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:

(ii) Find the half-life period for the reaction.

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(iv) \(C_{2}H_{5}Cl (g) \rightarrow C_{2}H_{4} (g) + HCl (g)\) Rate = \(k [C_{2}H_{5}Cl]\)

The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of \(A\) is \(4 \times 10^{10}s^{-1}\). Calculate \(k\) at 318K and \(E_{a}\).

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:

(i) Plot \([N_{2}O_{5}]\) against \(t\).

The rate constant for the decomposition of \(N_{2}O_{5}\) at various temperatures is given below:

Draw a graph between \(ln k\) and \(1/T\) and calculate the values of \(A\) and \(E_{a}\). Predict the rate constant at 30° and 50°C.

What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?

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:

(v) Calculate the rate constant.

For the reaction:
\(2A + B \rightarrow A_{2}B\)
the rate = \(k[A][B]^{2}\) with \(k = 2.0 \times 10^{-6} mol^{-2} L^{2} s^{-1}\). Calculate the initial rate of the reaction when \([A] = 0.1 \text{ mol } L^{-1}\), \([B] = 0.2 \text{ mol } L^{-1}\). Calculate the rate of reaction after \([A]\) is reduced to \(0.06 \text{ mol } L^{-1}\).

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 ?

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 = \(k[NO]^{2}\)

The rate of a reaction quadruples when the temperature changes from 293 K to 313 K. Calculate the energy of activation of the reaction assuming that it does not change with temperature.

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 decomposition of hydrocarbon follows the equation
\(k = (4.5 \times 10^{11}s^{-1}) e^{-28000K/T}\)
Calculate \(E_{a}\).

A reaction is first order in \(A\) and second order in \(B\).
(iii) How is the rate affected when the concentrations of both \(A\) and \(B\) are doubled?

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 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 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?

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 \(B\)?

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