A silver cup is plated with silver by passing 965 coulomb of electricity. The amount of Ag deposited is:

1. 1.08 g

2. 1.0002 g

3. 9.89 g

4. 107.89 g

 

Which is the correct representation for Nernst equation ?

1. \(E_{\mathrm{RP}}=E_{\mathrm{RP}}^{\circ}+\frac{0.059}{\mathrm{n}} \log \frac{[\text { oxidant }]}{[\text { reductant }]}\)

2. \(E_{\mathrm{OP}}=E_{\mathrm{OP}}^{\circ}-\frac{0.059}{\mathrm{n}} \log \frac{[\text { oxidant }]}{[\text { reductant }]}\)

3. \(E_{\mathrm{OP}}=E_{\mathrm{OP}}^{\circ}+\frac{0.059}{\mathrm{n}} \log \frac{[\text { reductant }]}{[\text { oxidant }]}\)

4. All of the above

When a copper wire is immersed in a solution of AgNO₃, the colour of the solution becomes blue because copper:

1. Forms a soluble complex with \(AgNO_3\)
2. Is oxidised to \(Cu^{2+}\)
3. Is reduced to \(Cu^{2-}\)
4. Splits up into atomic form and dissolves

The specific conductance of a 0.1 M KCl solution at 23 °C  is 0.012  Ω^-1 cm^-1 . The resistance of cells containing the solution at the same temperature was found to be 55 Ω. The cell constant will be:
 
1. 0.142cm^-1

2. 0.66 cm^-1

3. 0.918 cm^-1

4. 1.12cm^-1

Given below are the half-cell reactions,

Mn²⁺ + 2e^-  $\to \; Mn; \; \; \; \; \; \; E0\; =\; -1.18V$

$$ \to \; 2Mn2+; \; E0\; =\; +1.51V$$

$$ E0 for\; 3\; Mn2+ \to \; 2\; Mn+3 \; +$$Mn will be:

$$ $ 1.\; -2.69V;\; the\; reaction\; will\; not\; occur$$$

$$ $ 2.\; -2.69V;\; the\; reaction\; will\; occur$$$

$$ $ $ 3.\; -0.33V;\; the\; reaction\; will\; not\; occur$$$$

$$ $ $ $ 4.\; -0.33V;\; the\; reaction\; will\; occur$$$$$

E⁰ for Fe²⁺ + 2e → Fe is -0.44 volt and E⁰ for Zn²⁺ + 2e→ Zn is -0.76 volt, thus:

1. Zn is more electropositive than Fe

2. Fe is more electropositive than Zn

3. Zn is more electronegative

4. none of the above  

The voltage of the cell given below increases with: 

Cell: Sn(s) + 2Ag⁺(aq) → Sn²⁺(aq) + 2Ag(s)

1. Increase in size of the silver rod.

2. Increase in the concentration of Sn²⁺ ions.

3. Increase in the concentration of Ag⁺ ions.

4. None of the above.

A 5A current is passed through a solution of copper sulphate for 40 min. The amount of copper deposited at the cathode is 

1. 40.65g

2. 0.45g

3. 3.94g

4. 65.04g

$E_{\raisebox{1ex}{${\mathrm{Fe}}^{2+}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{Fe}$}\right.}^{\circ } = -0.441 \mathrm{V} and E_{\raisebox{1ex}{${\mathrm{Fe}}^{3+}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{Fe}}^{2+}$}\right.}^{\circ } =0.771 \mathrm{V}$, the standard emf of the reaction

$\mathrm{Fe} + 2{\mathrm{Fe}}^{3+} \stackrel{ }{\to }3{\mathrm{Fe}}^{2+}$will be

1. 0.111V

2. 0.330V

3. 1.653V

4. 1.212V

The standard electrode potential for Sn⁴⁺/Sn²⁺ couple is +0.15 V and that for the Cr³⁺/Cr couple is -0.74 V. These two couples in their standard state are connected to make a cell. The cell potential will be: 

1. +0.89 V

2. +0.18 V

3. +1.83 V

4. +1.199 V