MHT CET 2024 2nd May Morning Shift | Chemical Kinetics Question 83 | Chemistry

$$\begin{aligned} & 2 \mathrm{~N}_2 \mathrm{O}_{5(8)} \longrightarrow 4 \mathrm{NO}_{2(g)}+\mathrm{O}_{2(\mathrm{~g})} \\ & {\left[\frac{\mathrm{d}\left[\mathrm{~N}_2 \mathrm{O}_5\right]}{\mathrm{dt}}=0.02 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}\right]} \end{aligned}$$

$0.01 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$

$0.02 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$

$0.03 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$

$0.04 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$

MHT CET 2024 2nd May Morning Shift

MCQ (Single Correct Answer)

-0

Rate law for the reaction $2 \mathrm{NO}+\mathrm{Cl}_2 \rightarrow 2 \mathrm{NOCl}$ is rate $=\mathrm{k}[\mathrm{NO}]^2\left[\mathrm{Cl}_2\right]$. When will the value of k increase?

by increasing temperature

by increasing [NO]

by increasing $\left[\mathrm{Cl}_2\right]$

by increasing both [NO] and $\left[\mathrm{Cl}_2\right]$

MHT CET 2023 14th May Evening Shift

MCQ (Single Correct Answer)

-0

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

$$2.68 \times 10^{-2}$$ minute $$^{-1}$$

$$5.36 \times 10^{-2}$$ minute $$^{-1}$$

$$1.34 \times 10^{-2}$$ minute $$^{-1}$$

$$8.1 \times 10^{-2}$$ minute $$^{-1}$$

MHT CET 2023 14th May Evening Shift

MCQ (Single Correct Answer)

-0

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

$$2.5 \times 10^{-3}$$ time$$^{-1}$$

$$5.0 \times 10^{-3}$$ time$$^{-1}$$

$$7.5 \times 10^{-3}$$ time$$^{-1}$$

$$1.25 \times 10^{-3}$$ time$$^{-1}$$

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