Chemical Kinetics and Nuclear ChemistryHard

Question

For the reaction 2N2O5(g) → 4NO2(g) + O2(g), the concentration of NO2 increases by 2.4 × 10−2 M in 6 s. What will be the average rate of appearance of NO2 and the average rate of disappearance of N2O5?

Options

A.2 × 10−3 Ms−1, 4 × 10−3 Ms−1
B.2 × 10−3 Ms−1, 1 × 10−3 Ms−1
C.2 × 10 Ms−1, 2 × 10−3 Ms−1
D.4 × 10−3 Ms−1, 2 × 10−3 Ms−1

Solution

$r_{av,NO_{2}} = \frac{2.4 \times 10^{- 2}}{6} = 4 \times 10^{- 3}\text{ M}\text{s}^{- 1}$

and, $\frac{r_{N_{2}O_{5}}}{2} = \frac{r_{NO_{2}}}{4} \Rightarrow r_{N_{2}O_{2}} = 2 \times 10^{- 3}\text{M}\text{s}^{- 1}$

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