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The decomposition of N2O5 in CCl4 follows 2N2O5 -> 4NO2 + O2. Its concentration falls from 2.33 mol L^-1 to 2.08 mol L^-1 in 184 minutes. What is the average rate of reaction in mol L^-1 min^-1?
A6.79 x 10^-4
B1.36 x 10^-3
C2.72 x 10^-3
D3.40 x 10^-4
Answer & Solution
Correct answer: A. 6.79 x 10^-4
1. Rate $= -\dfrac{1}{2}\dfrac{\Delta[N_2O_5]}{\Delta t}$.
2. $\Delta[N_2O_5] = 2.08 - 2.33 = -0.25\ \text{mol L}^{-1}$ over $184\ \text{min}$.
3. Rate $= -\dfrac{1}{2}\times\dfrac{-0.25}{184} = \dfrac{0.25}{368}$.
4. $= 6.79\times10^{-4}\ \text{mol L}^{-1}\text{min}^{-1}$.
5. Distractor B omits the 1/2 factor; distractor C is the NO2 rate, not the reaction rate.
_Source: NCERT Class 12 Chemistry Ch 3 "Chemical Kinetics", p.5_
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