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 \( N_2O_5 \):
\( 2N_2O_5 \to 4NO_2 + O_2 \)
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 \( N_2O_5 \):
Show Hint
Use the rate law to calculate concentration by dividing the rate by the rate constant.
Updated On: Mar 25, 2026
- 14
- 1.2
- 0.04
- 0.8
Show Solution
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The Correct Option is C
Solution and Explanation
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).
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