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In the Hall process, aluminium is produced by the electrolysis of molten ${\mathrm{Al}}_2{\mathrm{O}}_3$ by the following reactions. How many second would it take to produce enough aluminum by the Hall process to make a case of 24 cans of aluminium soft-drink, if each can uses 5.0 g of Al, a current of 9650 amp is employed, and the current efficiency of the cell is 90.0%:
(1) 203.2
(2) 148.14
(3) 333
(4) 6.17

Consider the reaction given below:
$2{\mathrm{CH}}_3{\mathrm{COO}}^{-}\to {\mathrm{C}}_2{\mathrm{H}}_6\left(\mathrm{g}\right)+2{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}$
The electrolysis of acetate solution produces ethane. The current efficiency of the process is 80%. What volume of gases would be produced at 27$°\mathrm{C}$ and 740 torr, if the current of 0.5 amp is passed through the solution for 96.45 min?
1. 6.0 L
2. 0.60 L
3. 1.365 L
4. 0.91 L

100 mL of 0.05 M ${\mathrm{CuSO}}_4\left(\mathrm{aq}\right)$ solution was electrolyzed using inert electrodes by passing current till the pH of the resulting solution was 2. The solution after electrolysis was neutralized and then treated with excess KI and formed ${\mathrm{I}}_2$ titrated with 0.04 M ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3.$
Calculate the required volume (in mL) of ${\mathrm{Na}}_2{\mathrm{S}}_2{\mathrm{O}}_3$:
(1) 112.5 mL
(2) 100 mL
(3) 125 mL
(4) None of these

If the equilibrium constant for the reaction${\mathrm{H}}^{+}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right) \mathrm{is} {10}^{13}$ at certain temperature then what is the ${\mathrm{E}}^{°}$ for the reaction, $2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+2{\mathrm{e}}^{-}\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right)+2{\mathrm{OH}}^{-}\left(\mathrm{aq}\right)$
$\mathrm{Given}: \frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.066$
(1) 1.230 V
(2) -0.858 V
(3) -0.80 V
(4) -0.8274 V

A fuel cell develops an electrical potential from the combustion of butane at 1 bar and 298 K 
C₄H₁₀(g) + 6.5O₂(g) → 4 CO₂(g) + 5H₂O(l); E^o  of a cell is: 
(Given $∆G^o$ $=-\mathrm{2746 }kJ/mole$ )
1. 4.74 V
2. 0.547 V
3. 4.37 V
4. 1.09 V

$\Delta f{H^{\circ }}_{298}+T.\Delta {S^{\circ }}_{298}=(-474.78)+298\times (-0.32)$
$\Delta f{H^{\circ }}_{298}=-378.07kJ/mol$
Given: ${\mathrm{O}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+4{\mathrm{e}}^{-}\to 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right);\mathrm{E}°=1.23 \mathrm{V}$
(1) -285.07 kJ/mol
(2) -570.14 kJ/mol
(3) 285.07 kJ/mol
(4) None of these

The standard reduction potential of normal calomel electrode and reduction potential of saturated calomel electrodes are 0.27 and 0.33 volt respectively. What is the concentration of Cl^- in saturated solution of KCl?
(1) 0.1 M
(2) 0.01 M
(3) 0.001 M 
(4) None

Copper reduces ${\mathrm{NO}}_3^{-}$ into NO and ${\mathrm{NO}}_2$ depending upon concentration of ${\mathrm{HNO}}_3$ in solution. Assuming $\left[{\mathrm{Cu}}^{2+}\right]=0.1 \mathrm{M}, \mathrm{and} {\mathrm{P}}_{\mathrm{NO}}={\mathrm{P}}_{{\mathrm{NO}}_2}={10}^{-3}$ bar. At which concentration of ${\mathrm{HNO}}_3$, thermodynamic tendency for reduction of ${\mathrm{NO}}_3^{-}$ into NO and ${\mathrm{NO}}_2$ by copper is same?
$[\mathrm{Given}: {\mathrm{E}}_{{\mathrm{Cu}}^{2+}|\mathrm{Cu}}^{°}=+0.34 \mathrm{volt}, {\mathrm{E}}_{{\mathrm{NO}}_3^{-}|\mathrm{NO}}^{°}=+0.96 \mathrm{volt},$
${\mathrm{E}}_{{\mathrm{NO}}_3^{-}|{\mathrm{NO}}_2}^{°}=+0.79 \mathrm{volt}$
(1) ${10}^{1.23} \mathrm{M}$
(2) ${10}^{0.56} \mathrm{M}$
(3) ${10}^{0.66} \mathrm{M}$
(4) ${10}^{0.12 }\mathrm{M}$

