MHT CET 2023 12th May Evening Shift | Chemical Kinetics Question 14 | Chemistry

The rate law for the reaction $$\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$$ at $$25^{\circ} \mathrm{C}$$ is given by rate $$=k[A][B]^2$$. Calculate the rate of reaction if rate constant at same temperature is $$6.25 \mathrm{~mol}^{-2} \mathrm{~dm}^6 \mathrm{~s}^{-1}[[\mathrm{~A}]=1 \mathrm{M},[\mathrm{B}]=0.2 \mathrm{M}]$$

$$0.25 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$

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

$$0.75 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$

$$1.25 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$

MHT CET 2023 12th May Morning Shift

MCQ (Single Correct Answer)

-0

Calculate the time needed for reactant to decompose $$99.9 \%$$ if rate constant of first order reaction is 0.576 minute$$^{-1}$$.

8 minutes

12 minutes

16 minutes

20 minutes

MHT CET 2023 12th May Morning Shift

MCQ (Single Correct Answer)

-0

Calculate the rate constant of first order reaction if half life of reaction is 40 minutes.

$$1.733 \times 10^{-2}$$ minute $$^{-1}$$

$$1.951 \times 10^{-2}$$ minute $$^{-1}$$

$$1.423 \times 10^{-2}$$ minute $$^{-1}$$

$$1.256 \times 10^{-2}$$ minute $$^{-1}$$

MHT CET 2023 12th May Morning Shift

MCQ (Single Correct Answer)

-0

Identify rate law expression for $$2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NOCl}_{(\mathrm{g})}$$ if the reaction is second order in $$\mathrm{NO}$$ and first order in $$\mathrm{Cl}_2$$.

Rate $$=\mathrm{k}[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]$$

Rate $$=\mathrm{k}[\mathrm{NO}]\left[\mathrm{Cl}_2\right]$$

$$\mathrm{Rate}=\mathrm{k}[\mathrm{NO}]^2$$

Rate $$=\mathrm{k}\left[\mathrm{Cl}_2\right]$$

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