A gaseous reaction `A_(2)(g) rarr B(g) + (1)/(2) C(g)` shows increase in pressure form `100 mm` to `120 mm` in `5 min`. What is the rate of disappearance of `A_(2)` ?

Explanation

To solve the problem, we need to determine the rate of disappearance of \( A_2 \) in the reaction:

\[ A_2(g) \rightarrow B(g) + \frac{1}{2}C(g) \]

Given that the pressure increases from \( 100 \, \text{mm} \) to \( 120 \, \text{mm} \) in \( 5 \, \text{minutes} \), we can follow these steps:

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