# The correct statement about the given galvanic cell equation is - Zn(s) + 2Ag+­­­(aq) → Zn2+(aq) + 2Ag(s) 1. The current will flow from silver to zinc in the external circuit. 2. The current will flow from zinc to silver in the external circuit. 3. The current will flow from silver to zinc in the internal circuit. 4. The current will flow from zinc to silver in the internal circuit.

Subtopic:  Electrolytic & Electrochemical Cell |
60%
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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-

 1 -196.83 kJ 2 196.83 kJ 3 186.83 kJ 4 -186.83 kJ

Subtopic:  Relation between Emf, G, Kc & pH |
74%
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The incorrect statement(s) among the below is/are:

 (a) The unit of conductivity is S cm-2 (b) Specific Conductivity of weak and strong electrolytes always decreases with a decrease in concentration. (c) The unit of molar conductivity is S cm2 mol-1 (d) Molar conductivity increases with an increase in concentration.

1. (a)

2. (a) and (d)

3. (b) and (d)

4. (a) and (c)

Subtopic:  Conductance & Conductivity |
57%
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The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm–1. The molar conductivity will be -

 1 124 S cm2 mol-1 2 134 S cm2 mol-1 3 128 S cm2 mol-1 4 136 S cm2 mol-1
Subtopic:  Conductance & Conductivity |
88%
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The electricity required in coulombs for the oxidation of 1 mole of FeO to is:

 1 964.87 C 2 96487 C 3 96.487 C 4 9.6487 C
Subtopic:  Faraday’s Law of Electrolysis |
86%
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The value of Ecell 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

Subtopic:  Nernst Equation |
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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. 213.04 kJ

4. 31.12 kJ

Subtopic:  Relation between Emf, G, Kc & pH |
75%
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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 58.7) -

1. 2.42 g

2. 1.82 g

3. 3.93 g

4. 6.42 g

Subtopic:  Faraday’s Law of Electrolysis |
72%
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The correct increasing order of reducing power of the metals is:

 K+/K = –2.93 V Ag+/Ag = 0.80 V Hg2+/Hg = 0.79 V Mg2+/Mg = –2.37 V Cr3+/Cr = – 0.74 V

 1 Cr

Subtopic:  Electrode & Electrode Potential |
85%
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Mg(s) | Mg2+(0.001M) || Cu2+(0.0001 M) | Cu(s)

The value of  for the above reaction is -

1. 3.46 V

2. 3.15 V

3. 2.67 V

4. 1.24 V

Subtopic:  Nernst Equation |
86%
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