MHT CET 2023 13th May Evening Shift | Chemical Kinetics Question 54 | Chemistry

For the reaction, $$2 A+2 B \longrightarrow 2 C+D$$, the rate law is expressed as rate $$=k[A]^2[B]$$. Calculate the rate constant if rate of reaction is $$0.24 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$.

[[$$A$$]$$=0.5 \mathrm{M}$$ and $$[B]=0.2 \mathrm{M}$$]

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

$$9.6 \mathrm{~mol}^{-2} \mathrm{~dm}^6 \mathrm{~s}^{-1}$$

$$12.1 \mathrm{~mol}^{-2} \mathrm{~dm}^6 \mathrm{~s}^{-1}$$

$$14.4 \mathrm{~mol}^{-2} \mathrm{~dm}^6 \mathrm{~s}^{-1}$$

MHT CET 2023 13th May Morning Shift

MCQ (Single Correct Answer)

-0

Find the rate of formation of $$\mathrm{NO}_{2(\mathrm{~g})}$$ in the following reaction.

$$\begin{aligned} & 2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \\ & {\left[\frac{-\mathrm{d}\left[\mathrm{N}_2 \mathrm{O}_5\right]}{\mathrm{dt}}=0.02 \mathrm{~mol} \mathrm{~dm}^{-3}\right]} \end{aligned}$$

$$0.01 \mathrm{~mol} \mathrm{~dm}^{-3}$$

$$0.02 \mathrm{~mol} \mathrm{~dm}^{-3}$$

$$0.03 \mathrm{~mol} \mathrm{~dm}^{-3}$$

$$0.04 \mathrm{~mol} \mathrm{~dm}^{-3}$$

MHT CET 2023 13th May Morning Shift

MCQ (Single Correct Answer)

-0

Calculate the rate constant of the first order reaction if $$20 \%$$ of the reactant decomposes in 15 minutes.

$$1.488 \times 10^{-2}$$ minute $$^{-1}$$

$$1.881 \times 10^{-2}$$ minute $${ }^{-1}$$

$$1.984 \times 10^{-2}$$ minute $$^{-1}$$

$$1.18 \times 10^{-2}$$ minute $$^{-1}$$

MHT CET 2023 13th May Morning Shift

MCQ (Single Correct Answer)

-0

Which from following is the slope of the graph of $$[\mathrm{A}]_{\mathrm{t}}$$ versus time for zero order reaction?

$$-\mathrm{k}$$

$$\mathrm{k}$$

$$\frac{\mathrm{k}}{2.303}$$

$$\frac{-\mathrm{k}}{2.303}$$

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