Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO₃ for 15 minutes.
(Given : Molar mass of Ag = 108 g mol^–1 1F = 96500 C mol^–1)

Define fuel cell.

For the reaction

$$\begin{gathered} 2AgCl \left(s\right) + H_2 \left(g\right) (1 atm) \stackrel{ }{\to } 2 Ag \left(s\right) + 2H^{+} (0.1 M) + 2C{l}^{-} (0.1 M), \\ ∆G^o = - 43600 J at {25}^o C \end{gathered}$$

Calculate the e.m.f. of the cell.
[log 10^–n = – n]

Define fuel cell and write its two advantages.

Which among the following metals is employed to provide cathodic protection to iron?

• Zinc

• Nickel

• Tin

• Lead

Galvanization is applying a coating of:

• Cr

• Cu

• Zn

• Zn

Two Faraday of electricity is passed through a solution of CuSO₄. The mass of copper deposited at the cathode is: (at. mass of Cu = 63.5 amu)

• 0 g

• 63.5 g

• 2 g

• 2 g

The equivalent conductance of NaCl at concentration C at infinite dilution are λ_C and λ_∞ respectively. The correct relationship between λ_C and λ_∞  is given as (where the constant B is positive)

• λ_C = λ_∞ +(B)C

• λ_C = λ_∞ -(B)C

• λ_C = λ_∞ -(B)

• λ_C = λ_∞ -(B)

339.

Given below are the half-cell reactions
Mn²⁺ + 2e^- → Mn; E^o = - 1.18 eV
2(Mn³⁺ + e^- →Mn²⁺); E^o = +1.51 eV
The E^o for 3Mn²⁺ → Mn + 2Mn³⁺ will be

• -2.69 V; the reaction will not occur

• -2.69 V; the reaction will occure

• -0.33 V; the reaction will not occur

• -0.33 V; the reaction will not occur

Given, 


Based on the data given above, strongest oxidising agent will be

• Cl

• Cr³⁺

• Mn²⁺

• Mn²⁺