Basic Understanding Of Electrolysis Quiz

Reviewed by Editorial Team
The ProProfs editorial team is comprised of experienced subject matter experts. They've collectively created over 10,000 quizzes and lessons, serving over 100 million users. Our team includes in-house content moderators and subject matter experts, as well as a global network of rigorously trained contributors. All adhere to our comprehensive editorial guidelines, ensuring the delivery of high-quality content.
Learn about Our Editorial Process
| By Lucasyhw
L
Lucasyhw
Community Contributor
Quizzes Created: 1 | Total Attempts: 1,676
| Attempts: 1,678
Quiz Flashcard
SettingsSettings
Please wait...
  • 1/7 Questions

    Bob wants to have a silver coated knife, he knows he can do it using electrolysis. He prepares Silver Nitrate solution as the electrolyte he is going to use. But firstly what should he put at the cathode and anode so that he gets his silver-plated knife?

    • Cathode : Knife ; Anode: Silver metal
    • Cathode: Silver metal ; Anode: Knife
    • It is fine both ways
Please wait...
About This Quiz

When studying any realm of science, it’s always smart to try to come to terms with the basics before you tackle anything more complex. In this quiz on the process of electrolysis, we aim to do just that – give you a basic understanding of electrolysis in the hopes of expanding it at a later date.

Basic Understanding Of Electrolysis Quiz - Quiz

Quiz Preview

  • 2. 

    Which of the following is not an inert electrode?

    • Platinum

    • Mercury

    • Graphite

    Correct Answer
    A. Mercury
    Explanation
    Mercury is not an inert electrode because it can participate in redox reactions. Inert electrodes do not undergo any chemical reactions during an electrochemical process and only serve as a conductor for the flow of electrons. Platinum and graphite are examples of inert electrodes commonly used in electrochemical cells, while mercury can be oxidized or reduced, making it an active electrode.

    Rate this question:

  • 3. 

    Bob knows why he did not obtain his sodium metal when he electrolysed the sodium chloride solution he prepared. But he is now curious of how come Hydrogen ions can get discharged at the cathode. He came to the conclusion that it is beacause electrons from the current are transferred to the hydrogen ions to make them become hydrogen atoms.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    The explanation for the given answer is that when Bob electrolysed the sodium chloride solution, the positively charged sodium ions migrated towards the cathode. However, instead of being discharged, the hydrogen ions present in the solution were discharged at the cathode. This is because the electrons from the current were transferred to the hydrogen ions, causing them to become hydrogen atoms. Therefore, the statement that hydrogen ions can get discharged at the cathode due to the transfer of electrons is true.

    Rate this question:

  • 4. 

    Bob is doing an electrolysis experiment and he wants to obtain sodium metal. He has a typical electrolysis set-up with Graphite electrodes. He has a bottle of Sodium Chloride crystals. What should he do with the Sodium Chloride crystals before he starts the experiment , so that he gets the result he wants?

    • Put the NaCl crystals into the crucible

    • Dissolve the NaCl crystals in water

    • Melt the NaCl crystals

    Correct Answer
    A. Melt the NaCl crystals
    Explanation
    In order to obtain sodium metal through electrolysis, Bob needs to have the sodium ions in a molten state. By melting the NaCl crystals, the sodium and chloride ions will separate, allowing the sodium ions to be attracted to the cathode and be reduced to sodium metal. Dissolving the NaCl crystals in water would not allow the ions to be separated and would not result in the formation of sodium metal. Putting the NaCl crystals into the crucible without melting them would also not allow for the separation of the ions and the formation of sodium metal.

    Rate this question:

  • 5. 

    In the electrolysis of Dilute Sulfuric Acid, the gas produced at the cathode can rekindle a glowing splint.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    In the electrolysis of Dilute Sulfuric Acid, the gas produced at the cathode is hydrogen gas (H2). Hydrogen gas is highly flammable and can burn with a pop sound when ignited. It does not rekindle a glowing splint, but rather extinguishes it. Therefore, the statement is false.

    Rate this question:

  • 6. 

    In the extraction of aluminium from bauxite, carbon anodes are used. Why must the carbon anodes be constantly changed after a certain period of time?

    • The carbon anodes reacted with the electrolyte

    • The carbon from the carbon anodes dissolve into the electrolyte and migrates to the cathode

    • The oxygen liberated at the anode reacts with the carbon anodes

    Correct Answer
    A. The oxygen liberated at the anode reacts with the carbon anodes
    Explanation
    The oxygen liberated at the anode reacts with the carbon anodes, causing them to gradually deteriorate and reduce in size. As the carbon anodes dissolve into the electrolyte, they migrate to the cathode, resulting in a loss of material from the anodes. Therefore, the carbon anodes need to be constantly changed after a certain period of time to maintain the efficiency of the extraction process.

    Rate this question:

  • 7. 

    In the electrolysis of Copper(II) Sulfate solution, Copper(II) ions are preferentially discharged because of its lower position in the reactivity series as compared to Hydrogen ions.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    In the electrolysis of Copper(II) Sulfate solution, Copper(II) ions are not preferentially discharged because of its lower position in the reactivity series as compared to Hydrogen ions. In fact, during electrolysis, the more reactive species is preferentially discharged at the cathode, while the less reactive species is discharged at the anode. Since Copper(II) ions are less reactive than Hydrogen ions, they will be discharged at the anode, while Hydrogen ions will be discharged at the cathode. Therefore, the given statement is false.

    Rate this question:

Quiz Review Timeline (Updated): Mar 21, 2023 +

Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • May 07, 2011
    Quiz Created by
    Lucasyhw
Back to Top Back to top
Advertisement
×

Wait!
Here's an interesting quiz for you.

We have other quizzes matching your interest.