Representation of Cell

Q. With respect to the salt bridge in the cell representation, which of the following statements is correct?

1. Anode is at the left and cathode at the right
2. Anode is at the right and cathode at the left
3. Anode and cathode are seperated by symbol "|" which denotes the presence of salt bridge
4. All of the above

Q. The cell reaction for the given cell is spontaneous if $Pt,C{l}_{2_{\left(P_1\right)}}\left(g\right)|C{l}^{-}\left(1.0M\right)||C{l}^{-}\left(2M\right)|C{l}_{2_{\left(P_2\right)}}\left(g\right),Pt$

1. $P_1>P_2$
2. $2P_1<P_2$
3. $P_1=P_2$
4. $2P_2>P_1$

Q. Construct galvanic cells from the following pairs of half cells and calculate their emf at ${25}^{o}C.$

$C{d}^{2+}(aq,1M)\mid Cd\left(s\right);E_{C{d}^{2+}/Cd}^0=-0.40V$

$H{g}_{2}C{l}_2\left(s\right)\mid Hg\left(l\right)\mid C{l}^{-}(aq,0.1M);E_{C{l}^{-}/H{g}_{2}C{l}_2/Hg}^0=0.28V$

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.

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. For a spontaneous cell reaction, the sign of $\Delta G^0$ and $E_{cell}^0$ will be respectively:

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. The notation to indicate a boundary between two phases in a electro- chemical cell is

1. |
2. /
3. | |
4. \