Chemical Kinetics and Nuclear ChemistryMedium

Question

Azomethane(CH3NNCH3) decomposes according to the following equation.

CH3−N ≡ N−CH3(g) → C2H6(g) + N2(g)

The initial concentration of azomethane was 1.50 × 10−2 M. After 10 minutes, the concentration was decreased to 1.29 × 10−2 M. The average rate of reaction during this time interval is

Options

A.3.5 × 10−6 Ms−1
B.2.1 × 10−4 Ms−1
C.3.5 × 10−6 Mh−1
D.2.1 × 10−3 Mmin−1

Solution

$r_{av} = - \frac{\Delta C}{\Delta t} = \frac{- \left( 1.29 \times 10^{- 2} - 1.50 \times 10^{- 2} \right)}{10}$

$= 2.1 \times 10^{- 4}\text{ M mi}\text{n}^{- 1} $$$= \frac{2.1 \times 10^{- 4}}{60} = 3.5 \times 10^{- 6}\text{ M}\text{s}^{- 1}$$

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