1
MHT CET 2021 24th September Evening Shift
+1
-0

In a first reaction 60% of reactant decomposes in 4.606 min. What is half life of reaction? (k = 0.1989 min$$^{-1}$$)

A
3.48 min
B
2.4 min
C
3.0 min
D
1.74 min
2
MHT CET 2021 24th September Evening Shift
+1
-0

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 $$\mathrm{B}$$ ?

A
$$0.076 \mathrm{~mol} \mathrm{~s}^{-1}$$
B
$$0.038 \mathrm{~mol} \mathrm{~s}^{-1}$$
C
$$0.019 \mathrm{~mol} \mathrm{~s}^{-1}$$
D
$$0.095 \mathrm{~mol} \mathrm{~s}^{-1}$$
3
MHT CET 2021 24th September Evening Shift
+1
-0

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

A
$$t_{1 / 2}=\frac{k}{0.693}$$
B
$$k=\frac{[A]_0-[A]_1}{t_{1 / 2}}$$
C
$$t_{1 / 2}=\frac{0.693}{k}$$
D
$$t_{1 / 2}=\frac{[\mathrm{A}]_1-[\mathrm{A}]_0}{k}$$
4
MHT CET 2021 24th September Morning Shift
+1
-0

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

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