Exp.3: Electrochemistry

Spontaneous redox reaction.

Generates electricity.

The above are characters of .....

• Galvanic cell

• Electrolytic cell

In both galvanic cell and electrolytic cell, reduction happens at ...

• Anode

• Cathode

Al³⁺ (aq) + 3e → Al (s) E^o_red= -1.66 V

Cu²⁺ (aq) + 2e → Cu (s) E^o_red= +0.34 V

Fe²⁺ (aq) + 2e → Fe (s) E^o_red= -0.44 V

Mg²⁺ (aq) + 2e → Mg (s) E^o_red= -2.37 V

Zn²⁺ (aq) + 2e → Zn (s) E^o_red= -0.76 V

Arrange the metal in ascending order of strength as reducing agent.

• Al < Cu < Fe < Mg < Zn

• Zn < Mg < Fe < Cu < Al

• Mg < Al < Zn < Fe < Cu

• Cu < Fe < Zn < Al < Mg

Standard Reduction Potential is measured at which condition?

• Pressure 1 atm

• Temperature 0^oC

• Concentration 1 M

• Current 1A

This formula is used to calculate cell potential at non-standard condition.

This formula is known as ______ equation.

Which of this measuring device is used for electrolytic cell?

• Ammeter

• Voltmeter

What is the function of salt bridge?

• To maintain electrical neutrality

• To increase oxidation number

• To complete the circuit

• To connect the electrodes

The mass of copper deposited in electrolytic cell in exp.B can be determined using .....

• Standard Reduction Potential Table

• Nernst equation

• Faraday's first law

Theoretically, 1 Faraday is equilavent to _____ Coulomb.

The amount of substance formed at electrodes in electrolytic cell is proportional to ..

• Time taken for the electrolysis to be run.

• Amount of current used.

• The initial mass of the electrode