Question

\( 2N_2O_5 \to 4NO_2 + O_2 \) If rate and rate constant for above reaction are \( 2.40 \times 10^{-5} \, \text{mol L}^{-1} \text{s}^{-1} \) and \( 3 \times 10^{-5} \, \text{s}^{-1} \), respectively, then calculate the concentration of \( N_2O_5 \):

• A. 14
• B. 1.2
• C. 0.04
• D. 0.8

Hint:

Use the rate law to calculate concentration by dividing the rate by the rate constant.

Answer 1

The Correct Option is C

Step 1: Use rate equation.
From the rate law, the rate of the reaction is related to the concentration of \( N_2O_5 \): \[ \text{Rate} = k [N_2O_5] \] Substituting the given values for rate and rate constant, we find that the concentration of \( N_2O_5 \) is 0.04 M.
Thus, the correct answer is (3).