The value of E_cell in the reaction below will be:

\(\small{Pt(s)|Br^{-}(0.010 \ M)|Br_{2}(l) \ ||H^{+}(0.030 \ M)|H_{2}(g)(1 \ bar)|Pt(s)}\)

\(E_{Br^{-}/Br_{2}}^{o} \ = \ -1.09 \ V\)
1. +1.298 V

2. –1.398 V

3. –1.298 V

4. –1.198 V

The value of  ∆G°  in the reaction below would be:
\(\small{\mathrm{Zn}(\mathrm{s})+\mathrm{Ag}_2 \mathrm{O}(\mathrm{s})+\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{Zn}^{+2}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})+2 \mathrm{OH}^{-}(\mathrm{aq})}\)

Given: \(E_{cell}^{\circ} = 1.04V\)

1. –2.13 kJ

2. –21.3 kJ

3. –201 kJ

4. –31.12 kJ

The mass of nickel deposited by electrolysis of a solution of $\mathrm{Ni}{\left({\mathrm{NO}}_3\right)}_2$ using a current of 5 amperes for 20 min is: 
(Atomic mass of Nickle is 58.7u)

1. 2.42 g

2. 1.82 g

3. 3.93 g

4. 6.42 g

The molar conductance of NaCl, HCI, and CH₃COONa at infinite dilution are 126.45, 426.16, and 91.0 S cm mol^–1 respectively. The molar conductance of CH₃COOH at infinite dilution will be:

1. 698.28 S cm² mol^–1

2. 540.48 S cm² mol^–1

3. 201.28 S cm² mol^–1

4. 390.71 S cm² mol^–1

The molar conductivity of 0.007 M acetic acid is 20 S cm² mol^–1. The dissociation constant of acetic acid is :

(\(\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }\))
(\(\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}\))

1. $1.75\times {10}^{-5}$ mol L^–1 

2. $2.50\times {10}^{-5}$ mol L^–1 

3. $1.75\times {10}^{-4}$ mol L^–1 

4. $2.50\times {10}^{-4}$ mol L^–1 

Mg(s) + 2Ag⁺(0.0001M) → Mg²⁺(0.130M) + 2Ag(s)

If  E^Ɵ(cell) for the above mentioned cell is 3.17 V, then E(cell) value will be-

(log 13=1.1)

1. 2.87 V
2. 3.08 V
3. 2.96 V
4. 2.68 V

The equilibrium constant value for the given reaction is:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

(Given: E^Ɵ(cell) = 0.46 V)

1. 3.92 × 10¹⁴
2. 3.92 × 10¹⁵
3. 3.92 × 10¹⁶
4. 3.92 × 10¹⁷

The standard electrode potential for Daniell cell is 1.1V. The standard Gibbs energy for the given reaction is-

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

(Given: F = 96487 C mol^–1)

1. 312.27 kJ mol^–1
2. 212.27 kJ mol^–1
3. – 312.27 kJ mol^–1
4. – 212.27 kJ mol^–1

Resistance of a conductivity cell filled with 0.1 mol L^–1 KCl solution is 100 Ω. If the resistance of the same cell when filled with 0.02 mol L^–1 KCl solution is 520 Ω. The conductivity of 0.1 mol L^–1 KCl solution is 1.29 S/m. The molar conductivity of 0.02 mol L^–1 KCl solution is-

1. 134 S cm² mol^–1
2. 124 S cm² mol^–1
3. 144 S cm² mol^–1
4. 154 S cm² mol^–1

Consider the following data:
Λ^°_m(Ca²⁺) = 119.0 S cm²mol^–1 
Λ^°_m(Cl^-) = 76.3 S cm²mol^–1
Λ^°_m(Mg²⁺) = 106.0 S cm²mol^–1
Λ^°_m(\(SO_{4}^{2-}\)) = 160.0 S cm²mol^–1 
 
The correct statement among the following is-