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  4. Electrochemistry Chapter-Wise Test 2

Electrochemistry Chapter-Wise Test 2

Correct answer Carries: 4.

Wrong Answer Carries: -1.

The limiting molar conductivity of BaCl\(_2\) is 280 S cm\(^2\) mol\(^{-1}\). If \( \lambda^\circ_{Ba^{2+}} = 127 \, S \, cm^2 \, mol^{-1} \), what is \( \lambda^\circ_{Cl^-} \)?

\( \Lambda_m^\circ = \lambda^\circ_{Ba^{2+}} + 2\lambda^\circ_{Cl^-} \).

\( 280 = 127 + 2\lambda^\circ_{Cl^-} \), \( 2\lambda^\circ_{Cl^-} = 153 \), \( \lambda^\circ_{Cl^-} = 76.5 \, S \, cm^2 \, mol^{-1} \).

127 S cm\(^2\) mol\(^{-1}\)
153 S cm\(^2\) mol\(^{-1}\)
76.5 S cm\(^2\) mol\(^{-1}\)
280 S cm\(^2\) mol\(^{-1}\)
3

What is the equilibrium constant for a cell reaction with \( E^\circ_{cell} = 0.354 \, V \) at 298 K involving 2 electrons?

\( E^\circ_{cell} = \frac{0.059}{n} \log K_c \), \( 0.354 = \frac{0.059}{2} \log K_c \), \( \log K_c = 12, K_c = 10^{12} \).

10\(^6\)
10\(^8\)
10\(^{12}\)
10\(^{10}\)
3

In the electrolysis of molten NaCl, what is the product at the cathode?

Cathode: \( Na^+ + e^- \rightarrow Na \). Sodium metal is produced.

Cl\(_2\)
H\(_2\)
Na
O\(_2\)
3

How many electrons are involved in the reduction of 1 mole of \( IO_3^- \) to \( I_2 \) in acidic medium?

\( 2IO_3^- + 12H^+ + 10e^- \rightarrow I_2 + 6H_2O \). For 1 mol \( IO_3^- \), 5 electrons.

6
5
3
10
2

What is the standard Gibbs energy change for a cell with \( E^\circ_{cell} = 1.05 \, V \) and 2 electrons transferred? (F = 96500 C/mol)

\( \Delta_r G^\circ = -n F E^\circ_{cell} = -2 \times 96500 \times 1.05 = -202650 \, J/mol = -202.65 \, kJ/mol \).

-101.325 kJ/mol
-202.65 kJ/mol
-96.5 kJ/mol
-405.3 kJ/mol
2

In a dry cell, what is the reducing agent during discharge?

Anode: \( Zn \rightarrow Zn^{2+} + 2e^- \). Zn is oxidized, so it’s the reducing agent.

Zn
MnO\(_2\)
NH\(_4\)Cl
MnO(OH)
1

What is the time (in seconds) required to deposit 1.175 g of sodium from molten NaCl using a current of 2 A? (Atomic mass of Na = 23.5 g/mol, F = 96500 C/mol)

\( Na^+ + e^- \rightarrow Na \). 1 mol Na (23.5 g) requires 1F.

Moles = \( \frac{1.175}{23.5} = 0.05 \, mol \), Charge = \( 0.05 \times 96500 = 4825 \, C \).

\( t = \frac{Q}{I} = \frac{4825}{2} = 2412.5 \, s \).

2412.5 s
4825 s
9650 s
1206.25 s
1

The resistance of a conductivity cell with 0.02 M KCl solution is 400 Ω, and its conductivity is 0.0025 S cm\(^{-1}\). What is the cell constant?

\( \kappa = \frac{\text{cell constant}}{R} \), \( 0.0025 = \frac{\text{cell constant}}{400} \), cell constant = 1.0 cm\(^{-1} \).

0.25 cm\(^{-1}\)
2.5 cm\(^{-1}\)
1.0 cm\(^{-1}\)
0.5 cm\(^{-1}\)
3

A weak electrolyte has \( \Lambda_m^\circ = 390 \, S \, cm^2 \, mol^{-1} \) and a degree of dissociation of 0.02 at 0.1 M. What is the conductivity of the solution?

\( \Lambda_m = \alpha \Lambda_m^\circ = 0.02 \times 390 = 7.8 \, S \, cm^2 \, mol^{-1} \).

\( \kappa = \frac{\Lambda_m \times c}{1000} = \frac{7.8 \times 0.1}{1000} = 0.00078 \, S \, cm^{-1} \).

0.0078 S cm\(^{-1}\)
0.00078 S cm\(^{-1}\)
0.039 S cm\(^{-1}\)
0.00039 S cm\(^{-1}\)
2

In electrolysis of molten MgCl\(_2\), 0.24 g of Mg (atomic mass 24 g/mol) is deposited. What volume of Cl\(_2\) gas (STP) is produced at the anode? (F = 96500 C/mol)

Cathode: \( Mg^{2+} + 2e^- \rightarrow Mg \). Moles = \( \frac{0.24}{24} = 0.01 \, mol \), Charge = \( 0.01 \times 2 \times 96500 = 1930 \, C \).

Anode: \( 2Cl^- \rightarrow Cl_2 + 2e^- \). Moles Cl\(_2\) = \( 0.01 \, mol \), Volume = \( 0.01 \times 22.4 = 0.224 \, L \).

0.112 L
0.448 L
0.056 L
0.224 L
3

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