271. The reaction:
${\mathrm{CH}}_3\mathrm{COF} + {\mathrm{H}}_2\mathrm{O} \to {\mathrm{CH}}_3\mathrm{COOH}+\mathrm{HF}$

has been studied under the following initial conditions.

$$\begin{gathered} \mathrm{CASE} \mathrm{I}: \mathrm{CASE} \mathrm{II}: \\ {\mathrm{C}}_{{\mathrm{H}}_2\mathrm{O}} = 1.00 \mathrm{M} {\mathrm{C}}_{{\mathrm{H}}_2\mathrm{O}} = 0.02 \mathrm{M}. \\ {\mathrm{C}}_{{\mathrm{CH}}_3\mathrm{COF}} = 0.01 \mathrm{M} {\mathrm{C}}_{{\mathrm{CH}}_3\mathrm{COF}} = 0.80 \mathrm{M} \end{gathered}$$
Concentrations were monitored as a function of time and are given below:

Determine the order of the reaction and the rate constant for the reaction.

For the hydrolysis of methyl acetate in aqueous solution, the following results were obtained:

 (i) Show that it follows pseudo-first order reaction, as the concentration of water remains constant.

(ii) Calculate the average rate of reaction between the time intervals 30 to 60 seconds.

 (Given log 2 = 0.3010, log 4 = 0.6021)

 For a reaction A + B → P, the rate is given by Rate = k[A] [B]²

 (i) How is the rate of reaction affected if the concentration of B is doubled?

 (ii) What is the overall order of reaction if A is present in large excess?

A first order reaction takes 30 minutes for 50% completion. Calculate the time required for 90% completion of this reaction.

_{(log 2 = 0.3010)}

Write two differences between 'order of reaction' and 'molecularity of reaction?

The following data were obtained during the first-order thermal decomposition of SO₂Cl₂ at a constant volume:

SO₂Cl₂(g)--->  SO₂(g) + Cl₂(g)

 Calculate the rate constant. (Given :  log 4 = 0.6021, log 2 = 0.3010)

A reaction is second order in A and first order in B.

 (i) Write the differential rate equation.

(ii) How is the rate affected on increasing the concentration of A three times?

(iii) How is the rate affected when the concentrations of both A and B are doubled?

A first order reaction takes 40 minutes for 30% decomposition. Calculate t_1/2 for this reaction.

 (Given log 1.428 = 0.1548)

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

Rate constant ‘k’ of a reaction varies with temperature ‘T’ according to the equation:

where E_a is the activation energy.

When a graph is plotted for   a straight line with a slope of -4250 K is obtained. Calculate ‘E_a’ for the reaction.

(R = 8.314 JK^-1 mol^-1)