The specific conductivity of a solution depends upon :

Number of electrons involved in the deposition of 63.5g of Cu from a solution of $CuS{O}_4$ is-

Conc. (mol/litre)                    0.25             1

${\wedge }_m\left({\Omega }^{-1}c{m}^{2}mo{l}^{-1}\right)$            260              250

Value of ${{\wedge }_m}^0$ for $SrC{l}_2$ (strong electrolyte) in water at $25°C$ from the above data is -

Calculate the energy obtainable from a lead storage battery in which 0.1 mol lead is consumed. Assume a constant concentration of 10.0 M $H_2 S{O}_4$ 

Adiponitrile is manufactured electrolytically from acrylonitrile $C{H}_2= CHCN \to CN – (C{H}_2 {)}_4 – CH$

How many kg of adiponitrile (molecular mass = 108) is produced in 9.65 hr using a current of 3750 A with 80% efficiency?

A certain metal salt solutions is electrolysed in series with a silver coulometer. The weights of silver and the metal deposited are 0.5094 g and 0.2653 g. Calculate the valency of the metal if its atomic weight is nearly that of silver. 

The temperature coefficient, of the emf is $\frac{d\epsilon }{dT}$= – 0.00065 volt. $de{g}^{-1}$ for the cell $Cd\left|CdC{l}_2\left(1m\right)\right| \left|\underset{\left(s\right)}{AgCl}\right|Ag at 25°C$. Calculate the entropy change $∆S_{298K, }$ for the cell reaction,$Cd + 2AgCl \to C{d}^{++} + 2C{l}^{⊝}+ 2Ag$

The reduction potential of a half-cell consisting of a Pt electrode immersed in $1.5 M F{e}^{2+}$and $0.015 M F{e}^{3+}$ solution at $25°C is \left(E_{\left(F{e}^{+3}, Fe+2\right)}^{°}=+0.770 v\right)$.

In a concentration cell, $Zn/Z{n}^{2+} (1.0 M) \left|\right| Z{n}^{2+} (0.15 M)/Zn$ as the cell discharges,

In a half-cell containing $\left[T{l}^{3+}\right] = 0.1 M and [T{l}^{+} ] = 0.01 M,$ the cell potential is – 1.2496 V for the reaction $T{l}^{+}\to T{l}^{3+} + 2e^{-}$  The standard reduction potential of the $T{l}^{+} /T{l}^{3+}$ couple at $25°C$ is

Given cell: 

Pt(s) | H₂(g) | CH₃COOH,HCl || KCl(aq) | Hg₂Cl₂(s) | Hg

P = 1              0.1M        0.1M

Emf of the cell is found to be 0.045 V at 298 K and temperature coefficient is $3.4 \times {10}^{-4} V K^{-1}$. The cell entropy change of the following cell is : 

Given $K_{a\left(C{H}_{3}COOH\right)} = {10}^{-5} M$

2. 65.2

A dilute solution of $H_2 S{O}_4$ was electrolysed by passing a current of 2 amp. The time required for formation of 0.5 mole of oxygen is

The standard reduction potentials for $M{n}^{3+}/M{n}^{2+}$ and $Mn{O}_2 /M{n}^{3+}$ couples in acid medium at $25°C$ are 1.50 V and 1.00 V respectively. The following reaction:

$2M{n}^{3+} + 2H_{2}O \to M{n}^{2+} + Mn{O}_2 + 4H^{+} is$

$$\begin{gathered} \mathrm{Cu}\left(\mathrm{s}\right) \left|{\mathrm{Cu}}^{+2}(\mathrm{aq}, {10}^{-3})\right| \left|{\mathrm{Ag}}^{+}\left({10}^{-5}\mathrm{M}\right)\right| \mathrm{Ag}\left(\mathrm{s}\right) \\ \mathrm{if} {\mathrm{E}}_{{\mathrm{Cu}}^{+2}/\mathrm{Cu}}^0 = +0.34 \mathrm{V} \\ {\mathrm{E}}_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^0 = +0.80 \mathrm{V} \\ {\mathrm{E}}_{\mathrm{cell}} \mathrm{will} \mathrm{be} : \end{gathered}$$

$$\begin{gathered} 1. 0.46 \mathrm{V} \\ 2. 0.46 - \frac{\mathrm{RT}}{2\mathrm{F}} \mathrm{In} {10}^7 \\ 3. 0.46 +\hspace{0.17em}\frac{\mathrm{RT}}{2\mathrm{F}} \mathrm{In} {10}^7 \\ 4. 0.46 - \frac{\mathrm{RT}}{2\mathrm{F}} \mathrm{In} {10}^2 \end{gathered}$$

1If a 100 mL solution of 0.1M HBr is titrated using a very concentrated solution of NaOH, when the conductivity (specific conductance) of the solution at the equivalence point will 3e (assume volume change is negligible due to addition of NaOH). Calculate your answer in terms of ${10}^{-1}S{m}^{-1},$

