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 this reaction at `(N_2O_5)`=0.4M

Explanation

To find the rate of the reaction for the first-order decomposition of \( N_2O_5 \) at a concentration of 0.4 M, we can follow these steps:

### Step 1: Identify the order of the reaction
The reaction is given as a first-order decomposition of \( N_2O_5 \). This means that the rate of the reaction depends linearly on the concentration of \( N_2O_5 \).

### Step 2: Write the rate equation
For a first-order reaction, the rate equation can be expressed as:
\[
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