of reaction.

The half-life period for a zero-order reaction is given by $t_{1/2}=\frac{[\text{A}{]}_0}{2k}$.

Thus, the half-life period is directly proportional to the initial concentration of ammonia, not independent of it.

Therefore, the statement that the half-life period is independent of the initial concentration is incorrect.

Answer: Half life period of reaction is independent of the initial concentration of ammonia