Which of the following expressions is used to find the cell potential of the $Cd_{(s)} | Cd_{(aq)}^{2+} || Cu_{(aq)}^{2+} | Cu_{(s)}$ cell at $25^{\circ} C$?

Derive the Nernst equation for calculating $E_{cell}$ of a Daniell cell and explain the effect on $E_{cell}$ when there is a change in the concentration of $Zn^{2+}$ and $Cu^{2+}$ ions.

For the cell reaction with the indicated concentrations
$Al_{(s)} + 3Ag^{+}_{(aq)} \, (0.10 \, M) \to Al^{3+}_{(aq)} \, (0.30 \, M) + 3Ag_{(s)}$,
the measured voltage $(E_{cell})$ is $1.50 \, V$. Calculate $E^o_{cell} \, ........... \, V$
Given: $\frac{2.303 \, RT}{F} = 0.06 \, V ; \, \log \, 3 = 0.48$

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. $A$ simple model for such a concentration cell involving a metal $M$ is:
$M_{(s)} \mid M^{+}(aq; 0.05 \ M) \parallel M^{+}(aq; 1 \ M) \mid M_{(s)}$
For the above electrolytic cell the magnitude of the cell potential $|E_{cell}|=70 \ mV$.
$1.$ For the above cell
$(A)$ $E_{cell} < 0 ; \Delta G > 0$ $(B)$ $E_{cell} > 0 ; \Delta G < 0$
$(C)$ $E_{cell} < 0 ; \Delta G^{\circ} > 0$ $(D)$ $E_{cell} > 0 ; \Delta G^{\circ} > 0$
$2.$ If the $0.05 \ M$ solution of $M^{+}$ is replaced by $0.0025 \ M$ $M^{+}$ solution,then the magnitude of the cell potential would be
$(A)$ $35 \ mV$ $(B)$ $70 \ mV$ $(C)$ $140 \ mV$ $(D)$ $700 \ mV$
Give the answer for questions $1$ and $2$.

The pressure of $H_2$ required to make the potential of $H_2$-electrode zero in pure water at $298 \ K$ is

Write the Nernst equation for the $E_{cell}$ reaction in the Daniell cell. How will the $E_{cell}$ be affected when the concentration of $Zn^{2+}$ ions is increased?