The reaction, `2N_(2)O_(s)(g)iff4NO_(2)(g)+O_(2)(g)` was studied in a closed vessel It was found that the concentration of `NO_(2)` increases by `2*0xx10^(-2)"mol "L^(-1)` in five seconds. Calculate
(i) the rate of reaction (ii) the rate of change of concentration of `N_(2)O_(5)`.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Understand the Reaction
The given reaction is:
\[ 2N_2O \rightleftharpoons 4NO_2 + O_2 \]

### Step 2: Calculate the Rate of Reaction
The rate of reaction can be calculated using the change in concentration of the products. The concentration of \( NO_2 \) increases by \( 2.0 \times 10^{-2} \, \text{mol L}^{-1} \) in 5 seconds.
...