MHT CET 2023 14th May Morning Shift | Chemical Kinetics Question 4 | Chemistry

Find the rate law for the reaction, $$\mathrm{CHCl}_{3(\mathrm{~g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow \mathrm{CCl}_{4(\mathrm{~g})}+\mathrm{HCl}_{(\mathrm{g})}$$ if order of reaction with respect to $$\mathrm{CHCl}_{\mathrm{a}(\mathrm{g})}$$ is one and $$\frac{1}{2}$$ with $$\mathrm{Cl}_{2(\mathrm{~g})}$$.

Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]\left[\mathrm{Cl}_2\right]^{1 / 2}$$

Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^2\left[\mathrm{Cl}_2\right]^{1 / 2}$$

Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^{3 / 2}\left[\mathrm{Cl}_2\right]$$

Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^{1 / 2}\left[\mathrm{Cl}_2\right]$$

MHT CET 2023 14th May Morning Shift

MCQ (Single Correct Answer)

-0

The rate for reaction $$2 \mathrm{~A}+\mathrm{B} \rightarrow$$ product is $$6 \times 10^{-4} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$$ Calculate the rate constant if the reaction is first order in $$\mathrm{A}$$ and zeroth order in $$\mathrm{B}$$. [Given $$[\mathrm{A}]=[\mathrm{B}]=0.3 \mathrm{M}]$$

$$1 \times 10^{-3} \mathrm{~s}^{-1}$$

$$2 \times 10^{-3} \mathrm{~s}^{-1}$$

$$3 \times 10^{-3} \mathrm{~s}^{-1}$$

$$4 \times 10^{-3} \mathrm{~s}^{-1}$$

MHT CET 2023 14th May Morning Shift

MCQ (Single Correct Answer)

-0

Calculate half life of first order reaction if rate constant of reaction is $$2.772 \times 10^{-3} \mathrm{~s}^{-1}$$

125 s

250 s

100 s

150 s

MHT CET 2023 13th May Evening Shift

MCQ (Single Correct Answer)

-0

Which from following statements about rate constant is NOT true?

It is independent of concentration.

It varies with temperature.

It is equal to rate of reaction at unit concentration of reactants.

It's unit is independent of order of reaction.

PREVIOUS NEXT

MHT CET Subjects