Electrolysis And Electrolytic Cell Test! Quiz

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| Attempts: 4,136 | Questions: 15

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1. The use of electric energy to bring about a chemical reaction is ____________.

A) corrosion

B) spontaneous combustion

C) a galvanic cell

D) an electrolytic ell

Electrolytic cells  a device in which electrolysis (chemical reaction involving oxidation and reduction) is carried out by using electricity or in which conversion of electrical energy into chemical energy is done.

Explanation

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About This Quiz

Electrolysis And Electrolytic Cell Test! Quiz - Quiz

Do you know anything about Electrolysis and Electrolytic cells? Do you think you can pass this quiz? An electrolytic cell utilizes electrical energy to drive a non- spontaneous... see moreredox reaction. The cell is often used to decompose chemical compounds in a process called electrolysis. It is a technique that uses a direct electric current. Take this quiz and learn more about electrolysis and electrolytic cells. see less

2. __________ are electrical conductors which are placed in an electrolyte to provide surfaces for oxidation and reduction half-reactions.

A) Electrolytes

B) Electrodes

C) Ions

D) Electrolysis

Electrodes are electrical conductors that are placed in an electrolyte to provide surfaces for oxidation and reduction half-reactions. They facilitate the transfer of electrons between the electrolyte and the external circuit, allowing the flow of current during electrolysis. Electrodes can be made of various materials, such as metals or graphite, depending on the specific application.

Explanation

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3. Which of the following statements is INCORRECT?

A) In an electrolytic cell, reduction occurs at the anode.

B) Aluminum metal would form at the cathode during the electrolysis of molten AlBr3.

C) The Anode is labeled "+" in an electrolytic cell.

D) Electrons move from the cathode to the anode through the internal supply.

Reduction occurs at the cathode while oxidation occurs at the anode.

Explanation

Reduction occurs at the cathode while oxidation occurs at the anode.

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4. Which of the following is NOT an electrolyte?

A) Sodium chloride solution

B) Aqueous ammonia

C) Molten sodium chloride

D) Molten naphtalene

Molten naphthalene does not have free ions.

Explanation

Molten naphthalene does not have free ions.

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5. Under standard conditions, which one of the following statements about the half cell process is true for the cell?

A) Cu2+ is reduced at the anode

B) Cu2+ is reduced at the cathode

C) Cd2+ is reduced at the anode

D) Cd2+ is reduced at the cathode

In a half cell process, reduction occurs at the cathode. Therefore, the correct answer is B) Cu2+ is reduced at the cathode.

Explanation

In a half cell process, reduction occurs at the cathode. Therefore, the correct answer is B) Cu2+ is reduced at the cathode.

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6. During the electrolysis of molten sodium iodide, sodium ions move ________.

A) to the anode, which is positively charged

B) to the cathode, which is positively charged

C) to the cathode, which is negatively charged

D) to the anode, which is negatively charged

In an electrolytic cell, the cathode is negative. In a galvanic cell, the cathode is positive.

Explanation

In an electrolytic cell, the cathode is negative. In a galvanic cell, the cathode is positive.

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7. What can be observed at the cathode of the platinum electrode?

A) A brown gas is released.

B) A grey solid is deposited.

C) The platinum electrode is corroded.

D) No observation.

Lead(II) ions move to the cathode. They receive an electron. Lead is formed.

Explanation

Lead(II) ions move to the cathode. They receive an electron. Lead is formed.

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The diagram above shows the electrolysis of molten lead(II) bromide, PbBr₂ using platinum electrodes. An electric current flows through molten lead (II) bromide for 10 minutes. What can be observed at the anode of the platinum electrode?

A) A brown gas is released.

B) A grey solid is deposited.

C) The platinum electrode is corroded.

D) No observation.

Bromide ions move to the anode and donate their electron. Bromine gas is releases.

Explanation

Bromide ions move to the anode and donate their electron. Bromine gas is releases.

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9. The electrolysis of an aqueous sodium chloride solution using inert electrodes produces gaseous chlorine at one electrode. At the other electrode, gaseous hydrogen is produced, and the solution around the electrode becomes basic. Which of the following equations is the correct equation for the cathode half-reaction in this electrolytic cell?

