Electrolytic Cells

Chemistry ⇒ Redox Reactions and Electrochemistry

Electrolytic Cells starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Electrolytic Cells. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 11

A current of 0.5 A is passed through an electrolytic cell containing AgNO₃ solution for 1930 seconds. Calculate the mass of silver deposited. (Molar mass of Ag = 108 g/mol, 1 Faraday = 96500 C)

A solution of copper(II) sulfate is electrolyzed using platinum electrodes. What is observed at the cathode?

A student electrolyzes a solution of potassium iodide using inert electrodes. What is observed at the anode?

Calculate the mass of copper deposited at the cathode when a current of 2.0 A is passed through a copper(II) sulfate solution for 1 hour. (Molar mass of Cu = 63.5 g/mol, 1 Faraday = 96500 C)

Calculate the number of moles of electrons required to deposit 5.4 g of silver from AgNO₃ solution. (Molar mass of Ag = 108 g/mol)

Describe the main difference between a galvanic cell and an electrolytic cell.

During the electrolysis of aqueous copper(II) sulfate using copper electrodes, what happens to the mass of the anode?

During the electrolysis of aqueous copper(II) sulfate using inert electrodes, what is the product at the anode?

During the electrolysis of water, what is the ratio of the volumes of hydrogen and oxygen gases produced?

Explain the role of the electrolyte in an electrolytic cell.

Explain why a direct current (DC) source is required for the operation of an electrolytic cell.

Explain why electrolysis of molten NaCl produces different products compared to electrolysis of aqueous NaCl.

Explain why inert electrodes are used in some electrolytic cells.

In an electrolytic cell, which electrode attracts cations?

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

State Faraday's first law of electrolysis.

State the products formed at the electrodes during the electrolysis of molten lead(II) bromide.

A certain electrolytic cell requires a minimum applied voltage of 2.2 V to operate. If the cell is supplied with only 1.5 V, what will happen? Explain your answer.

A current of 3.00 A is passed through molten magnesium chloride (MgCl₂) for 2 hours. Calculate the mass of magnesium metal deposited at the cathode. (Molar mass of Mg = 24.3 g/mol, 1 Faraday = 96500 C)

A student sets up an electrolytic cell with aqueous potassium nitrate (KNO₃) and inert electrodes. Predict and explain the products formed at each electrode, considering the standard electrode potentials.