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

In a first order reaction the concentration of reactant decreases from $800 \mathrm{mol}/{\mathrm{dm}}^{\mathrm{3}}$ to  $50 \mathrm{mol}/{\mathrm{dm}}^{\mathrm{3}}$ in $200 \sec$. The rate constant of reaction in ${\mathrm{s}}^{-\mathrm{1}}$ is

The rate-constant of a reaction is $3.5\times {10}^{-12}{\mathrm{s}}^{-1}$. The half-life of this reaction (in s) 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 $k?$

The rate constant for the first-order reaction is $60\mathrm{ }{\mathrm{s}}^{-1}$. How much time will it take to reduce the concentration of the reactant to $1/16$ of initial value?

Which of the following curve represent zero order reaction of $\mathrm{A}\mathrm{ }\to \mathrm{ }$products?

The inactivation of a viral preparation in a chemical bath is found to be a first order reaction. Calculate the rate constant for the viral inactivation if in the beginning $1.5\mathrm{ }\mathrm{\%}$ of the virus is inactivated per minute.

 $\left(\mathrm{Given}:\ln \frac{100}{98.5}=0.01511\right)$

Two first-order reactions have half times in the ratio of $8 : 1.$ The ratio of time intervals ${\mathrm{t}}_1:{\mathrm{t}}_2$ is:

Here, the time ${\mathrm{t}}_1$ and ${\mathrm{t}}_2$ are time period for ${\left(\frac{1}{4}\right)}^{\mathrm{th}}$ and ${\left(\frac{3}{4}\right)}^{\mathrm{th}}$ completion.

Which of the following equations represent integrated rate equation of zero order reaction?

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

The reaction $\mathrm{A}\to \mathrm{C}+\mathrm{D}$ was found to be second order in $\mathrm{A}$. The rate constant for the reaction was determined to be $2.42 \mathrm{L}/\mathrm{mol}/\mathrm{s}$. If the initial concentration is $0.5 \mathrm{mole}/\mathrm{L},$ what is the value of $t_{\frac{1}{2}}$in sec?

(Express your answer by multiplying with 100 and rounding off to two significant figures)

A drop $(0.05 \mathrm{mL})$ of a solution contains $3.0\times {10}^{-6}$ moles of ${\mathrm{H}}^{+}$ Ions. If the rate constant of disappearance of ${\mathrm{H}}^{+}$ ion is $1.0\times {10}^7\mathrm{mol} {\mathrm{litre}}^{-1} {\sec }^{-1},$  the time taken for  ${\mathrm{H}}^{+}$ ions in the drop to disappear is $\mathrm{p}\times {10}^{-\mathrm{q}}. \text{Calculate the value of} \mathrm{q}-\mathrm{p}$.

Give the nearest integer as the answer.