A) H2 + 2OH- → 2H2O + 2e-

B) 2H2O + 2e- → H2 + 2OH-

C) 2Cl- → Cl2 + 2e-

D) Cl2 + 2e- → 2Cl-

The correct equation for the cathode half-reaction in this electrolytic cell is B) 2H2O + 2e- → H2 + 2OH-. This is because gaseous hydrogen is produced at the cathode, which is represented by the H2 on the product side of the equation. Additionally, the solution around the electrode becomes basic, indicating the presence of hydroxide ions (OH-), which are represented on the product side of the equation as well. The 2e- on the reactant side of the equation represents the reduction of two electrons at the cathode.

Explanation

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10. Which of the following pair is CORRECT?

A) Anode: positive terminal where reducation occurs; Cathode: negative terminal where oxidation occurs

B) Anode: negative terminal where oxidation occurs; Cathode: postive terminal where reduction occurs

C) Anode: negative terminal where reduction occurs; Cathode: postive terminal where oxidation occurs

D) Anode: positive terminal where oxidation occurs; Cathode: negative terminal where reduction occurs

In an electrochemical cell, oxidation occurs at the anode, which is the electrode where electrons are lost. Since electrons are negatively charged, the anode must be the positive terminal. Reduction, on the other hand, occurs at the cathode, which is the electrode where electrons are gained. Since electrons are gained at the cathode, it must be the negative terminal. Therefore, option D is correct.

Explanation

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11. Which of the following are correct half-equations for the reactions happen at the anode and cathode?

A) Anode: 2Br-(l) --> Br2(g) + 2e-; Cathode: Pb(s) --> Pb2+(l) + 2e-

B) Anode: Pb2+(l) + 2e- --> Pb(s); Cathode: 2Br-(l) --> Br2(g) + 2e-

C) Anode: 2Br-(l) --> Br2(g) + 2e-; Cathode: Pb2+(l) + 2e- --> Pb(s)

D) Anode: Pb2+(l) + 2e- --> Pb (s); Cathode: Br2(g) + 2e- --> 2Br-(l)

The correct answer is C) Anode: 2Br-(l) --> Br2(g) + 2e-; Cathode: Pb2+(l) + 2e- --> Pb(s). This is the correct answer because at the anode, bromide ions (Br-) are oxidized to form bromine gas (Br2) and release two electrons. This is represented by the half-equation 2Br-(l) --> Br2(g) + 2e-. At the cathode, lead ions (Pb2+) are reduced and gain two electrons to form solid lead (Pb). This is represented by the half-equation Pb2+(l) + 2e- --> Pb(s).

Explanation

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12. In an electrolytic cell, the negative electrode is called the __________.

A) anode, at which oxidation occurs

B) anode, at which reduction occurs

C) cathode, at which oxidation occurs

D) cathode, at which reduction occurs

The negative electrode is known as the cathode. A positive electrode is called anode, where oxidation occurs.

Explanation

The negative electrode is known as the cathode. A positive electrode is called anode, where oxidation occurs.

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13. Which of the following statement about the transfer of charge in an electrolytic cell is INCORRECT?

A) Negative ions are called anions and positive ions are called cations.

B) Anions move through the electrolyte to the cathode and cations move to the anode.

C) An electrolyte conducts electricity by the movement of dissolved anions and cations.

D) Electrons travel from the negative terminal of the source to the cathode, and from the anode to the positive terminal of the source.

Anions move to the anode. Cations move to the cathode.

Explanation

Anions move to the anode. Cations move to the cathode.

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14. The anode and cathode are determined by the __________.

A) site of oxidation and reduction half-reactions.

B) movement of ions in the electrolyte

C) connection of terminals of the external sources

D) reduction potential s of ions

In an electrolytic cell, the anode and cathode are determined by the connection of terminals of the external sources. The electrode connected to the positive terminal is the anode.

Explanation

In an electrolytic cell, the anode and cathode are determined by the connection of terminals of the external sources. The electrode connected to the positive terminal is the anode.

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15. Which of the following will NOT affect the selective discharge of ions?

A) Types of electodes

B) Types of electrolyte

C) Positions of ions in the eletrochemical series

D) Concentration of ions in electrolysis

Types of electrolyte will not affect the product at the electrode.

Explanation

Types of electrolyte will not affect the product at the electrode.

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