One ml of methyl acetate was added to 20 ml of 0.5 N sulphuric acid. 2 ml of the reaction mixture was with drawn at various time intervals and titrated against a solution of standard alkali. The titre values are tabulated. Show that the reaction is first order and calculate the rate constant and half life period of the reaction.

Rate constant of a first order reaction is 0.45 sec^(-1) , calculate its half life.

A certain amount of methyl acetate was hydrolysed in the presence of excess of "0.05 M HCl at "25^(@)C . 20 mL of reaction mixture were removed and titrated with NaOH solution, the volume V of alkali required for neutralisation after time ‘t’ were as follows : {:("t(min)",0,20,40,60,oo),("v(mL)",20.2,25.6,29.5,32.8,50.5):} Show that the reaction is the first order reaction.

The initial rate of a first order reaction is 5.2 xx 10^(-6)" mol.lit"^(-1).s^(-1) at 298 K. When the initial concentration of reactant is 2.6xx10^(-3)" mol.lit"^(-1) , calculate the first order rate constant of the reaction at the same temperature.

During the discharge of a lead storage battery, the density of sulphuric acid fell from 1.294 g mL^(-1) to 1.139 g mL^(-) . Sulphuric acid of density 1.294 g mL^(-1) is 39% by weight and that of density 1.139 g mL^(-1) is 20% by weight. The battery hold 3.5 litre of acid and discharge. Calculate the no. of ampere hour for which the battery must have been used. The charging and discharging reactions are: Pb+SO_(4)^(2-) rarr PbSO_(4)+2e (charging) PbO_(2)+4H^(+)+SO_(4)^(2-)+2e rarr PbSO_(4)+2H_(2)O (discharging)