Class 12 Chemistry

Chapter 3 – Electrochemistry

Magical Series Assignment 2

 

Q.1.     The standard electrode potential for Daniell cell is 1.1 V Calculate the standard Gibbs energy for the cell reaction. (F = 96500 C mol^–1)

Q.2.     A zinc rod is dipped in 0.1 M solution of ZnSO₄. The salt is 95% dissociated at this dilution at 298 K. Calculate the electrode potential. [E^o_Zn2+/Zn = – 0.76 V, log 0.095 = -1.0222]

Q.3.     Determine the value of equilibrium constant (K_C) and ∆G^o for the following reactions:

Ni(s) + 2Ag⁺(aq) → Ni²⁺(aq) + 2Ag(s)

(E^o = 1.05 V; 1 F = 96500 C mol^–1)

Q.4.     Calculate the emf for the given cell at 25°C:

Cr | Cr³⁺ (0.1 M) || Fe²⁺ (0.01 M) | Fe

Given: E^o_Cr3+/Cr = –0.74 V, E^o_Fe2+/Fe = –0.44 V.

Q.5.     Write the cell reaction and calculate the e.m.f. of the following cell at 298 K:

Sn(s) | Sn²⁺ (0.004 M) || H⁺ (0.020 M) | H₂(g) (1 bar) | Pt(s)

(Given: E^o_Sn2+/Sn = –0.14 V)

Q.6.     For the reaction,

2AgCl(s) + H₂(g) (1 atm) → 2Ag(s) + 2H⁺ (0.1 M) + 2Cl^–(0.1 M)

∆G^o = – 43600 J at 25 °C. Calculate the e.m.f. of the cell. (log 10^–n = –n).

Q.7.     Calculate E^o_cell for the following reaction at 298 K.

2Al(s) + 3Cu²⁺(0.01 M) → 2Al³⁺(0.01 M) + 3Cu(s)

Given: E_cell = 1.98 V.

Q.8.     Calculate emf of the following cell at 25°C:

Fe | Fe²⁺(0.001 M) || H⁺(0.01 M) | H₂(g, l bar) | Pt(s)

E^o_Fe2+/Fe = –0.44 V, E^o_H+/H2 = 0.00 V

Q.9.     Calculate the emf of the following cell at 25°C

Zn | Zn²⁺ (0.001 M) || H⁺(0.01 M) | H₂(g)(1 bar) | Pt(s)

E^o_Zn2+/Zn = –0.76 V, E^o_H+/H2 = 0.00 V

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