1
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
$$0.095 \mathrm{~mol} \mathrm{~s}^{-1}$$
2
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
$$t_{1 / 2}=\frac{[\mathrm{A}]_1-[\mathrm{A}]_0}{k}$$
3
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
$$\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}_2\right]}{\left[\mathrm{H}_2 \mathrm{O}_2\right]\left[\mathrm{O}_2\right]^{1 / 2}}$$
4
MHT CET 2021 24th September Morning Shift
+1
-0

A reaction is first order with respective to $$\mathrm{A}$$ and second order with respective to $$\mathrm{B}$$. What is the effect on reaction rate if concentration of B is increased 3 times?

A
Rate increases 6 times
B
Rate increases 2 times
C
Rate increases 9 times
D
Rate increases 3 times
EXAM MAP
Medical
NEET