The chorate ion can disproportionate in basic solution according to reaction,
$2{\mathrm{ClO}}_3^{-}\rightleftharpoons {\mathrm{ClO}}_2^{-}+{\mathrm{ClO}}_4^{-}$
What is the equilibrium concentration of perchlorate ions from a solution initially at 0.1 M in chlorate ions at 298 K?
$\mathrm{Given}: {\mathrm{E}}_{{\mathrm{ClO}}_4^{-}|{\mathrm{ClO}}_3^{-}}^{°}=0.36 \mathrm{V} \mathrm{and} {\mathrm{E}}_{{\mathrm{ClO}}_3^{-}|{\mathrm{ClO}}_2^{-}}^{°}=0.33 \mathrm{V} \mathrm{at} 298 \mathrm{K}$
(1) 0.019 M
(2) 0.024 M
(3) 0.1 M
(4) 0.19 M

Equivalent conductivity of ${\mathrm{BaCl}}_2, {\mathrm{H}}_2{\mathrm{SO}}_4 \mathrm{and} \mathrm{HCl} \mathrm{are} {\mathrm{x}}_1, {\mathrm{x}}_2 \mathrm{and} {\mathrm{x}}_3 {\mathrm{Scm}}^{-1} {\mathrm{eq}}^{-1}$ at infinite dilution. If conductivity of saturated ${\mathrm{BaSO}}_4$ solution is x ${\mathrm{Scm}}^{-1}, \mathrm{then} {\mathrm{K}}_{\mathrm{sp}} \mathrm{of} {\mathrm{BaSO}}_4$ is:
(1) $\frac{500\mathrm{x}}{({\mathrm{x}}_1+{\mathrm{x}}_2-2{\mathrm{x}}_3)}$
(2) $\frac{{10}^6{\mathrm{x}}^2}{{\left({\mathrm{x}}_1+{\mathrm{x}}_2-2{\mathrm{x}}_3\right)}^3}$
(3) $\frac{2.5\times {10}^5{\mathrm{x}}^2}{{\left({\mathrm{x}}_1+{\mathrm{x}}_2-{\mathrm{x}}_3\right)}^2}$
(4)  $\frac{0.25{\mathrm{x}}^2}{{\left({\mathrm{x}}_1+{\mathrm{x}}_2-{\mathrm{x}}_3\right)}^2}$

The ionization constant of a weak acid is $1.6\times {10}^{-5}$ and the molar conductivity at infinite dilution is $380\times {10}^{-4} {\mathrm{Sm}}^2 {\mathrm{mol}}^{-1}$. If the cell constant is 0.01 ${\mathrm{m}}^{-1}$ then conductance of 0.01 M acid solution is:
(1) $1.52\times {10}^{-5} \mathrm{s}$
(2) 1.52 s
(3) $1.52\times {10}^{-3} \mathrm{s}$
(4) $1.52\times {10}^{-4} \mathrm{s}$

Three electrolytic cells X, Y, Z containing solution of NaCl, ${\mathrm{AgNO}}_3 \mathrm{and} {\mathrm{CuSO}}_4$ respectively are connected in series combination. During electrolysis 21.6 gm of silver deposite at cathode in cell Y. Which is incorrect statement.
(1) 6.35 gm copper deposite at cathode in cell Z
(2) 2.24 litre ${\mathrm{Cl}}_2$ liberated at 1 atm and 273 K at cathode in cell X
(3) 2.24 litre ${\mathrm{O}}_2$ liberated at 1 atm and 273 K at anode in cell Y
(4) 2.24 litre ${\mathrm{H}}_2$ liberated at 1 atm and 273 K at cathode in cell X

$$\begin{gathered} \mathrm{Zn}\left(\mathrm{s}\right)\left|\mathrm{Zn}{{\left(\mathrm{CN}\right)}_4}^{2-}\left(0.5\mathrm{M}\right),{\mathrm{CN}}^{-}\left(0.01\right)\right| \\ \left|\mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_4^{2+}\left(0.5\mathrm{M}\right), {\mathrm{NH}}_3\left(\mathrm{M}\right)\right|\mathrm{Cu}\left(\mathrm{s}\right) \\ \mathrm{Given}: {\mathrm{K}}_{\mathrm{f}} \mathrm{of} \mathrm{Zn}{{\left(\mathrm{CN}\right)}_4}^{2-}={10}^{16} , \\ {\mathrm{K}}_{\mathrm{f}} \mathrm{of} \mathrm{Cu}{\left({\mathrm{NH}}_3\right)}_4^{2+}={10}^{12}, \\ \mathrm{E}°\mathrm{Zn}\overline{){\mathrm{Zn}}^{+2}=0.76\mathrm{V} ;} \\ \mathrm{E}{°}_{{\mathrm{Cu}}^{+2}\overline{)\mathrm{Cu}}}=0.34\mathrm{V}, \frac{2.303\mathrm{RT}}{\mathrm{F}}=0.06 \end{gathered}$$
The emf of the above cell is:
(1) 1.22 V
(2) 1.10 V
(3) 0.98 V
(4) None of these