Electrochemical Cells, Galvanic Cells

Q.

An electrolytic cell is used to convert ________.

Q.

Are Voltaic Cells Rechargeable?

Q. If $K_{sp}\left(AgCl\right)={10}^{-12}{K}_{sp}\left(AgBr\right)={10}^{-15}$, then the emf of the cell $A{g}_{\left(s\right)}|AgB{r}_{\left(s\right)}|B{r}_{0.4M}^{-}||C{l}_{2M}^{-}|AgC{l}_{\left(s\right)}|A{g}_{\left(s\right)}$ is

1. $0V$
2. $0.04135V$
3. Data insufficient
4. $0.136V$

Q.

What is an Electrolytic cell used to convert?

Q.

Is plasma a superconductor?

Q. Which of the following conversion takes place in a galvanic cell?

1. Electrical energy to chemical energy
2. Chemical energy to electrical energy
3. Chemical energy to mechanical energy
4. Mechanical energy to chemical energy

Q. In a galvanic cell, the salt bridge

1. Does not participate chemically in the cell reaction
2. Stops the diffusion of ions from one electrode to another
3. Minimize the liquid junction potential
4. Ensures mixing of the two electrolytic solution

Q. What is the work of salt bridge?

1. Maintains the electric neutrality in internal circuit.
2. It transfers the electrons from negative rod to positive rod.
3. Cools down the cell by injecting ions into electrolytes.
4. It accelerates the equilibrium.

Q. Match the following with regard to electrochemical cell

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

Q. In the experiment set up for the measurement of EMF of a half cell using a reference electrode and a salt bridge, when the salt bridge is removed, the voltage

1. Does not change
2. Decreases to half the value
3. Increase to maximum
4. Drops to zero

Q. A saturated solution of $KN{O}_3$ is used to make a salt bridge because

1. the velocity of $K^{+}$ is greater than that of $N{O}_3^{-}$
2. the velocity of $K^{+}$ is lesser than that of $N{O}_3^{-}$
3. the velocity of $K^{+}$ and $N{O}_3^{-}$ are nearly the same
4. $KN{O}_3$ is highly soluble in water

Q.

Which of the following is FALSE regarding the salt bridge used in voltaic cells? The salt bridge:

1. allows two half-cells to be separated

2. maintains electrical neutrality in half cells

3. allows mixing of the two electrode solutions

4. allows ions to cross over slowly

Q.

[BHU 1981]

1. Reduction occurs at the copper cathode

2. Oxidation occurs at the copper cathode

3. Reduction occurs at the anode

4. Chemical energy is converted to light energy

Q.

State the property of :
Zinc due to which it is used in dry cells.

Q. All electrolytic cells are electrochemical cells but all elctrochemical cells are not electrolytic cells.

1. True
2. False

Q. Which of the following reaction is correct for a given electrochemical cell at ${25}^{\circ }C$ ?
$Pt\left(s\right)|B{r}^{-}\left(aq\right)|B{r}_2\left(g\right)||C{l}_2\left(g\right)|C{l}^{-}\left(aq\right)|Pt\left(s\right)$

1. $2B{r}^{-}\left(aq\right)+C{l}_2\left(g\right)\to 2C{l}^{-}\left(aq\right)+B{r}_2\left(g\right)$
2. $B{r}_2\left(g\right)+2C{l}^{-}\left(aq\right)\to 2B{r}^{-}\left(aq\right)+C{l}_2\left(g\right)$
3. $B{r}_2\left(g\right)+C{l}_2\left(g\right)\to 2B{r}^{-}\left(aq\right)+2C{l}^{-}\left(aq\right)$
4. $2B{r}^{-}\left(aq\right)+2C{l}^{-}\left(aq\right)\to B{r}_2\left(g\right)+C{l}_2\left(g\right)$

Q. In this electrochemical cell the direction of current is .

1. zinc to copper rod
2. copper to zinc rod
3. anode to cathode

Q.

Assertion : Salts like $KCl,KN{O}_3$ i.e., inert electrolytes are used in salt bridge.

Reason : An inert electrolyte can easily be filled in the U-tube.

1. If both assertion and reason are true and the reason is the correct explanation of the assertion.
2. If both assertion and reason are true but reason is not the correct explanation of the assertion.
3. If assertion is true but reason is false.
4. If the assertion and reason both are false.

Q. Two metal rods A, B are dipped is their ionic solutions respectively.
Following reactions happen at each electrode
$A\to A^{2+}+2e^{-}{B}^{2+}+2e^{-}\to B$
Which of these two rods acquire negative charge

1. A
2. B

Q. In a galvanic cell, the correct statement will be:

1. Current flows from the anode to the cathode
2. Anode is the positive terminal
3. If $E_{cell}<0$, it is a spontaneous reaction
4. Cathode is the positive terminal