For the decomposition,
`N_(2)O_(5)(g) rarr N_(2)O_(4)(g) + 1//2O_(2)(g)`, the initial pressure of `N_(2)O_(5)` is `114 mm` and after `20 sec`, the pressure of reaction mixture becomes `133 mm`.
Calculate the rate of reaction in terms of :
(a) change in pressure `sec^(-1)` and
(b) change in molarity `sec^(-1)`. Given that reaction is carried out at `127^(@)C`.

Explanation

To solve the problem, we need to calculate the rate of reaction for the decomposition of \( N_2O_5 \) in two ways: in terms of change in pressure and change in molarity.

### Given Data:
- Initial pressure of \( N_2O_5 \) = \( P_0 = 114 \, \text{mm} \)
- Final pressure after 20 seconds = \( P_t = 133 \, \text{mm} \)
- Time, \( t = 20 \, \text{s} \)

### Step 1: Calculate the change in pressure
...