The rate for the decomposition of `NH_(3)` on platinum surface is zero order. What are the rate of production of `N_(2)` and `H_(2)` if `K = 2.5 xx 10^(-4) "mol litre"^(-1)s^(-1)`?

Explanation

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

### Step 1: Write the balanced chemical equation for the decomposition of NH₃.
The decomposition of ammonia can be represented as:
\[ 2 \text{NH}_3 \rightarrow \text{N}_2 + 3 \text{H}_2 \]

### Step 2: Identify the order of the reaction and the rate constant.
The problem states that the reaction is zero-order with respect to NH₃, and the rate constant \( K \) is given as:
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