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(A) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.$1$. The rate law for this reaction is: $	ext{

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Rate of the reaction depends on concentration of $NH_3$

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(A) For a zero order reaction,the rate of reaction is independent of the concentration of the reactant.$1$. The rate law for this reaction is: $	ext{Rate} = k[NH_3]^0 = k$.$2$. Since the rate is equal to the rate constant $(k)$,option $B$ is true.$3$. At high pressure,the catalyst surface is fully saturated with $NH_3$ molecules. Therefore,increasing the pressure further does not increase the rate of reaction,making option $C$ true.$4$. Since the rate is constant,the rate of decomposition of ammonia remains constant,making option $D$ true.$5$. Option $A$ states that the rate depends on the concentration of $NH_3$,which is false for a zero order reaction. Thus,option $A$ is the correct answer.

At high pressure,the following reaction is zero order:
$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$
Choose the option which is not true with respect to the reaction,from the choices given below:

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At high pressure,the following reaction is zero order:$2NH_{3(g)} \xrightarrow[Pt \ \text{catalyst}]{1130 \ K} N_{2(g)} + 3H_{2(g)}$Choose the option which is not true with respect to the reaction,from the choices given below: