Chemistry Assessment 020725

Which of the following factors does NOT affect the amount of substance deposited during electrolysis?

The charge on the ion

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The current passed through the electrolyte

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The time for which current is passed

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The density of the electrolyte

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During the electrolysis of molten NaCl, which of the following reactions occurs at the cathode?

Na⁺ + e⁻ → Na

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2Cl⁻ → Cl₂ + 2e⁻

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2H₂O + 2e⁻ → H₂ + 2OH⁻

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NaCl → Na⁺ + Cl⁻

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A charge of 9650 C is passed through an electrolytic cell containing AgNO₃ solution. How much silver (Ag) will be deposited? (Ag = 108 g/mol, 1 Faraday = 96500 C)

10.8 g

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1.08 g

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0.108 g

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108 g

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Electrolysis is used in all of the following processes EXCEPT:

Electroplating

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Metal extraction

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Battery discharge

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Production of chlorine

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If a current of 4 A is passed through molten Al₂O₃ for 9650 s, what mass of Al is deposited? (Al = 27 g/mol, n = 3, F = 96500 C)

2.7 g

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5.4 g

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8.1 g

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10.8 g

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ow much oxygen gas (in liters at STP) is produced when 1 Faraday of charge is passed through water? (1 mol of gas = 22.4 L at STP, n = 4 for O₂ production)

11.2 L

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2.8 L

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22.4 L

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5.6 L

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How much copper (Cu) is deposited when a current of 2 A is passed through CuSO₄ solution for 1 hour?
(Cu = 63.5 g/mol, ? = 2, F=96500 C)

1.18 g

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2.36 g

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3.54 g

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4.72 g

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What charge (in Coulombs) is required to deposit 0.5 g of silver from AgNO₃ solution? (Ag = 108 g/mol, n = 1, F = 96500 C)

447.7 C

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5000 C

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9650 C

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10000 C

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During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is

0.5 mole

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2 moles

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1 moles

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1.5 moles

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What amount of electricity must be supplied to an electrolytic cell in order to produce 0.100Kg of Iron from Iron(III)oxide? (Given: Fe = 55.85 g/mol, Faraday’s constant F = 96500 C/mol)

775,680 C

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258,560 C

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129,280 C

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517,120 C

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Chemistry Assessment 020725

Stephen February 7, 2025

Chemistry Assessment 020725

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