Electrolytic Cells

Q.

What is the spontaneous redox reaction?

Q.

What is meant by electrolysis of water

Q.

What is Agar Agar in salt bridge.

Q.

Which of the following is an example of a primary cell?

1. Dry cell

2. Nickel - Cadmium cell

3. Mercury cell

4. Lithium ion cell

Q.

When an aqueous solution of sodium sulphate is electrolysed, on cathode we get:

1. Na

2. SO₃

3. H₂

4. SO₂

Q.

Differentiate between rechargeable and non rechargeable cell

Q. The electrochemical cell shown below is a concentration cell, $M|M^{2+}$ (Saturated solution of a sparingly soluble salt, $M{X}_2\left)||M^{2+}\right(0.001mold{m}^{-3})M.$ The emf of the cell depends on the difference in concentration of $M^{2+}$ ions at the two electrodes. The emf of the cell at 298K is 0.059

The solubility product $(K_{sp}:mo{l}^{3}d{m}^{-9})$ of $M{X}_2$ at 298 K based on the information available the given concentration cell is (take $2.303\times R\times 298/F=0.059V)$

1. $1\times {10}^{-15}$
2. $4\times {10}^{-15}$
3. $1\times {10}^{-12}$
4. $4\times {10}^{-12}$

Q.

Which of the following options is not correct regarding a salt bridge?

1. Contains $N{H}_{4}Cl$.

2. Maintains electrical neutrality of cell.

3. Salt bridge is a straight tube.

4. Contains gelatin.

Q. A galvanic cell converts ______ energy to electrical energy.

1. heat
2. sound
3. chemical
4. light

Q.

Answer in one word.

A device which converts chemical energy to electrical energy.

Q.

Choose the incorrect statement from the following for a Galvanic cell.

1. Electrons flow from cathode to anode.

2. It involves redox reaction.

3. Anode is negative and Cathode is positive.

4. Oxidation occurs at anode.

Q. If a salt bridge is removed between two half cells, then the voltage .

1. doubles
2. does not change
3. drops to zero

Q. The conversion of energy to energy takes place through redox reaction in a galvanic cell.

1. chemical
2. mechanical
3. electrical
4. thermal

Q.

Give one word for the following.

A simple device that maintains the flow of electric current in the circuit.

Q. In a galvanic cell, and happens at anode and cathode respectively.

1. oxidation
2. reduction
3. double displacement
4. combination

Q. How does Galvanic cell work?

Q.

State the transformation of energy in an electric cell.

Q.

The cell reaction in a galvanic cell is

$Cu\left(s\right)+2A{g}^{+}\left(aq\right)\to C{u}^{+2}\left(aq\right)+2Ag\left(s\right)$

Then the incorrect statement is

1. Its cell notation is $Cu|C{u}^{+2}\left(aq\right)||A{g}^{+}\left(aq\right)|Ag$

2. Ag electrode acts as the cathode and Cu electrode acts as the anode

3. electrons flow from copper rod to silver rod through the external circuit

4. Cu electrode is marked positive and Ag electrode is marked negative

Q.

Which of the following can be recharged and used again and again?

1. secondary cell

2. primary cell

Q.

Which of the following can be reused after charging?

1. Dry cell

2. Leclanché cell

3. Voltaic cell

4. Lead acid cell

Q.

Picture of a galvanic cell is given.

a)Identify the anode in the given cell.
b)Write the chemical equation of the reaction taking place at the anode.
c)In which electrode does oxidation take place?

Q. In a galvanic cell, and happens at anode and cathode respectively.

1. combination
2. oxidation
3. double displacement
4. reduction

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

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

Q. Match the following with regard to electrochemical cell

1. cathode
2. anode
3. postive
4. negative

Q.

Study the diagram given below and answer the questions that follow:
(1) Give the names of electrodes A and B.
(2) Which electrode is the oxidising electrode?

Q. An electric current is passed through an aqueous solution of lead(II) chloride. The half-reactions are:
Cathode- ${\text{Pb}}^{x+}\left(\text{aq}\right)+x{e}^{-}\to \text{Pb(s)}$
Anode - ${\text{Cl}}^{-y}\left(\text{aq}\right)\to \text{Cl(s)}+y{e}^{-}$
Find the value of x + y.

1. 3

Q.

who invented the electricity?

Q. An electric current is passed through an aqueous solution of lead(II) chloride. The half-reactions are:
Cathode- ${\text{Pb}}^{x+}\left(\text{aq}\right)+x{e}^{-}\to \text{Pb(s)}$
Anode - ${\text{Cl}}^{-y}\left(\text{aq}\right)\to \text{Cl(s)}+y{e}^{-}$
Find the value of x + y.

1. 3

Q. One mole of $N_2\left(g\right)$ is mixed with 2 moles of $H_2\left(g\right)$ in a 4 litre vessel. If $50$% of $N_2\left(g\right)$ is converted to $H_2\left(g\right)$ by the following reaction :
$N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2{NH}_3\left(g\right)$
What will be the value of $K_c$ for the following equilibrium?
${NH}_3\left(g\right)\rightleftharpoons \frac{1}{2}{N}_2\left(g\right)+\frac{3}{2}{H}_2\left(g\right)$

1. $256$
2. $\frac{1}{16}$
3. $16$
4. none of these

Q.

Differentiate between rechargeable and non rechargeable cell