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Chemical Kinetics question bank (Chemistry)

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Q1.

The decomposition of $\text{N}_2\text{O}_{5(g)}$ occurs as: $2\ \text{N}_2\text{O}_{5(g)} \rightarrow 4\ \text{NO}_{2(g)} + \text{O}_{2(g)}$.
If initial concentration of $\text{N}_2\text{O}_{5(g)}$ is $1.63 \times 10^{-2}\ \text{mol L}^{-1}$ and after $400$ seconds it is $1.36 \times 10^{-2}\ \text{mol L}^{-1}$, calculate the rate of reaction.

(A)

$3.38 \times 10^{-6}\ \text{mol L}^{-1}\ \text{s}^{-1}$

(B)

$2.25 \times 10^{-6}\ \text{mol L}^{-1}\ \text{s}^{-1}$

(C)

$1.78 \times 10^{-6}\ \text{mol L}^{-1}\ \text{s}^{-1}$

(D)

$3.0 \times 10^{-6}\ \text{mol L}^{-1}\ \text{s}^{-1}$

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Q2.

For a first order reaction, (A) $\rightarrow$ Products, the concentration of A changes from $0.1$ M to $0.025$ M in $40$ minutes. The rate of reaction when the concentration of A is $0.01$ M is

(A)

$3.47 \times 10^{-4}$ M/min

(B)

$3.47 \times 10^{-5}$ M/min

(C)

$1.73 \times 10^{-4}$ M/min

(D)

$1.73 \times 10^{-5}$ M/min

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