Question

A Lead storage battery is the most important type of secondary cell having a lead anode and a grid of lead packed with PbO2 as cathode. A 38% solution of sulphuric acid is used as electrolyte. (Density=1.294 g mL-1) The battery holds 3.5 L of the acid. During the discharge of the battery, the density of H2SO4 falls to 1.139 g mL-1. (20% H2SO4 by mass)(1) Write the reaction taking place at the cathode when the battery is in use.(2) How much electricity (in Coulombs) is required to carry out the reduction of one mole of PbO2?(3) What is the molarity of sulphuric acid before discharge?(4) What is the mass of sulphuric acid in the solution after discharge? (5) Write the products of electrolysis when dilute sulphuric acid is electrolysed using platinum electrodes..please explain this step by step..... i will mark u as brainliest answer....​

Answer 1

Explanation:

Here ,

strength of H2SO4 is 5.018 M

we are using secondary cell .

secondary cell are recharged by the electric current here The reaction can be backward direction (reversed) by an external. electrical energy sources , Pb ( lead) storage battery supply is used again and again as they can be charged and discharged .

=>products of anode is oxygen gas

=> products of cathode is hydrogen gas

For the whole solution see the adjoining attachment ...

Thanks.....