AP EAPCET 2018 (25-APR Shift-1)

For a first order reaction ${\mathrm{A}}_5\to 5{\mathrm{B}}_2$, the concentrations vs time plot is as shown. The half-life of the reaction is

For zero order reaction, a plot of ${\mathrm{t}}_{1/2}$ versus $[\mathrm{A}{]}_0$ will be

Which statement among the following is incorrect?

For a $\mathrm{A}+\mathrm{B}\to$ products the rate of the reaction is given by Rate $=\mathrm{K}\left[\mathrm{A}\right][\mathrm{B}{]}^2$. The units of rate constant $\left(\mathrm{K}\right)$ will be

The rate constants for a reaction at $400 \mathrm{K}$ and $500 \mathrm{K}$ are $2.60\times {10}^{-5} {\mathrm{s}}^{-1}$ and $2.60\times {10}^{-3} {\mathrm{s}}^{-1}$,respectively. The activation energy of the reaction in ${\mathrm{kJmol}}^{-1}$ is ______

The rate equation for a first-order reaction is given by $\left[\mathrm{R}\right]={\left[\mathrm{R}\right]}_0{\mathrm{e}}^{-\mathrm{kt}}$. A straight line with positive slope is obtained by plotting (${\left[\mathrm{R}\right]}_0=$ Initial concentration of the reactant, $\left[\mathrm{R}\right]=$ concentration of the reactant at time $\mathrm{t}$)

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 an elementary reaction, ${\mathrm{X}}_{\left(\mathrm{g}\right)}⟶{\mathrm{Y}}_{\left(\mathrm{g}\right)}+{\mathrm{Z}}_{\left(\mathrm{g}\right)}$, the ${\mathrm{t}}_{1/2}$ is $10$ minutes. In what period of time would the concentration of $\mathrm{X}$ be reduced to $10\%$ of its original concentration?