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CBSE

Subject

Chemistry

NEET Chemistry : Electrochemistry

Multiple Choice Questions

161.

For a cell involving one electron E°_cell= 0.59 V at 298 K, the equilibrium constant for the cell reaction is :[ Given that $\frac{2.303}{F} = 0.059 V at T = 298 K]$ .

1.0 × 10⁵
1.0 × 10¹⁰
1.0 × 10³⁰
1.0 × 10²

162.

Distribution law was given by :

Henry
vant Hoff
Nernst
Ostwald

163.

In the electrochemical reaction, $2 {Fe}^{3 +} + Zn \to {Zn}^{2 +} + 2 {Fe}^{2 +}$ increasing the concentration of Fe²⁺

increases cell emf
increases the current flow
decrease the cell emf
alter the pH of the solution

164.

The cell reaction of a cell is $Mg (s) + {Cu}^{2 +} (aq) \to Cu (s) + {Mg}^{2 +} (aq) .$ If the standard reduction potentials of Mg and Cu are - 2.37 and + 0.34V respectively. The emf of the cell is

2.03V
-2.03V
+2.71V
-2.71V

165.

When Cu reacts with AgNO₃ solution, the reaction takes place is:

oxidation of Cu
reduction of Cu
oxidation of Ag
reduction of NO $_{3}^{-}$

166.

For the cell reaction

2Fe³⁺ (aq) +2l^-(aq) → 2Fe²⁺(aq) + I₂(aq)

E $_{cell}^{⊝}$ = 0.24V at 298 K. The standard Gibbs energy (Δ_rG^Θ) of the cell reaction is:

[Given that Faraday constant F = 96500 C mol^–1]

– 23.16 kJ mol^–1
46.32 kJ mol^-1
23.16 kJ mol^-1
- 46.32 kJ mol^-1

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