If the decomposition of nitrogen oxide as `2N_2O_5 to 4NO_2 + O_2` follows a first order kinetics. K=3.0 × 10^(-5) sec^(-1) .
What concentration of `N_2O_5` would give a rate of `2.45 xx 10^(−5) "mol L"^(-1) s^(-1)` ?

Explanation

To solve the problem, we need to find the concentration of \( N_2O_5 \) that would give a specified rate of reaction, given that the decomposition of \( N_2O_5 \) follows first-order kinetics.

### Step-by-Step Solution:

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