`4NH_3 + 5O_2 to 4NO + 6H_2O`. If rate of formation of NO is `6 xx 10^(−4) "atm min"^(-1)`, calculate the rate of formation of `H_2O`.

Explanation

To solve the problem, we need to relate the rate of formation of \( \text{H}_2\text{O} \) to the rate of formation of \( \text{NO} \) based on the stoichiometry of the given reaction:

\[ 4 \text{NH}_3 + 5 \text{O}_2 \rightarrow 4 \text{NO} + 6 \text{H}_2\text{O} \]

### Step-by-Step Solution:

1. **Identify the Stoichiometric Coefficients:**
From the balanced equation, we see that:
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