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

(Given, equilibrium constant is 10⁶)

1.	0.17	2.	0.01
3.	0.05	4.	1.77

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

(Given F = 96500 C mol^–1; R = 8.314 J K^–1 mol^–1) 

1. 4.0 × 10¹²

2. 1.0 × 10²

3. 1.0 × 10¹⁰

4. 2.0 × 10¹¹

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:

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

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

1. 2.14 V

2. 4.28 V

3. 6.42 V

4. 8.56 V

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:

The following metals should be arranged so that they push one another out of the salt solution in that order: 

Al, Cu, Fe, Mg, and Zn.
 

1. Cu <Fe<Zn< Al< Mg

2. Zn< Fe< Cu< Mg< Al

3. Mg<Cu <Zn <Fe< Al

4. Al<Zn<Fe< Cu< Mg

The correct increasing order of reducing power of the metals is:

The correct statement about the given galvanic cell equation is -

Zn_(s) + 2Ag⁺­­­_(aq) → Zn²⁺_(aq) + 2Ag_(s)

 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-

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

1. a

2. a and d

3. b and d

4. a and c