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1
MHT CET 2023 14th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

Calculate the rate constant of the first order reaction if $$80 \%$$ of the reactant decomposes in 60 minutes.

A
$$2.68 \times 10^{-2}$$ minute $$^{-1}$$
B
$$5.36 \times 10^{-2}$$ minute $$^{-1}$$
C
$$1.34 \times 10^{-2}$$ minute $$^{-1}$$
D
$$8.1 \times 10^{-2}$$ minute $$^{-1}$$
2
MHT CET 2023 14th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

What is the value of rate constant for first order reaction if slope for the graph of rate versus concentration is $$2.5 \times 10^{-3}$$ ?

A
$$2.5 \times 10^{-3}$$ time$$^{-1}$$
B
$$5.0 \times 10^{-3}$$ time$$^{-1}$$
C
$$7.5 \times 10^{-3}$$ time$$^{-1}$$
D
$$1.25 \times 10^{-3}$$ time$$^{-1}$$
3
MHT CET 2023 14th May Evening Shift
MCQ (Single Correct Answer)
+1
-0

The rate law for the reaction $$\mathrm{A}+\mathrm{B} \rightarrow$$ product is rate $$=\mathrm{k}[\mathrm{A}][\mathrm{B}]$$. When will the rate of reaction increase by factor two?

A
$$[\mathrm{A}]$$ and $$[\mathrm{B}]$$ both are doubled
B
$$[\mathrm{A}]$$ is doubled and $$[\mathrm{B}]$$ is kept constant
C
$$[\mathrm{B}]$$ is doubled and $$[\mathrm{A}]$$ is halved
D
[A] is kept constant [B] is halved
4
MHT CET 2023 14th May Morning Shift
MCQ (Single Correct Answer)
+1
-0

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 $$\mathrm{Cl}_{2(\mathrm{~g})}$$.

A
Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]\left[\mathrm{Cl}_2\right]^{1 / 2}$$
B
Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^2\left[\mathrm{Cl}_2\right]^{1 / 2}$$
C
Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^{3 / 2}\left[\mathrm{Cl}_2\right]$$
D
Rate $$=\mathrm{k}\left[\mathrm{CHCl}_3\right]^{1 / 2}\left[\mathrm{Cl}_2\right]$$
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