Previous Year Papers

Download Solved Question Papers Free for Offline Practice and view Solutions Online.

Test Series

Take Zigya Full and Sectional Test Series. Time it out for real assessment and get your results instantly.

Test Yourself

Practice and master your preparation for a specific topic or chapter. Check you scores at the end of the test.

Electrochemistry

Short Answer Type

1. How would you determine the standard electrode potential of the system Mg²⁺/Mg?

2203 Views

2. Can you store copper sulphate solutions in a Zinc pot?

1384 Views

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

879 Views

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

1279 Views

Long Answer Type

5. Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M) $\to$ Ni²⁺ (0.160 M) + 2Ag(s)
Given that ${E^{o}}_{Cell} = 1.05 V$

Answer:

Ni (s) + 2 {Ag}^{+} (aq) \to {Ni}^{2 +} (aq) + 2 As (s)

E_{cell} = {E^{o}}_{cell} + \frac{RT}{2 F} \ln \frac{{[{Ag}^{+} (aq)]}^{2}}{[{Ni}^{2 +} (aq)]}

E_{cell} = {E^{o}}_{cell} + \frac{0.059}{2} \log \frac{{[{Ag}^{+} (aq)]}^{2}}{[{Ni}^{2 +} (aq)]}

The equation is also written as

or

E_{cell} = {E^{o}}_{cell} - \frac{0.059}{2} \log \frac{[{Ni}^{2 +} (aq)]}{{[{Ag}^{+} (aq)]}^{2}} = 1.05 V - 0.0295 \log \frac{0.160}{0.002}

= 1.05 V – 0.0295 x log 80

= 1.05 V – 0.0295 x 1.9031

= 1.05 V – 0.056 = 0.99 V.

1585 Views

6. The cell in which the following reaction occurs:
2Fe³⁺ (aq) + 2I^–(aq)

\to

2Fe²⁺ (aq) + I₂(s) has E⁰_cell = 0.236 V at 298 K. Calculate the standerd Gibbs energy and the equilibrium constance of the cell reaction.

919 Views

Short Answer Type

7. Why does the conductivity of a solution decrease with dilution?

233 Views

8. Suggest a way to determine the Λ°_m value of water.

175 Views

Long Answer Type

9. The molar conductivity of 0.025 mol L^–1methanoic acid is 46.1 S cm² mol^–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H⁺) = 349.6 S cm²mol^–1 and λ° (HCOO^– ) = 54.6 s cm² mol^–1.

225 Views

Short Answer Type

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

198 Views

Previous Year Papers

Test Series

Test Yourself

Short Answer Type

Long Answer Type

5. Calculate the emf of the cell in which the following reaction takes place:Ni(s) + 2Ag+ (0.002 M) → Ni2+ (0.160 M) + 2Ag(s)Given that EoCell = 1.05 V

Short Answer Type

Long Answer Type

Short Answer Type

5. Calculate the emf of the cell in which the following reaction takes place:
Ni(s) + 2Ag⁺ (0.002 M) $\to$ Ni²⁺ (0.160 M) + 2Ag(s)
Given that ${E^{o}}_{Cell} = 1.05 V$