MHT CET 2021 24th September Evening Shift | Chemical Kinetics Question 131 | Chemistry

For the reaction, $$2 \mathrm{~A}+\mathrm{B} \rightarrow 2 \mathrm{C}$$, rate of disappearance of $$\mathrm{A}$$ is $$0.076 \mathrm{~mol} \mathrm{~s}^{-1}$$. What is the rate of disappearance of $$\mathrm{B}$$ ?

$$0.076 \mathrm{~mol} \mathrm{~s}^{-1}$$

$$0.038 \mathrm{~mol} \mathrm{~s}^{-1}$$

$$0.019 \mathrm{~mol} \mathrm{~s}^{-1}$$

$$0.095 \mathrm{~mol} \mathrm{~s}^{-1}$$

MHT CET 2021 24th September Evening Shift

MCQ (Single Correct Answer)

-0

Half-life and rate constant for first order reaction are related by equation,

$$ t_{1 / 2}=\frac{k}{0.693} $$

$$ k=\frac{[A]_0-[A]_1}{t_{1 / 2}} $$

$$ t_{1 / 2}=\frac{0.693}{k} $$

$$ t_{1 / 2}=\frac{[\mathrm{A}]_1-[\mathrm{A}]_0}{k} $$

MHT CET 2021 24th September Morning Shift

MCQ (Single Correct Answer)

-0

If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

$$\mathrm{r}=\frac{\mathrm{k}}{\left[\mathrm{H}_2 \mathrm{O}_2\right]}$$

$$\mathrm{r}=\mathrm{k}\left[\mathrm{H}_2 \mathrm{O}_2\right]$$

$$\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}\right]\left[\mathrm{O}_2\right]^{1 / 2}}{\left[\mathrm{H}_2 \mathrm{O}_2\right]}$$

$$\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}_2\right]}{\left[\mathrm{H}_2 \mathrm{O}_2\right]\left[\mathrm{O}_2\right]^{1 / 2}}$$

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