The decomposition of `NH_3` on platinum surface is a zero order reaction. What would be the rate of production of `N_2 and H_2` if `k=2.5xx10^(-4) "mol L"^(-1) s^(-1)` ?

Explanation

To solve the problem regarding the decomposition of ammonia (NH₃) on a platinum surface as a zero-order reaction, we will follow these steps:

### Step 1: Write the balanced chemical equation
The decomposition of ammonia can be represented by the following balanced equation:
\[ 2 \text{NH}_3 \rightarrow \text{N}_2 + 3 \text{H}_2 \]

### Step 2: Identify the rate constant and its significance
We are given that the rate constant \( k = 2.5 \times 10^{-4} \, \text{mol L}^{-1} \text{s}^{-1} \). In a zero-order reaction, the rate of reaction is constant and independent of the concentration of the reactants.
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