The Integrated Rate Equation

Give two exapmles for zero order reaction.

Hydrolysis of an ester in an aqueous solution was studied by titrating the liberated carboxylic acid against sodium hydroxide solution. The concentrations of the ester at different time intervals are given below:

Show that, the reaction follows first order kinetics.

The rate constant for a first order reaction is $2.3\times {10}^{-4} {\mathrm{s}}^{-1}$. If the initial concentration of the reaction is $0.01 \mathrm{M}$ What concentration will remain after one hour?

A first order reaction is 40% complete in 50 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?

From the following data, show that the decomposition of hydrogen peroxide is a reaction of the first order:

Where t is the time in minutes and V is the volume of standard ${\mathrm{KMnO}}_4$ solution required for titrating the same volume of the reaction mixture.

Benzene diazonium chloride in aqueous solution decomposes according to the equation ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{N}}_2\mathrm{Cl}\to {\mathrm{C}}_6{\mathrm{H}}_5\mathrm{Cl} + {\mathrm{N}}_2$. Starting with an initial concentration of $10 \mathrm{g} {\mathrm{L}}^{-1}$, the volume of ${\mathrm{N}}_2$ gas obtained at $50 °\mathrm{C}$ at different intervals of time was found to be as under:

Show that the above reaction follows the first order kinetics. What is the value of the rate constant?

A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?

The time for half change in a first order decomposition of a substance A is 60 seconds. Calculate the rate constant. How much of A will be left after 180 seconds?

Explain pseudo first order reaction with an example.

The decomposition of ${\mathrm{Cl}}_2{\mathrm{O}}_7$ at $500 \mathrm{K}$ in the gas phase to ${\mathrm{Cl}}_2$ and ${\mathrm{O}}_2$ is a first order reaction. After $1 \min$ at $500 \mathrm{K}$, the pressure of ${\mathrm{Cl}}_2{\mathrm{O}}_7$ falls from $0.08$ to $0.04 \mathrm{atm}$. Calculate the rate constant in ${\mathrm{s}}^{-1}$.

Describe the graphical representation of first order reaction.

Derive integrated rate law for a zero order reaction $\mathrm{A} \to \mathrm{Products}$.

If 75% of a first order reaction was completed in 60 minutes , 50% of the same reaction under the same conditions would be completed in

In a homogeneous reaction $\mathrm{A}\to \mathrm{B}+\mathrm{C}+\mathrm{D}$, the initial pressure was ${\mathrm{P}}_0$ and after time $\mathrm{t}$ it was $\mathrm{P}$. Expression for rate constant in terms of ${\mathrm{P}}_0, \mathrm{P}$ and $\mathrm{t}$ will be

In a first order reaction $\mathrm{x}\to \mathrm{y}$; if $\mathrm{k}$ is the rate constant and the initial concentration of the reactant $\mathrm{x}$ is $0.1 \mathrm{M}$, then, the half life is

For a first order reaction, the rate constant is 6.909 min^-1 the time taken for 75% conversion in minutes is

This reaction follows first order kinetics. The rate constant at particular temperature is $2.303\times {10}^{-2} {\mathrm{hour}}^{-1}$. The initial concentration of cyclopropane is $0.25 \mathrm{M}$. What will be the concentration of cyclopropane after $1806$ minutes? ($\log 2=0.3$)

For a first order reaction $\mathrm{A}\to \mathrm{B}$ the rate constant is $\mathrm{x} {\min }^{-1}$. If the initial concentration of $\mathrm{A}$ is $0.01 \mathrm{M}$, the concentration of $\mathrm{A}$ after one hour is given by the expression.