Free NCERT Solutions For Class 12 Chemistry Chapter 3 : Electrochemistry Free PDF Download

Intext Questions

Question 1:
How would you determine the standard electrode potential of the system Mg2+1 Mg?

Question 2:
Can you store copper sulphate solutions in a zinc pot?

Question 3:
Consult the table of standard electrode potentials and suggest three substances that can oxidize ferrous ions under suitable conditions.

Solution 3:

Question 4:
Calculate the potential of hydrogen electrode in contact with a solution whose pH is 10.

Question 7:
Why does the conductivity of solution decrease with dilution?

Question 10:
If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?

Question 13:
Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.

Question 15:
Explain how rusting of iron is envisaged as setting up of an electro chemical cell

NCERT EXERCISES

Question 1:
Arrange the following metals in the order in which they displace each other from the solution of their salts: Al, Cu, Fe, Mg and Zn

Question 4:
Calculate the standard cell potentials of galvanic cell in which the following reactions take place

Question 6:
In the button cells widely used in watches and other devices the following reaction takes places:

Question 7:
Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their variation with concentration.

Question 8:
The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm-1 . Calculate its molar conductivity.

Solution 8:

Question 13:
How much electricity in terms of Faraday is required to produce.
(i) 20.0 g of Ca from molten CaCl2?
(ii) 40.0 g of Al from molten Al2O3?

Question 14:
How much electricity is required in coulomb for the oxidation of
(i) 1 mol of H2O to O2
(ii) 1 mol of FeO to Fe2O3

Question 16:
Three electrolytic cells, A, B, C containing solutions of ZnSO4, AgNO3 and CuSO4 , respectively are connected in series. A steady current of 1.5 amperes was passed through them until 45 g of silver deposited at the cathode of cell B. How long did the current flow? What mass of copper and zinc were deposited?

Question 18:
Predict the products of electrolysis in each of the following .
(i) An aqueous solution of AgNO3 with silver electrodes.
(ii) An aqueous solution of AgNO3 With platinum electrodes.
(iii) A dilute solution of H2SO4 with platinum electrodes.
(iv) An aqueous solution of CuCl2 with platinum electrodes.