Integrated Rate Law for Zero and First Order Reactions

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

What is the order of a reaction whose rate constant is $5 \mathrm{x} {10}^{-4} {\mathrm{mol}}^{-1}\mathrm{litre} {\mathrm{s}}^{-1}$?

At $30°\mathrm{C}$, the half life for the decomposition of ${\mathrm{AB}}_2$ is $200 \mathrm{s}$ and is independent of the initial concentration of ${\mathrm{AB}}_2$. The time required for $80\%$ of the ${\mathrm{AB}}_2$ to decompose is (Given: $\log 2 = 0.30; \log 3 = 0.48$)

$\mathrm{A}\to \mathrm{B}+\mathrm{C}$

The rate constant of the given reaction is $2.5\times {10}^2$ $\mathrm{mole} {\mathrm{lit}}^{-1} {\sec }^{-1}$ at initial concentration of reactant $0.5\mathrm{M}$. Calculate order of reaction.

The number of incorrect statement/s from the following is ______________

A. The successive half lives of zero order reactions decreases with time.

B. A substance appearing as reactant in the chemical equation may not affect the rate of reaction

C. Order and molecularity of a chemical reaction can be a fractional number

D. The rate constant units of zero and second order reaction are $\mathrm{molL}{}^{-1} {\mathrm{s}}^{-1}$ and ${\mathrm{mol}}^{-1} \mathrm{L} {\mathrm{s}}^{-1}$ respectively

${\mathrm{t}}_{87.5}$ is the time required for the reaction to undergo $87.5\%$ completion and ${\mathrm{t}}_{50}$ is the time required for the reaction to undergo $50\%$ completion. The relation between ${\mathrm{t}}_{87.5}$ and ${\mathrm{t}}_{50}$ for a first order reaction is ${\mathrm{t}}_{87.5}=\mathrm{x}\times {\mathrm{t}}_{50}$
The value of $\mathrm{x}$ is $\_\_\_\_\_\_\_\_\_.$ (Nearest integer)

$\mathrm{A}\left(\mathrm{g}\right)\to 2 \mathrm{B}( \mathrm{g})+\mathrm{C}\left(\mathrm{g}\right)$ is a first order reaction. The initial pressure of the system was found to be $800 \mathrm{mm} \mathrm{Hg}$ which increased to $1600 \mathrm{mm} \mathrm{Hg}$ after $10 \min$. The total pressure of the system after $30$min will be $\mathrm{mm} \mathrm{Hg}$. (Nearest integer)

A molecule undergoes two independent first order reactions whose respective half lives are $12 \min$ and $3 \min$. If both the reactions are occurring then the time taken for the $50\%$ consumption of the reactant is ______ $\min$. (Nearest integer)

For a chemical reaction $A+B\to$ Product, the order is $1$ with respect to $A$ and $B$.

What is the value of $x$ and $y$?

A has half life of $5$ years. Find the amount of A left after $15$ years.

For the first order reactions, the ratio of ${\mathrm{t}}_{50\%} \mathrm{and} {\mathrm{t}}_{87.5\%}$ will be $1 : \mathrm{x}$. Find the value of $\mathrm{x}$ ?

Prove that the time required for $99.9\%$ of a $1$st order reaction is ten times the half life period.

Sketch the graph for first order reaction by taking $\ln \left[\mathrm{A}\right]$ of concentration of reaction along y- axis and time on x-axis?

Sketch the graph for  zero order reaction by take of concentration of reaction along $\mathrm{y}-$ axis and time on $\mathrm{x}-$axis?

The reaction $\mathrm{A}\to \mathrm{B}+\mathrm{C}$ is found to be zero order reaction. If it takes $3.3\times {10}^2$ seconds for an initial concentration of $\mathrm{A}$ to go from $0.50 \mathrm{M} \mathrm{to} 0.25\mathrm{M}$, what is the rate constant for the reaction.

A first order reaction is found to have a half-life of $1.15 \times {10}^{4 }\mathrm{s}$.

What will be the time required for completion of $99\%$ of the reaction?

A first order reaction is $25\%$ completed in $40$ minutes. calculate the value of rate constant. In what time will the reaction be $80\%$ completed?  Given: $\log 3=0.477, \log 4=0.602.$

In a first order reaction $\mathrm{A}\to \mathrm{B}$, If $\mathrm{K}$ is the rate constant and initial concentration of the reactant $\mathrm{A} \mathrm{is} 0.5 \mathrm{M}$ then the half life is :