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

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

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

1.	1.25 V	2.	-1.75 V
3.	1.75 V	4.	4.0 V

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

What will be the quantity of iron deposited by ferrous and ferric ion by 1F (Fe = 56)

(1) 14g, 9.3 g                                          

(2) 28g, 18.6 g

(3) 56g, 37.2g                                         

(4) None of these

The unit of specific conductance is:

What is the value of 

$p{K}_b (C{H}_{3}CO{O}^{-} )$
$if {\lambda }_m^0= 390 \& {\lambda }_m = 7.8$
$for 0.04 of a C{H}_{3}COOH at 25°C$

(A) 9.3                                               

(B) 9.2

(C) 4.7                                               

(D) 4.8

Given that a certain electric current generates 0.504 grams of hydrogen in 2 hours. How many gram of mass of copper can be liberated by the same current when applied for the same duration in a solution of CuSO₄?

1. 12.7

2. 16

3. 31.8

4. 63.5