Emf of the following cell at 298 K in V is x × 10^–2 . The cell is Zn|Zn²⁺ (0.1 M) || Ag⁺ (0.01 M) | Ag. The value of x is-
(Rounded off to the nearest integer)
\(\begin{aligned} & \text { Given; } \mathrm{E}_{\mathrm{Zn}^{2+}}^{\mathrm{o}} / \mathrm{Zn}=-0.76 \mathrm{~V} \\ & \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=+0.80 \mathrm{~V} ; \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \end{aligned}\)

1. 157
2. 147
3. 144
4. 154

For the given cell :

$\mathrm{Cu}\left(\mathrm{s}\right)\left|{\mathrm{Cu}}^{2+}\left({\mathrm{C}}_1\mathrm{M}\right)\right|\left|{\mathrm{Cu}}^{2+}\left({\mathrm{C}}_2\mathrm{M}\right)\right|\mathrm{Cu}\left(\mathrm{s}\right)$ change in Gibbs energy $\left(∆\mathrm{G}\right)$ is negative, if:

1. ${\mathrm{C}}_1=2{\mathrm{C}}_2$

2. ${\mathrm{C}}_2=\raisebox{1ex}{${\mathrm{C}}_1$}\!\left/ \!\raisebox{-1ex}{$\sqrt{2}$}\right.$

3. ${\mathrm{C}}_1={\mathrm{C}}_2$

4. ${\mathrm{C}}_2=\sqrt{2}{\mathrm{C}}_1$

The reduction potential of hydrogen half-cell will be negative if:

1. P(H₂) = 1atm and [H⁺] = 2.0 M

2. P(H₂) = 1 atm and [H⁺] = 1.0 M

3. P(H₂) = 2 atm and [H⁺] = 1.0 M

4. P(H₂) = 2 atm and [H⁺] = 2.0 M

For the following cell with hydrogen electrodes at two different pressures p₁ and p₂ 
Pt(H₂) | H⁺(aq) |Pt (H₂)
  p₁         1M        p₂   
emf  is given by:

1. \(\frac{R T}{F} \log _{e} \frac{P_{1}}{p_{2}}\)
2. \(\frac{R T}{2F} \log _{e} \frac{P_{1}}{p_{2}}\)
3. \(\frac{R T}{F} \log _{e} \frac{P_{2}}{p_{1}}\)
4. \(\frac{R T}{2F} \log _{e} \frac{P_{2}}{p_{1}}\)