The correct expression that  represents the equivalent conductance at infinite dilution of $A{l}_2{\left(S{O}_4\right)}_3$ is: (Given that ${\wedge }_{A{l}^{3+}}^{°} and {\wedge }_{S{O}_4^{2-}}^{°}$ are the equivalent conductances at infinite dilution of the respective ions)

Consider the following relations for emf of a electrochemical cell :
(a) emf of cell = (Oxidation potential of anode) – (Reduction potential of cathode)
(b) emf of cell = (Oxidation potential of anode) + (Reduction potential of cathode)
(c) emf of cell = (Reduction potential of anode) + (Reduction potential of cathode)
(d) emf of cell = (Oxidation potential of anode) – (Oxidation potential of cathode)

The correct relation among the given options is : 

The concentration of $ZnC{l}_2$ solution will change when it is placed in a container which is made of :

The cell reaction of an electrochemical cell is \(Cu^{2+}(C_{1}) + Zn \to Cu + Zn^{2+}(C_{2})\).
The change in free energy will be the function of :

For the disproportionation of copper :

$2C{u}^{+}\to C{u}^{+2}+Cu, E°$ is :-
(Given $E°$ for Cu⁺²/Cu is 0.34 V & Eº for Cu⁺²/Cu⁺ is 0.15 V )

Cell reaction is spontaneous when :

At infinite dilution equivalent conductances of Ba⁺² & Cl^– ions are 127 & 76 ohm^–1cm^–1 eq^–1 respectively. Equivalent conductance (ohm^–1cm^–1 eq^–1)of BaCl₂ at infinite dilution is :

The value of E⁰ cell for the following reaction is -
\(Cu^{2+}+ Sn^{2+}\to Cu +Sn^{4+ }\)

(Given , equilibrium constant is 10⁶)

The standard Emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25ºC. The equilibrium constant of the reaction would be :-

In the silver plating of copper, K[Ag(CN)₂] is used instead of AgNO₃. The reason is : -

On the basis of the information available from the reaction :

$\frac{4}{3}\mathrm{Al}+{\mathrm{O}}_2\to \frac{2}{3}{\mathrm{Al}}_2{\mathrm{O}}_3, ∆\mathrm{G}=-827 \mathrm{KJ} {\mathrm{mol}}^{-1}$

of O₂, the minimum e.m.f. required to carry out electrolysis of Al₂O₃ is : (F=96500 C mol^–1)

The EMF of a Daniel cell at 298 K is E₁  Zn|ZnSO₄(0.01 M) || CuSO₄(1.0 M)|Cu .
When the concentration of ZnSO₄ is 1.0 M and that of CuSO₄ is 0.01 M, the EMF is changed to E₂. The correct relationship between E₁ and E₂ is :

Arrange the following metals in the order in which they displace each other from the solution of their salts 

Al, Cu, Fe, Mg, and Zn.

 2Cr(s) + 3Cd²⁺(aq) → 2Cr³⁺(aq) + 3Cd

${{\mathrm{E}}^{⊝}}_{{\mathrm{Cr}}^{3+}/\mathrm{Cr}}= -0.74 \mathrm{V}$; ${{\mathrm{E}}^{⊝}}_{{\mathrm{Cd}}^{2+}/\mathrm{Cd}}=-0.40 \mathrm{V}$

The value of $∆{\mathrm{G}}_r^{\mathrm{o}}$ in the above reaction will be - 

a. The unit of conductivity is $\mathrm{S} {\mathrm{cm}}^{-2}$.

b. Specific Conductivity of weak and strong electrolytes always decreases with a decrease in concentration.

c. The unit of molar conductivity is $\mathrm{S} c{\mathrm{m}}^2 {\mathrm{mol}}^{-1}$

d. Molar conductivity increases with an increase in concentration.

The incorrect statement (s) among the above is/ are : 

The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm^–1 . The molar conductivity will be -

The electricity required in coulombs for the oxidation of 1 mole of FeO to ${\mathrm{Fe}}_2{\mathrm{O}}_3$is-

Pt_(s) | Br^-_{(0.010 M)} | Br_2 (l) || H⁺_{(0.030 M)} | H_{2  (1 bar)} | Pt_(s)  

${\mathrm{E}}_{{\mathrm{Br}}^{-}/{\mathrm{Br}}_2}^{\mathrm{o}}=-1.09 \mathrm{V}$

The value of ${\mathrm{E}}_{\mathrm{cell} }$ in the above reaction will be : 

$$\begin{gathered} \mathrm{Zn}\left(\mathrm{s}\right) \hspace{0.17em}+ {\mathrm{Ag}}_2\mathrm{O}\left(\mathrm{s}\right) +{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right) \to \\ {\mathrm{Zn}}^{+2}\left(\mathrm{aq}\right) +2\mathrm{Ag}\left(\mathrm{aq}\right) +\hspace{0.17em}2{\mathrm{OH}}^{-}\left(\mathrm{aq}\right) \end{gathered}$$

${\mathrm{E}}_{\mathrm{cell}}^{°} = 1.04$ ; the value of $∆\mathrm{G}°$ in the above reaction would be -

The mass of nickel deposited by electrolysis of a solution of $\mathrm{Ni}{\left({\mathrm{NO}}_3\right)}_2$ using a current of 5 amperes for 20 min is (atomic mass of Nickle is 58.7) -

Consider the following graph.

The strong electrolyte in the above graph is represented by -

Consider the following graph of molar conductivity of KCl solution at different concentrations. 

The value of limiting molar conductivity for KCl is $150.0 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}$.  The value of the slope at the point A will be : 

The molar conductance of NaCl, HCI, and CH₃COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol^-1 respectively. The molar conductance of CH₃COOH at infinite dilution is. Choose the right option for your answer.

The molar conductivity of 0.007 M acetic acid is 20 S cm² mol^-1. The dissociation constant of acetic acid is -

$$\begin{gathered} \left[\mathrm{\Lambda }{°}_{{\mathrm{H}}^{+}}=350 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}\right] \\ \left[\mathrm{\Lambda }{°}_{{\mathrm{CH}}_3{\mathrm{COO}}^{-}}=50 \mathrm{S} {\mathrm{cm}}^2 {\mathrm{mol}}^{-1}\right] \end{gathered}$$

For a cell reaction involving  a two-electron change, the standard Emf of the cell is found to be 0.295V at 25^oC . The equilibrium constant of the reaction at 25^oC will be :