MHT CET 2025 26th April Morning Shift | Chemical Kinetics Question 6 | Chemistry

Rate of the reaction $\mathrm{A}+\mathrm{B} \longrightarrow$ product is $3.6 \times 10^{-2} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$ and rate law is $\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}]^2$. What is rate constant of the reaction if $[\mathrm{A}]=0.2 \mathrm{M}$ and $[\mathrm{B}]=0.1 \mathrm{M}$ ?

$10 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{~s}^{-1}$

$18 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{~s}^{-1}$

$24 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{~s}^{-1}$

$4.8 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{~s}^{-1}$

MHT CET 2025 26th April Morning Shift

MCQ (Single Correct Answer)

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Calculate rate constant of a first order reaction having pre exponential factor $1.6 \times 10^{13} \mathrm{~s}^{-1}$.

$$ \left(\mathrm{E}_{\mathrm{a}} / 2.303 \mathrm{RT}=21\right) $$

$1.6 \times 10^{-13}$

$3.2 \times 10^{-13}$

$3.2 \times 10^{-8}$

$1.6 \times 10^{-8}$

MHT CET 2025 25th April Evening Shift

MCQ (Single Correct Answer)

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If Instantaneous rate of reaction is stated as $-\frac{1}{2} \frac{\mathrm{~d}[x]}{\mathrm{dt}}=-\frac{\mathrm{d}[\mathrm{y}]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{~d}[\mathrm{z}]}{\mathrm{dt}}$, identify the reaction.

$x-2 y \longrightarrow 2 z$

$2 x+y \longrightarrow 2 z$

$x+y \longrightarrow z$

$\quad 2 x-2 y \longrightarrow z$

MHT CET 2025 25th April Evening Shift

MCQ (Single Correct Answer)

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Which of the following is an example of second order reaction?

$2 \mathrm{H}_2 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{H}_2 \mathrm{P}_{(\ell)}+\mathrm{O}_{2(\mathrm{~g})}$

$\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{HI}_{(\mathrm{g})}$

$\mathrm{CH}_3 \mathrm{CHO}_{(\mathrm{g})} \longrightarrow \mathrm{CH}_{4(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})}$

$2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$

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