# An electrochemical cell is shown below Pt, H2(1 atm)| HCI (0.1 M)CH3COOH (0.1 M)| H2(1 atm), Pt The EMF of the cell will not be zero, because 1. EMF depends on molarities of acids used 2. pH of 0.1 M HCl and 0.1 M CH3COOH is not same 3. the temperature is constant 4. acids used in two compartments are different

Subtopic:  Electrode & Electrode Potential |
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Saturated solution of KNO3 is used to make 'salt-bridge' because:

1. velocity of K+ is greater than that of ${\mathrm{NO}}_{3}^{-}$

2. velocity of ${\mathrm{NO}}_{3}^{-}$ is greater than that of K+

3. Velocities of both K+ and ${\mathrm{NO}}_{3}^{-}$ are nearly the same

4. KNO3 is highly soluble in water

Subtopic:  Batteries & Salt Bridge |
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A current is passed through two voltameters connected in series. The first voltmeter connected in series. The first voltmeter contains XSO4(aq) while the second voltmeter contains Y2SO4(aq). The relative  atomic masses of X and Y are in the ratio of 2:1. The ration of the mass of X liberated to the mass of Y liberated is:

1. 1:1

2. 1:2

3. 2:1

4. none of these

Subtopic:  Faraday’s Law of Electrolysis |
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The mass of silver(eq. mass = 108) displaced by that quantity of current which displaced 5600 mL of hydrogen at STP is:

1. 54 g

2. 108 g

3. 5.4 g

4. none of these

Subtopic:  Faraday’s Law of Electrolysis |
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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

Subtopic:  Faraday’s Law of Electrolysis |
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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

Subtopic:  Nernst Equation |
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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

Subtopic:  Electrochemical Series |
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The specific conductance of a 0.1N KCl solution at 23$°\mathrm{C}$ is 0.012 ${\mathrm{\Omega }}^{-1}{\mathrm{cm}}^{-1}$. The resistance of cell containing the solution at the same temperature was found to be 55 $\mathrm{\Omega }$. The cell constant will be
1. 0.142cm-1

2. 0.66 cm-1

3. 0.918 cm-1

4. 1.12cm-1

Subtopic:  Conductance & Conductivity |
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Given below are the half-cell reactions,

Mn2+ + 2e-

Mn will be:

Subtopic:  Electrode & Electrode Potential |
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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

Subtopic:  Electrode & Electrode Potential |
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