MHT CET 2024 15th May Evening Shift | Chemical Kinetics Question 4 | Chemistry

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

MHT CET 2024 15th May Morning Shift

MCQ (Single Correct Answer)

-0

For the reaction

$$\begin{aligned} & 2 \mathrm{NO}_{(\mathrm{s})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{s})} \\\\ & \text { rate }=\mathrm{k}[\mathrm{NO}]^2\left[\mathrm{H}_2\right] . \end{aligned}$$

What is the order of reaction with respect to $\mathrm{H}_2$ and overall order of reaction respectively?

$0,2$

$1,3$

$2,1$

$3,1$

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