Electrolytic Cell

Q. When a lead storage battery is charged, it acts as:

1. A fuel cell
2. An electrolytic cell
3. A galvanic cell
4. A concentration cell

Q.

The salt bridge in the electrochemical cell serves to

1. accelerate the attainment of equilibrium

2. increase the voltage of the cell

3. maintain electrical neutrality

4. increase the oxidation/reduction rate

Q.

In an electrolytic cell the electrode at which the electrons enter is called the___; the chemical change that occurs at this electrode is called___.

1. Anode, oxidation
2. Anode, reduction
3. Cathode, oxidation
4. Cathode, reduction

Q. What is the direction of flow of electrons in an electrolytic cell?

Q. Which of the following statements are true about an electrolytic cell?

1. The reaction is non-spontaneous
2. A potential equal to the cell potential needs to be applied.
3. The flow of electrons is from anode to cathode.
4. The flow of current is from anode to cathode.

Q.

In the electrolytic cell, flow of electrons is fron:

1. Cathode to anode in solution

2. Cathode to anode through external supply

3. Cathode to anode through solution

4. Anode to cathode through external supply

Q. $\begin{array}{cccc}& \text{List - I}& & \text{List - II}\\ \text{(P)}& \text{Very dilute solution of HCl}& \text{(1)}& O_2\text{evolved at anode}\\ \text{(Q)}& \text{Very dilute solution of KCl}& \text{(2)}& H_2\text{evolved at cathode}\\ \text{(R)}& \text{Concentrated solution of NaCl}& \text{(3)}& C{l}_2\text{evolved at anode}\\ \text{(S)}& \text{Fairly concentrated solution of}AgN{O}_3& \text{(4)}& \text{Na deposition at cathode}\\ & & \text{(5)}& \text{Ag deposition at cathode}\\ & & \text{(6)}& \text{K deposition at cathode}\end{array}$
Match each product in LIST-I with one or more reaction in LIST-II and choose the correct option.

1. $P\to 1,2;Q\to 1,2;R\to 2,3;S\to 1,5$
2. $P\to 1,2;Q\to 2,3;R\to 2,3;S\to 1,5$
3. $P\to 2,3;Q\to 3,6;R\to 3,4;S\to 1,5$
4. $P\to 2,3;Q\to 3,6;R\to 2,3;S\to 2,5$

Q. An electric current is passed through an aqueous solution of lead(II) chloride. What are the half-reactions those takes place at the cathode and anode?

1. $Anode:P{b}^{2+}+2e^{-}\to Pb;Cathode:C{l}^{-}\to Cl+e^{-}$
2. $Anode:P{b}^{2+}+2e^{-}\to Pb;Cathode:Cl\to C{l}^{+}+e^{-}$
3. $Cathode:P{b}^{2+}\to P{b}^{+}+2e^{-};Anode:C{l}^{-}\to Cl+e^{-}$
4. $Anode:Pb\to P{b}^{2+}+2e^{-};Cathode:C{l}^{-}\to Cl+e^{-}$

Q.

Electrolysis involves oxidation and reduction respectively at

[CPMT 1973; AMU 1983; NCERT 1983, 84; MH CET 2001]

1. Anode and cathode

2. Cathode and anode

3. At both the electrodes

4. None of the above