$2{\stackrel{\oplus }{\mathrm{Ag}}}_{\left(\mathrm{aq}\right)} + {\mathrm{Cu}}_{\left(\mathrm{s}\right)} \stackrel{ }{\rightleftharpoons } {{\mathrm{Cu}}_{\left(\mathrm{aq}\right)}}^{+2} + 2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

The cell potential for this reaction is 0.46V. Which of the following change will increase the potential the most ?

(1) $\left[\stackrel{\oplus }{\mathrm{Ag}}\right]$ concentration is doubled

(2) [Cu²⁺] concentration is halved

(3) Size of Cu_(s) electrode is doubled

(4) size of Ag_(s) electrode is decreased to half

What will be the value of $∆\mathrm{G}°$ for the rection ${\mathrm{Cu}}^{+2} + \mathrm{Fe} \stackrel{ }{\rightleftharpoons } {\mathrm{Fe}}^{+2} + \mathrm{Cu} ,$

if ${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Cu}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Cu}$}\right.}^{\circ } = +0.34 \mathrm{V} \mathrm{and} {\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Fe}}^{+2}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{\circ } = -0.44 \mathrm{V}$$$

(1) -65.62 KJ

(2) -75.27 KJ

(3) -150.54 KJ

(4) +150.54 KJ

The cell reaction of micro electrochemical cell fromed during rusting of iron is:-

For the cell reaction

${\mathrm{Cu}}_{{\mathrm{c}}_1}^{+2} \left(\mathrm{aq}\right) +\hspace{0.17em}\mathrm{Zn}\left(\mathrm{s}\right) \stackrel{ }{\to } {\mathrm{Zn}}_{{\mathrm{C}}_2}^{+2} \left(\mathrm{aq}\right) + \mathrm{Cu}\left(\mathrm{s}\right)$

the change in free energy at a given temperature is a function of 

(1) $\mathcal{l}$nC₁

(2) $\mathcal{l}$n$\frac{{\mathrm{C}}_2}{{\mathrm{C}}_1}$ 

(3) $\mathcal{l}$n (C₁ +C₂)

(4) $\mathcal{l}$nC₂

${\mathrm{}}_{}^{}$The Emf of the following voltaic cell is:$$

\(\text {Ni }| \text {Ni}^{2+} (1 \text M) || \text {Au} ^{+3} \text {(1M) |Au}\)

\(\left ({~\mathrm{E}_{{\mathrm{Ni}^{+2}}/{\mathrm{Ni}}}^0=-0.25 \mathrm{~V}, \mathrm{E}_{{\mathrm{Au}^{+3}}/{\mathrm{Au}}}^0=1.50 \mathrm{~V}}\right )\)

The same amount of electric current is apassed through aqueous solution of MgSO₄ and AlCl₃. If 2.8 g Mg metal is deposited at amount of Al metal deposited in second cell will be

(1) 2.1 g

(2) 2.49 g

(3) 3.15 g

(4) 3.73g

A device that converts energy of combustion of fuels like hydrogen and methane, directly into electrical energy is known as

(1) fuel cell
(2) electrolytic cell
(3) dynamo
(4) Ni-Cd cell

$F_2$ gas can’t be obtained by the electrolysis of any $F^{-1}$salt because-

(A) Fluorine is the strongest reducing agent

(B) Fluorine is the strongest oxidising agent.

(C) Fluorine easily combine with atmospheric $O_2$

(D) All

If the E°_cell for a given reaction has a negative value then which of the following gives the correct relationships for the values of $∆$G° and K_eq?

(a) $∆$G° < 0;K_eq > 1

(b) $∆$G° < 0; K_eq < 1

(c) $∆$G°> 0; K_eq < 1

(d) $∆$G° > 0; K_eq > 1

Acetic acid has K_a = 1.8 × 10^–5 while formic acid had K_a = 2.1 × 10^–4. What would be the magnitude of the emf of the cell

Pt(H₂) $\left|\begin{array}{l}0.1\mathrm{M} \mathrm{acetic} \mathrm{acid}+\\ 0.1\mathrm{M} \mathrm{sodium} \mathrm{acetate}\end{array}\right|\left|\begin{array}{l}0.1\mathrm{M} \mathrm{formic} \mathrm{acid}+\\ 0.1\mathrm{M} \mathrm{sodium} \mathrm{formate}\end{array}\right|$ Pt(H₂) at 25°C

(1) 0.0315 volt

(2) 0.0629 volt

(3) 0.0455 volt

(4) 0.0545 volt