Chemical Kinetics - PYQ Practice (Physical Chemistry)

If the rate constant for a first order reaction is \(2.303 \times 10^{-3} \mathrm{~s}^{-1}\). Find the time required to reduce \(4 \mathrm{~g}\) of the reactant to \(0.2 \mathrm{~g}\).

For a \(A+B \rightarrow\) products, the rate of the reaction is given by rate \(=k[A][B]^2\). The units of rate constant \((k)\) will be

For an elementary reaction, \(X(g) \longrightarrow Y(g)+Z(g)\), the \(t_{1 / 2}\) is \(10 \mathrm{~min}\). In what period of time would the concentration of \(X\) be reduced to \(10 \%\) of its original concentration?

Which statement among the following is incorrect?

For zero order reaction, a plot of \(t_{1 / 2}\) versus \([A]_0\) will be

The time required for completion of \(93.75 \%\) of a first order reaction is \(x\) minutes. The half-life of it (in minutes) is

. The rate constant for a zero order reaction \(A \longrightarrow\) products is \(0.0030 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~S}^{-1}\). How long it will take for the initial concentration of \(A\) to fall from 0.10 M to 0.075 M ?

The rate constant of a reaction at 500 K and 700 K are \(0.02 \mathrm{~s}^{-1}\) and \(0.2 \mathrm{~s}^{-1}\) respectively. The activation energy of the reaction (in \(\left.\mathrm{kJ} \mathrm{mol}^{-1}\right)\) is \(\left(R=8.3 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

For a first order reaction the concentration of reactant was reduced from $0.03 \mathrm{molL}^{-1}$ to $0.02 \mathrm{molL}^{-1}$ in 25 min . What is its rate (in $\mathrm{molL}^{-1} \mathrm{~s}^{-1}$ )?

Isomerisation of gaseous cyclobutene to butadiene is first order reaction. At $T(\mathrm{~K})$. The rate constant of reaction is $33 \times 10^{-4} \mathrm{~s}^{-1}$. What is the time required (in min ) to complete $90 \%$ of this reaction at the temperature? $(\log 2=03)$

$A \rightarrow$ products, is a first order reaction. The following data is obtained for this reaction at $T(\mathrm{~K})$. The value of $x: y$ is

$$\begin{array}{cc} \hline \text { Rate }\left(\mathrm{molL}^{-1} \mathrm{~min}^{-1}\right) & {[A]} \\ \hline 0.2 & 0.02 \mathrm{M} \\ \hline 0.4 & x \mathrm{M} \\ \hline 1.0 & y \mathrm{M} \\ \hline \end{array}$$

Activation energy for the hydrolysis of sucrose by acid is $X \mathrm{~kJ} \mathrm{~mol}^{-1}$ whereas activation energy for the hydrolysis of sucrose by sucrase is $Y \mathrm{~kJ} \mathrm{~mol}^{-1} . X$ and $Y$ respectively are