The rate constant for the first-order decomposition at `45^@C` of `N_2O_5`, dissolved in chloroform, is `6.2 xx 10^(-4) "min"^(-1). 2N_2O_5 to 4NO_2 +O_2`
(a) What is the rate of decomposition when `[N_2O_5]` = 0.40 M?
(b) What are the rates of formation of `NO_2` and of `O_2` when `[N_2O_5]` = 0.40 M?

Explanation

To solve the problem step by step, we will break it down into parts (a) and (b) as requested.

### (a) What is the rate of decomposition when [N2O5] = 0.40 M?

1. **Identify the rate law for a first-order reaction**: For a first-order reaction, the rate of decomposition can be expressed as:
\[ \text{Rate} = k \times [N_2O_5] \]
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