By how much will the potential of half cell Cu²⁺| Cu change if the solution is diluted to 100 times at 298 K. It will -

1.	Increase by 59 mV	2.	Decrease by 59 mV
3.	Increase by 29.5 mV	4.	Decrease by 29.5 mV

What will be the molar conductance at infinite dilution for NH₄OH. If at infinite dilution the molar conductances of Ba(OH)₂, BaCl₂ and NH₄Cl are 523.28, 280.0 and 129.8 ohm^-1 cm^-1 mol^-1 respectively.
1. 502.88
2. 373.68
3. 251.44
3. 226.96

At 25$°$C the specific conductance of sturated solution of AgCl is 2.3 X 10-6 ohm^-1cm^-1. What will be the solubility of AgCl at 25$°$C if ionic conductances of ${\mathrm{Ag}}^{\oplus }$ and ${\mathrm{Cl}}^{⊝}$ at infinite dilution are 61.9 and 76.3 ohm^-1cm²mol^-1 respectively.

1. 1.66 X 10^-11M

2. 3.18 X 10^-6M

3. 6.01 X 10^-5M

4. 1.66 X 10^-5M

$2{\stackrel{\oplus }{\mathrm{Ag}}}_{\left(\mathrm{aq}\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{Cu}}_{\left(\mathrm{s}\right)}<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons }<mspace\; width="1em"></mspace>{{\mathrm{Cu}}_{\left(\mathrm{aq}\right)}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$

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 ${\mathrm{Cu}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Fe}<mspace\; width="1em"></mspace>\stackrel{<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>}{\rightleftharpoons }<mspace\; width="1em"></mspace>{\mathrm{Fe}}^{+2}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>\mathrm{Cu}<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>$

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

(1) -65.62 KJ

(2) -75.27 KJ

(3) -150.54 KJ

(4) +150.54 KJ

At 298 K the Emf of the following cell is:

\(\small{Pt|H_{2}(1 \ atm)|H^{+}(0.02 \ M) \ || \ H^{+}(0.01 \ M)|H_{2}(1 \ atm)|Pt}\)

1. - 0.017 V

2. 0.0295 V

3. 0.1 V

4. 0.059 V

At 25$°$C temperature Zn electrode is placed in 0.1M solution of zinc salt then what will be the reduction potential ? If it is assumed that salt dissociates 25% at this dilution (${\mathrm{E}}_{\raisebox{1ex}{${\mathrm{Zn}}^{2+}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Zn}$}\right.}^{°}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>-0.76<mspace\; width="1em"></mspace>\mathrm{V}$)

(1) -0.713 V

(2) - 0.81 V

(3) + 0.778 V

(4) - 0.84 V

The reduction potential of Hydrogen electrode is -118mV then the concentration of ${\mathrm{H}}^{\oplus }$ion in solution will be :-

(1) 10^-4M

(2) 2M

(3) 0.01M

(4) 10^-3M

The maximum work which can be obtained from a Daniel cell \(Zn_{(s)}\ |\ Zn^{+2}_{(aq)}\ || Cu^{+2}_{(aq)}\ |\ Cu_{(s)}\) is:

1. +106.15 kJ

2. -212.3 kJ

3. -424.6 kJ

4. +212.3 kJ

CuSO₄ solution is treated separately with KCl and KI. In which case, Cu⁺² will be reduced to ${\mathrm{Cu}}^{\oplus }$ ?

(1) with KCl

(2) with KI

(3) with KCl and KI both

(4) None of these