Integrated Rate Equations of Chemical Reaction

In a first-order reaction, the concentration of reactant decreases from $\text{800}{\text{ mol/dm }}^3{\text{ to 50 mol/dm }}^3$ in$2 \times {10}^2 \mathrm{s}$. The rate constant of reaction in ${\mathrm{s}}^{-1}$ is

Acid catalysed hydrolysis of esters is pseudo first order reactions because water is present in excess in given reaction.

For acid catalysed hydrolysis of ester rate law obtained is rate $= \left[\mathrm{ester}\right]\left[{\mathrm{H}}^{+}\right]$, where $\mathrm{k} = 0.01{\mathrm{M}}^{-1}{\mathrm{hr}}^{-1}$. What is the half-life if the initial concentrations are $0.02 \mathrm{M}$ for the ester and $0.05 \mathrm{M}$ for the catalysing acid?

Select the correct statement for a first-order reaction from the following.

The hydrolysis of ester is a

The half life of a first order reaction is $12 \min$. Fraction of the reactant left behind after $1\mathrm{hr}$ from the beginning is

Graph of half life of first-order reaction and initial concentration of reactant is a:

Graph of half life of zero-order reaction and initial concentration of reactant is a:

The consecutive reaction $\mathrm{X}⟶\mathrm{Y}⟶\mathrm{Z}$ takes place in a closed container. Initially, the container has ${\mathrm{A}}_0$ moles of $\mathrm{X}$ (and no $\mathrm{Y}$ and $\mathrm{Z}$). The plot of total moles of the constituents in the container as a function of time will be

Which among the following represents the expression for $(3/4{)}^{\mathrm{th}}$ life of $1^{\mathrm{st} }$ order reaction?

If the rate constant of a first order reaction is $4.606\times {10}^{-3}{ \mathrm{s}}^{-1}$, then find the time required for $400 \mathrm{g}$ of the reactant to reduce to $50 \mathrm{g}$.

If the decomposition reaction ${\mathrm{A}}_{\left(\mathrm{g}\right)}⟶{\mathrm{B}}_{\left(\mathrm{g}\right)}$ follows first order kinetics, then the graph of rate of formation of $\mathrm{B},$ denoted by $\mathrm{R},$ against time $\text{'}t\text{'}$ will be

If the rate constant for a first order reaction is $\mathrm{k},$ then find the time required for completion of $80\%$ of the reaction.

Reactant $R$ gives $n$ different products $\left(P_r:r=1,2,3,\cdots ,n\right)$ in $n$ parallel first order reactions. Rate constant for the formation of any produet $P_r$ is $rk$ where $r=1,2,3,\cdots ,n.$ For the decay of $R,$ what is the overall rate constant in terms of $k?$

For a zero-order reaction, with the initial reactant concentration $\mathrm{a}$, the time for completion of the reaction is:

The accompanying figure depicts the change in concentration of species $\mathrm{X}$ and $\mathrm{Y}$ for the elementary reaction $\mathrm{X}\to \mathrm{Y}$ as a function of time. The point of intersection of two curves represents:

The order of a reaction for which a linear line (with a negative slope) is obtained in a graph of $\log (\mathrm{a}-\mathrm{x})$ vs $\mathrm{t}$ is:

Two-third life for a first-order reaction is $55$ minutes. The value of its velocity constant is nearly

For a first order reaction $\mathrm{R}\to \mathrm{P}$, the rate constant is $\mathrm{k}$. If the initial concentration of $\mathrm{R}$ is ${\left[\mathrm{R}\right]}_0$, the concentration of $\mathrm{R}$ at any time $\text{'}\mathrm{t}\text{'}$ is given by the expression: