The rate constant for the first order decomposition of `N_(2)O_(5)` dissolved in chloroform at `45^(@)C` is `3.1 xx10^(-4)min^(-1)`
`2N_(2)O_(5)to 4NO_(2)+O_(2)`
What is the rate of decomposition of `N_(2)O_(5)` when `[N_(2)O_(5)] =0.40 `M ?

Explanation

To solve the problem, we need to determine the rate of decomposition of \( N_2O_5 \) when its concentration is \( 0.40 \, M \). Given that the decomposition of \( N_2O_5 \) is a first-order reaction, we can use the following relationship:

### Step 1: Write the rate law for the reaction
For a first-order reaction, the rate law can be expressed as:
\[ \text{Rate} = k [N_2O_5] \]
where:
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