Representation of Cell

Q. KOLBES ELECTROLYSIS

Q. what is meant by exhaustive electrolysis of water?

Q.

In the cell: Zn, Zn²⁺(aq) || H⁺(aq), H₂(1 atm)Pt, during the working, the p^H around cathode

1. Decreases

2. Increases

3. No change

4. None of these

Q. A voltaic cell is represented as:
$A\left(s\right)|A^{2+}$$\left(aq\right)||B^{2+}$$\left(aq\right)|B\left(s\right)$
Which of the following statements is false regarding the above cell ?

1. None of the above
2. The cell reactions are represented as $A^{2+}\left(aq\right)+2e^{-}\to A\left(s\right)$ and $B\left(s\right)\to B^{2+}\left(aq\right)+2e^{-}$
3. The double vertical line indicates salt bridge
4. A is called the anode and B is called the cathode

Q. One beaker contains 0.15 M $Cd(N{O}_3{)}_2$ and a Cd metal electrode. The other beaker contains 0.20 M $AgN{O}_3$ and a Ag metal electrode. If the reduction potential, $E_{A{g}^{+}/Ag}^0=0.77Vand{E}_{C{d}^{2+}/Cd}^0=-0.40$
The cell representation of a cell is:

1. $Cd\left(s\right)|C{d}^{2+}(aq,0.15M)||A{g}^{+}(aq,0.20M)|Ag\left(s\right)$
2. $A{g}^{+}(aq,0.20M)|Ag\left(s\right)||Cd\left(s\right)|C{d}^{2+}(aq,0.15M)$
3. $C{d}^{2+}|Cd\left(s\right)(aq,0.15M)||Ag\left(s\right)|A{g}^{+}(aq,0.20M)$
4. None of the above.

Q. Which of the following is the cathodic half cell reaction of the given galvanic cell?

1. $Cu\left(s\right)\to C{u}^{2+}\left(aq\right)+2e^{-}$
2. $Ag\left(s\right)\to A{g}^{2+}\left(aq\right)+e^{-}$
3. $2A{g}^{+}\left(aq\right)+2e^{-}\to 2Ag\left(s\right)$
4. $C{u}^{2+}\left(aq\right)+2e^{-}\to Cu\left(s\right)$

Q. In a galvanic cell, 96500 C of + ve charge hours through an external circuit from electrode of higher potential. If the emf of the galvanic cell is 1.0V (i.e, 1.0 J/C), the electrical work done by the cell is

1. 
2. 
3. 
4. 

Q. $F{e}^{3+}\left(aq\right)$ and $I^{-}\left(aq\right)$

Q. The limiting molar conductivities ${\Lambda }^0$
for $NaCl,KBr\text{and}KCl$ are $126,152\text{and}150Sc{m}^{2}mo{l}^{-1}$ respectively. The ${\Lambda }^0$ for $NaBr$ is:

1. $176Sc{m}^{2}mo{l}^{-1}$
   
2. $128Sc{m}^{2}mo{l}^{-1}$
   
3. $302Sc{m}^{2}mo{l}^{-1}$
   
4. $278Sc{m}^{2}mo{l}^{-1}$

Q. Which of the following represents the anode half-cell reaction for the following galvanic cell: $Cu\left(s\right)|C{u}^{2+}\left(aq\right)||A{g}^{+}\left(aq\right)|Ag\left(s\right)$

1. $Cu\left(s\right)+2A{g}^{+}\left(aq\right)\to C{u}^{2+}\left(aq\right)+2Ag\left(s\right)$
2. $Cu\left(s\right)\to C{u}^{2+}\left(aq\right)+2e^{-}$
3. $2A{g}^{+}\left(aq\right)+2e^{-}\to 2Ag\left(s\right)$
4. $A{g}^{+}\left(aq\right)+e^{-}\to Ag\left(s\right)$

Q. What does the double line in the following cell represntation stand for?
$Mg\left(s\right)|M{g}^{2+}\left(aq\right)||A{l}^{3+}\left(aq\right)|Al\left(s\right)$

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

Q. A solution contains $F{e}^{2+},F{e}^{3+}and{I}^{-}ions.$ This solution was treated with iodine at ${35}^{\circ }C.E^0$ for $F{e}^{3+}/F{e}^{2+}is+0.77Vand{E}^{0}for{I}_2/2I^{-}=0.536V.$ The favourable redox reaction is -
( <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> AIPMT MAINS 2011)

1. $F{e}^{2+}\text{will be oxidized to}F{e}^{3+}$
2. $I_2\text{will be the reduced to}{I}^{-}$
3. $I^{-}\text{will be oxidized to}{I}_2$
4. There will be no redox reaction

Q. The limiting molar conductivities ${\Lambda }^0$
for $NaCl,KBr\text{and}KCl$ are $126,152\text{and}150Sc{m}^{2}mo{l}^{-1}$ respectively. The ${\Lambda }^0$ for $NaBr$ is:

1. $128Sc{m}^{2}mo{l}^{-1}$
   
2. $302Sc{m}^{2}mo{l}^{-1}$
   
3. $278Sc{m}^{2}mo{l}^{-1}$
4. $176Sc{m}^{2}mo{l}^{-1}$