The reaction `2N_(2)O_(5)(g) to 2N_(2)O_(4)(g)+O_(2)(g)` obeys the rate law , rate =`k[N_(2)O_(5)]` where `k=0.0084 s^(-1)`
If `2.50` moles of `N_(2)O_(5)` were taken in a `5.0` -litre flask , how many moles of `N_(2)O_(4)` would remain after 60 seconds ?

Explanation

To solve the problem step by step, we need to determine how many moles of \( N_2O_4 \) will remain after 60 seconds when starting with 2.50 moles of \( N_2O_5 \) in a 5.0-litre flask.

### Step 1: Calculate the initial concentration of \( N_2O_5 \)

The concentration \( C \) is calculated using the formula:
\[ C = \frac{\text{moles}}{\text{volume (L)}} \]
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