Consider a certain reaction \(A \rightarrow Products\) with \(k = 2.0 \times 10^{-2}s^{-1}\). Calculate the concentration of \(A\) remaining after 100 s if the initial concentration of \(A\) is \(1.0 mol L^{-1}\).

The experimental data for decomposition of \(N_{2}O_{5}\) [\(2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}\)] in gas phase at 318K are given below:

(iii) Draw a graph between \(log[N_{2}O_{5}]\) and \(t\).

The decomposition of dimethyl ether leads to the formation of \(CH_{4}\), \(H_{2}\) and \(CO\) and the reaction rate is given by
Rate = \(k [CH_{3}OCH_{3}]^{\frac{3}{2}}
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,
Rate = \(k(p_{CH_{3}OCH_{3}})^{\frac{3}{2}}
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?

For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data are obtained. 

Calculate the rate constant.

The experimental data for decomposition of \(N_{2}O_{5}\) [\(2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}\)] in gas phase at 318K are given below: 

(iv) What is the rate law ?

A reaction is first order in \(A\) and second order in \(B\).
(ii) How is the rate affected on increasing the concentration of \(B\) three times?

For a first order reaction, show that time required for 99% completion is twice the time required for the completion of 90% of reaction.

The decomposition of \(NH_{3}\) on platinum surface is zero order reaction. What are the rates of production of \(N_{2}\) and \(H_{2}\) if \(k = 2.5 \times 10^{-4} mol^{-1} L s^{-1}\)?

Calculate the half-life of a first order reaction from their rate constants given below:
(iii) \(4 years^{-1}\)

A first order reaction takes 40 min for 30% decomposition. Calculate \(t_{1/2}\).

Calculate the half-life of a first order reaction from their rate constants given below:
(ii) \(2 min^{-1}\)

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) \(3NO(g) \rightarrow N_{2}O (g)\) Rate = \(k[NO]^{2}\)

A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
(ii) reduced to half ?

The experimental data for decomposition of \(N_{2}O_{5}\) [\(2N_{2}O_{5} \rightarrow 4NO_{2} + O_{2}\)] in gas phase at 318K are given below:

(vi) Calculate the half-life period from \(k\) and compare it with (ii).

The rate constant for a first order reaction is \(60 s^{-1}\). How much time will it take to reduce the initial concentration of the reactant to its \(\frac{1}{16}\)th value?

The following results have been obtained during the kinetic studies of the reaction: \(2A + B \rightarrow C + D\)

Determine the rate law and the rate constant for the reaction.

Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law, with \(t_{1/2} = 3.00\) hours. What fraction of sample of sucrose remains after 8 hours ?

The rate constant for the first order decomposition of \(H_{2}O_{2}\) is given by the following equation:
\(log k = 14.34 – \frac{1.25 \times 10^{4}K}{T}\)
Calculate \(E_{a}\) for this reaction and at what temperature will its half-period be 256 minutes?

Order of a reaction is

In a reaction between \(A\) and \(B\), the initial rate of reaction (\(r_{0}\)) was measured for different initial concentrations of \(A\) and \(B\) as given below: 

What is the order of the reaction with respect to \(A\) and \(B\)?