Hydrolysis of methyl acetate in aqueous solution has been studied by titrating the liberated acetic acid against sodium hydroxide. The concentration of an ester at different temperatures is given below.

t(min)	0	20	40	60	∝
v (ml)	20.2	25.6	29.5	32.8	50.4

Show that the reaction is the first order reactions.

Prove that the time required for the completion \({ \frac { 3 }{ 4 } }^{ th }\) of the reaction of a first order is twice the time required for the completion of a half of the reaction.

(i) Molecularity of any reaction is not equal to zero. Why?
(ii) For which type of reactions, order, and molecularity have the same value?

A reaction is of 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 concentration of both A and B is doubled?

Give examples for first order reaction.

Give the characteristics of first order reaction.

The rate constant, the activation energy and frequency factor of a chemical reaction at 25^oC are 3.0 x 10^-4 S^-1; 104.4 kJ mol^-1  and 6.0 x 10¹⁴ S^-1 respectively. What is the value of the rate constant when T ⟶ ∞?

The energy of achivation for the formation of hydrogen iodide is 150 kJ mol^-1 The rate constant of this reaction at 673 K is 2.3 x 10^-3. Calculate the rate constant at 773 K.

A first order reaction is found to have a rate A constant k = 7.39 x 10^-5 S^-1. Find the half life of this reaction.

The rate constant k for the first order gas phase decomposition of ethyl iodide, C₂H₅I ⟶ C₂H₄ + HI is 1.60 x 10^-5 s^-1 at 600k and 6.36 x 10^-3 s^-1 at 700K. Calculate the energy of activation for this reaction.

The activation energy of the reaction 2HI_(g) ⟶ H_2(g) +I_2(g) is 209.5 KJ mol^-1 at 581 K. Calculate the fraction of molecules of reactants having energy equal to or greater than activation energy.

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) 3NO_(g) ⟶ N₂O_(g) Rate = K[NO]²
(ii) H₂O_2(aq) + 3I^-_(aq) +2H⁺ ⟶ 2H₂O_(l) +I₃^- Rate = K[H₂O₂][I^-]
(iii) CH₃CHO_(g) ⟶ CH_4(g) + CO_(g) Rate = K[CH₃ CHO]^3/2
(iv) C₂H₅Cl_(g) ⟶ C₂H_2(g) + HCl_(g) Rate = K[C₂H₅Cl]²

The decomposition of NH₃ on platinum surface is zero order reaction what are the rates of production of N₂ and H₂ if k = 2.5 x10^-4 mol + L S^-1.

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

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