$\left[Given {{\wedge }^{°}}_{\left(N{a}^{+}\right)}=8\times {10}^{-3}S{m}^{2}mo{l}^{-1} {{\wedge }^{°}}_{\left(B{r}^{-}\right)}=4\times {10}^{-3}S m^2 mo{l}^{-1}\right]$

The volume of gases liberated at STP when a charge of 2F is passed through aqueous solution of sodium phosphate, is :

It is desired to convert the energy derived from the combustion of propane into electrical energy, via a fuel cell. Given that the standard free energies of formation of $C_3{H}_8 \left(g\right), H_{2}O\left(l\right) and C{O}_2 \left(g\right)$ are -23.5, -237.2 and -394.4 $kJ mo{l}^{-1}$ respectively, calculate the standard EMF of the propane fuel cell.

The temperature coefficient of a standard Cd-cell is $–5.0 \times {10}^{-5} V{k}^{-1}$ whose emf at $25°C$ is 1.018 V. During the cell operation, the temperature will -

Na-amalgam is prepared by electrolysis of NaCl solution using liquid Hg as a cathode. How

long should the current of 10 amp. is passed to produce 10% Na – Hg on a cathode of 10

gm Hg. (atomic mass of Na = 23).

The standard reduction potential of a silver chloride electrode is 0.2 V and that of a silver electrode is 0.79 V. The maximum amount of AgCl that can dissolve in ${10}^6 L of a 0.1 M AgN{O}_3$ solution is 

The $k= 4.95 \times {10}^{-5}S c{m}^{-1}$ for a 0.00099 M solution. The reciprocal of the degree of dissociation of acetic acid, if ${\wedge }_m^0$ for acetic acid is 400 S $c{m}^{2}mo{l}^{-1}$ is :

Pure water is saturated with pure solid AgCl, a silver electrode is placed in the solution and the potential is measured against normal calomel electrode at $25°C$. This experiment is then repeated with a saturated solution of AgI. If the difference in potential in the two cases is 0.177 V. What is the ratio of solubilities of AgCl and AgI at the temperature of the experiment ?

A hydrogen electrode X was placed in a buffer solution of sodium acetate and acetic acid in the ratio a : b and another hydrogen electrode Y was placed in a buffer solution of sodium acetate and acetic acid in the ratio b : a. If reduction potential values for two cells are found to be $E_{1}and E_2$ respectively w.r.t standard hydrogen electrode, the $p{K}_a$ value of the acid can be given as

Calculate the useful work of the reaction \(Ag(s) + {1 \over 2} Cl_2(g) \rightarrow AgCl(s)\) 

$$\begin{gathered} Given, \\ {E^{°}}_{C{l}_2/C{l}^{-}}=+1.36 V, {E^{°}}_{AgCl/Ag,C{l}^{-}}=0.22 V \\ If P_{C{l}_2}=1 atm and T=298 K \end{gathered}$$

The specific conductivity of a saturated solution of KI₃ is 4.59 × 10^-6 ohm^-1 cm^-1 and it's molar conductance is 1.53 ohm^-1 cm² mol^-1. The K_sp Of KI₃ will be : 

A 100.0 mL dilute solution of Ag⁺ is electrolyzed for 15.0 minutes with a current of 1.25 mA and the silver is removed completely. The initial [Ag⁺]is :-

A resistance of 50$\Omega$ is registered when two electrodes are suspended into a beaker containing a dilute solution of a strong electrolyte such that exactly half of the them are submerged into solution. If the solution is diluted by adding pure water (negligible conductivity) so as to just completely submerge the electrodes, the new resistance offered by the solution would be

Acetic acid has $K_a = 1.8 \times {10}^{-5}$ while formic acid has $K_a = 2.1 \times {10}^{-4}$. What would be the magnitude of the emf of the cell 

                  $Pt\left(H_2\right)\left|\begin{array}{c}0.1 M acetic acid + \\ 0.1 M sodium acetate\end{array}\right| \left|\begin{array}{c}0.1 M formic acid \\ 0.1 M sodium formate\end{array}\right|Pt\left(H_2\right) at 25°C$ ?

Following cell has EMF 0.7995 V 

If we add enough KCl to the Ag cell so that the final $C{l}^{-}$is 1M. Now the measured emf of the cell is 0.222 V. The $K_{SP}$ of AgCl would be :

$Pt | H_2 (1 atm) | HN{O}_3 \left(1M\right) \left|\right| AgN{O}_3 \left(1M\right) | Ag$. 

A flashlight cell has the cathodic reaction $2Mn{O}_2 \left(s\right) + Z{n}^{+2}+ 2\text{'}{e}^{-}\to Zn M{n}_2{O}_4 \left(S\right)$

If the flashlight cell is to give out 4.825 mA, how long could it run if initially 8.7 g of the

limiting reagent $Mn{O}_2$ is present? [Mn = 55, O = 16]