If the Emf of the following cell Zn|Zn²⁺ (0.1 M) || Ag⁺ (0.01 M) | Ag at 298 K in V is \(x × 10^{–2}\). Find the value of x is:
(Rounded off to the nearest integer)

\(\begin{aligned} & \text {Given:} ~\mathrm{E}_{{\mathrm{Zn}^{2+}}/ \mathrm{Zn}}=-0.76 \mathrm{~V} \\ & \mathrm{E}_{\mathrm{Ag}^{+} / \mathrm{Ag}}^{\mathrm{o}}=+0.80 \mathrm{~V} ; \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059 \end{aligned}\)

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 p_{2 ,} then the emf is given by:
Pt(H₂) | H⁺(aq) |Pt (H₂)
  p₁       1M        p₂

The magnitude of the change in oxidizing power of the ${\mathrm{MnO}}_4^{-}/{\mathrm{Mn}}^{2+}\text{couple is \hspace{0.17em}}\mathrm{x}\times {10}^{-4}$ , if the H⁺concentration is decreased from 1 M to 10^–4 M at 25°C. (Assume concentration of ${\mathrm{MnO}}_4^{-}\text{and\hspace{0.17em}}{\mathrm{Mn}}^{2+}$to be same on change in H⁺ concentration). The value of x is: 

[Given : $\frac{2.303\mathrm{RT}}{\mathrm{F}}=\mathrm{0.059]}$

1. 3440
2. 3521
3. 3776
4. 3880