MHT CET 2024 16th May Morning Shift | Chemical Kinetics Question 3 | Chemistry

A zero order reaction has half life time of 0.2 minute. If initial concentration of reactant is $0.2 \mathrm{~mol} \mathrm{dm}^{-3}$. Find rate constant.

$0.2 \mathrm{~mol}^{-1} \mathrm{dm}^3 \mathrm{~min}^{-1}$

$0.5 \mathrm{~mol}^{-1} \mathrm{dm}^3 \mathrm{~min}^{-1}$

$1.4 \mathrm{~mol}^{-1} \mathrm{dm}^3 \mathrm{~min}^{-1}$

$6.0 \mathrm{~mol}^{-1} \mathrm{dm}^3 \mathrm{~min}^{-1}$

MHT CET 2024 15th May Evening Shift

MCQ (Single Correct Answer)

-0

The reaction given below $2 \mathrm{NH}_{3(\mathrm{g})} \xrightarrow{\mathrm{Pt}} \mathrm{N}_{2(\mathrm{g})}+3 \mathrm{H}_{2(\mathrm{g})}$ has rate of reaction $2.5 \times 10^{-6} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{sec}^{-1}$ formation of $\mathrm{H}_{2(\mathrm{~g})}$ ?

$2.5 \times 10^{-6} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$

$3.75 \times 10^{-6} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$

$5.0 \times 10^{-6} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$

$7.5 \times 10^{-6} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{sec}^{-1}$

MHT CET 2024 15th May Evening Shift

MCQ (Single Correct Answer)

-0

For reaction $\mathrm{A}+\mathrm{B} \rightarrow$ product, rate of reaction is $3.6 \times 10^{-2} \mathrm{sec}^{-1}$. When $[\mathrm{A}]=0.2 \mathrm{moldm}^{-3}$ and $[B]=0.1 \mathrm{moldm}^{-3}$, calculate rate constant of reaction if reaction is first order in A and second order is B ?

$3.6 \mathrm{~mol}^{-2} \mathrm{dm}^6 \mathrm{sec}^{-1}$

$1.8 \mathrm{~mol}^{-2} \mathrm{dm}^{-6} \mathrm{sec}^{-1}$

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

$36 \mathrm{~mol}^{-2} \mathrm{dm}^{-6} \mathrm{sec}^{-1}$

MHT CET 2024 15th May Evening Shift

MCQ (Single Correct Answer)

-0

For a reaction $\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}]^2$, if concentration of $A$ is doubled the rate of reaction

increases by 2

increases by 4

decrease by $\frac{1}{2}$

decreases by 2

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