Electrochemistry

For the electrochemical reaction, Zn + Cu2+ -> Zn2+ + Cu, given E°(Zn2+/Zn) = -0.76 V and E°(Cu2+/Cu) = +0.34 V, the standard cell potential is:

1. -1.10 V
2. 0.42 V
3. 1.10 V
4. 0.76 V

Rusting of iron is an example of:

1. Electroplating
2. Electrolysis
3. Corrosion
4. Reduction

In a hydrogen-oxygen fuel cell, the main product formed is:

1. Hydrogen peroxide
2. Water
3. Ozone
4. Sulfuric acid

Which of the following is a secondary (rechargeable) battery?

1. Dry cell
2. Mercury cell
3. Lead-acid storage battery
4. Zinc-carbon cell

Which of the following statements correctly distinguishes a galvanic cell from an electrolytic cell?

1. Both convert electrical energy into chemical energy.
2. A galvanic cell converts chemical energy into electrical energy, whereas an electrolytic cell converts electrical energy into chemical energy.
3. A galvanic cell requires an external power source, whereas an electrolytic cell does not.
4. Oxidation occurs at the cathode in both cells.

A current of 2 A is passed through an electrolytic solution for 30 minutes. The quantity of electricity passed is:

1. 1200 C
2. 1800 C
3. 3600 C
4. 7200 C

According to Faraday's First Law of Electrolysis, the mass of a substance deposited is directly proportional to:

1. Resistance of the electrolyte
2. Current only
3. Quantity of electricity passed
4. Potential difference

According to Kohlrausch's law, the limiting molar conductivity of an electrolyte is equal to:

1. Product of ionic conductivities
2. Sum of the limiting ionic conductivities of its constituent ions
3. Difference of ionic conductivities
4. Average ionic conductivity

Molar conductivity is related to conductivity by the expression:

1. Lambda m = kappa x C/1000
2. Lambda m = kappa x 1000/C
3. Lambda m = C/kappa
4. Lambda m = kappa/C^2

The SI unit of conductivity (kappa) is:

1. S cm^-1
2. S m^-1
3. ohm cm
4. ohm^-1 cm^2

The primary function of the salt bridge in a galvanic cell is to:

1. Supply electrons to the electrodes.
2. Increase the cell potential.
3. Maintain electrical neutrality by allowing ion migration.
4. Prevent oxidation at the anode.

The relation between Gibbs free energy and cell potential is:

1. Delta G = nFEcell
2. Delta G = -nFEcell
3. Delta G = Ecell/F
4. Delta G = n/Ecell

The Nernst equation at 298 K is:

1. Ecell = E°cell + (0.0591/n) log Q
2. Ecell = E°cell - (0.0591/n) log Q
3. Ecell = E°cell - nF
4. Delta G = -nFEcell

The standard cell potential is calculated using the relation:

1. E°cell = E°anode - E°cathode
2. E°cell = E°cathode - E°anode
3. E°cell = E°anode + E°cathode
4. E°cell = E°cathode/E°anode

In a galvanic (voltaic) cell, oxidation takes place at the:

1. Cathode
2. Salt bridge
3. Anode
4. Electrolyte