1
MHT CET 2021 24th September Morning Shift
MCQ (Single Correct Answer)
+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
$$\mathrm{r}=\mathrm{k} \frac{\left[\mathrm{H}_2 \mathrm{O}_2\right]}{\left[\mathrm{H}_2 \mathrm{O}_2\right]\left[\mathrm{O}_2\right]^{1 / 2}}$$
2
MHT CET 2021 24th September Morning Shift
MCQ (Single Correct Answer)
+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
3
MHT CET 2021 24th September Morning Shift
MCQ (Single Correct Answer)
+1
-0

For the reaction $$\mathrm{A}+\mathrm{B} \rightarrow$$ product, rate of reaction is $$3.6 \times 10^{-2} \mathrm{mol~dm}^{-3} \mathrm{sec}^{-1}$$. When $$[\mathrm{A}]=0.2 \mathrm{~mol} \mathrm{dm}^{-3}$$ and $$[\mathrm{B}]=0.1 \mathrm{~mol} \mathrm{~dm}^{-3}$$, find rate constant of reaction if it is second order with respective to both reactants.

A
$$18 \mathrm{~mol}^{-3} \mathrm{dm}^9 \mathrm{sec}^{-1}$$
B
$$90 \mathrm{~mol}^{-3} \mathrm{dm}^9 \mathrm{sec}^{-1}$$
C
$$72 \mathrm{~mol}^{-3} \mathrm{dm}^9 \mathrm{sec}^{-1}$$
D
$$36 \mathrm{~mol}^{-3} \mathrm{~dm}^9 \mathrm{sec}^{-1}$$
4
MHT CET 2021 23rd September Evening Shift
MCQ (Single Correct Answer)
+1
-0

Which of the following equations represents integrated rate law for zero order reaction?

A
$$k=\frac{[\mathrm{A}]_{\mathrm{t}}-[\mathrm{A}]_0}{\mathrm{t}}$$
B
$$\mathrm{k}=\frac{1}{\mathrm{t}} \log _{10} \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}$$
C
$$k=\frac{[\mathrm{A}]_0-[\mathrm{A}]_1}{\mathrm{t}}$$
D
$$k=\frac{t}{2.303} \times \log _{10} \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}$$
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