Test: Nernst Equation Conductance of Electrolytic Solutions (November 11) - NEET MCQ

The correct answer is Option C.

Reactions with a negative ∆G release energy, which means that they can proceed without an energy input (are spontaneous). In contrast, reactions with a positive ∆G need an input of energy in order to take place (are non-spontaneous). Reactions with a positive ∆H and negative ∆S are non-spontaneous at all temperatures.

The correct answer is Option B.
The relationship between ΔG^o and E^o is given by the following equation: ΔG^o=−nFE^o. Here, n is the number of moles of electrons and F is the Faraday constant.

The correct answer is Option D.

Redox reaction:
Cd(s)→Cd²⁺+2e
Cu²⁺+2e→Cu(s)
E_cell = E°_cell − (0.059/2) log ([Cd²⁺]/ [Cu²⁺])
Decreases [Cd²⁺] to 0.1M and increases [Cu²⁺] to 1.0M

On dilution, molarity decreases and molar conductance increases, Hence, specific conductance decreases.

Specific conductance = Conductance x Cell constant
∴ x = k (0.01 N KCI) = y x cell constant
∴ k (0.01N NaCI) = z x cell constant 

Molar conductance 

When temperature increases, conductance increases. Thus, resistivity and conductivity both are temperature dependent. By Nernst equation,

Thus, Emf of the cell is dependent on temperature.

Thus, cell constant is temperature independent.

(CH₃COOH) = (CH₃COONa) + (HCI) - (NaCI)
= 91.0+ 426.2 -126.5 
= 517.2 - 126.5 
= 390.7 Scm²mol^-1

Water has also conductance, hence to obtain pure value of conductance of AgCI, conductance of water should be substracted from the conductance of AgCI given.

Pure specific conductance of AgCI = (3.41 x 10^-6 - 1.60 x 10^-6)

= 1.81 x 10^-6Ω ^-1cm^-1

AgCI is sparingly soluble, hence its solubility may be taken its concentration.
Also, in saturated solution sparingly soluble salt

∴   

∴   AgCl (s)  Ag⁺ + Cl^-

∴ Ksp = [Ag⁺] [Cl^-] = S²
= (1.31 x 10^-5)²
= 1.72 x 10^-10 mol²L^-2