Integrated Rate Law for Zero and First Order Reactions

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

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

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 :

In $30$ minutes, a first-order reaction is $50\%$ complete. Calculate the amount of  time it took to complete $87.5$ percent of the reaction.

For a reaction : $2{\mathrm{A}}_{\left(\mathrm{g}\right)}\to {\mathrm{B}}_{\left(\mathrm{g}\right)} + 3{\mathrm{C}}_{\left(\mathrm{g}\right)}$, rate constant of disappearance of $\mathrm{A}$ is ${10}^{-3} \mathrm{M} {\sec }^{-1}$. If initially $2 \mathrm{M}$ of $\mathrm{A}$ is taken then what will be concentration of $\mathrm{C}$ afterr $5$ minutes?

For a chemical reaction, $\mathrm{A}+\mathrm{B}\to \mathrm{Products}$, the order is one with respect to each A and B. Value of x and y from the given data is :

The initial concentration of a zero order reaction is decreased from $4 \mathrm{mol} {\mathrm{L}}^{-1}$ to $1 \mathrm{mol} {\mathrm{L}}^{-1}$. Time for half change

Select the correct statements out of I, II and III for a zero order reaction:

I. Quantity of the product formed is directly proportional to time.

III. If $50\%$ reaction takes place in $100$ minutes, $75\%$ reaction will take place in $150$ minutes.

III.Larger the initial concentration of the reactant, greater is the half-life period.

Define half-life period and average life. Derive relation between them.

Define half-life period. How is it related to the order of a reaction?

Derive integrated rate equation for rate constant for a first order reactants. What would be units of the first order rate constant, if the concentration is expressed in moles per litre and time in seconds?

Derive the equation for the rate constant of a first order reaction and show that the time required for the completion of half of the first order reaction is independent of initial concentration.

Show that for the reactions of first order, half-life period is independent of initial concentrations.

Derive the relationship between rate constant and half-life period of a first order reaction.

The following data were obtained during the first order thermal decomposition of ${\mathrm{SO}}_2{\mathrm{Cl}}_2$ at a constant volume

${\mathrm{SO}}_2{\mathrm{Cl}}_2\left(\mathrm{g}\right)⟶{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$

Calculate the rate constant.

(Given: $\log 4=0.6021,\log 2=0.3010$)

A first order reaction takes $20$ minutes for $25\%$ decomposition. Calculate the time when $75\%$ of the reaction will be completed. (Given: $\log 2=0.3010,\log 3=0.4771,\log 4=0.6021$)

The thermal decomposition of a compound is of first order. If $50\%$ of the compound is decomposed in $120$ minutes, how long will it take for $90\%$ of the compound to decompose?

The rate constant of a first order reaction is $60{ \mathrm{s}}^{-1}$. How much time it will take to reduce $75\%$ of its original concentration?