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Question 1/101/10
Electrode materials - Inert and active electrodes
Electrode materials - Inert and active electrodes
Electrode materials - Inert and active electrodes
A copper(II) sulfate solution is electrolysed using copper electrodes. Compared with using platinum electrodes, what change is expected at the anode?
Select the answer:Select the answer
1 correct answer
A.
Copper ions are reduced and the anode gains mass
B.
Water is oxidised and the anode remains unchanged
C.
Copper atoms are oxidised and the anode gradually dissolves
D.
Sulfate ions are reduced and the anode becomes coated with copper
Copper is an active electrode in copper(II) sulfate solution, so copper atoms at the anode are oxidised to Cu²⁺ ions and enter the solution, causing the anode to lose mass. Platinum is inert and would not normally participate in this electrode reaction.
Right Answer: C
Quiz
Question 2/102/10
Industrial electrolysis of brine
Industrial electrolysis of brine
Industrial electrolysis of brine
In a membrane cell used for the industrial electrolysis of concentrated brine, the membrane separates the anode and cathode compartments. What is the main reason for this separation?
Select the answer:Select the answer
1 correct answer
A.
To prevent chlorine from reacting with sodium hydroxide formed at the cathode
B.
To increase the electrical conductivity of the brine solution
C.
To ensure that hydrogen is oxidised at the anode instead of chloride ions
D.
To allow sodium ions to be discharged preferentially at the cathode
Chlorine is produced at the anode, while hydrogen and sodium hydroxide are formed in the cathode compartment. The membrane allows sodium ions to pass through but limits mixing, preventing chlorine from reacting with sodium hydroxide to form unwanted products such as hypochlorite. Its main purpose is not to increase conductivity or change which species is discharged.
Right Answer: A
Quiz
Question 3/103/10
Extraction of aluminium by electrolysis
Extraction of aluminium by electrolysis
Extraction of aluminium by electrolysis
In the electrolytic extraction of aluminium, alumina is dissolved in molten cryolite rather than electrolysed as pure molten alumina. What is the main purpose of using cryolite?
Select the answer:Select the answer
1 correct answer
A.
To react with aluminium oxide and form aluminium chloride
B.
To lower the operating temperature and improve the electrolyte's electrical conductivity
C.
To prevent oxygen ions from reaching the positive electrode
D.
To provide the aluminium ions that are discharged at the negative electrode
Cryolite dissolves alumina, lowers the melting point of the mixture and improves its electrical conductivity, making electrolysis more practical. It does not supply the aluminium ions; those come from the dissolved aluminium oxide.
Right Answer: B
Quiz
Question 4/104/10
Electroplating
Electroplating
Electroplating
A steel component is to be coated with copper using an aqueous copper sulfate solution and a copper electrode. Which arrangement will produce the intended coating?
Select the answer:Select the answer
1 correct answer
A.
Connect the steel component to the positive terminal and use the copper electrode as the cathode
B.
Connect both electrodes to the negative terminal so copper ions are attracted to the steel
C.
Connect the steel component to the negative terminal and use the copper electrode as the anode
D.
Connect the steel component to the positive terminal and use an inert electrode as the anode
The component being plated must be the cathode, connected to the negative terminal, because copper ions gain electrons there and are reduced to copper metal. The copper electrode acts as the anode, where copper dissolves to replenish copper ions in the solution.
Right Answer: C
Quiz
Question 5/105/10
Electrolytes and ionic conduction
Electrolytes and ionic conduction
Electrolytes and ionic conduction
A student states: “In an aqueous sodium chloride electrolysis cell, the electric current is carried through the solution by electrons moving between the electrodes.” Which correction is most accurate?
Select the answer:Select the answer
1 correct answer
A.
Electrons carry the current through the solution, while sodium and chloride ions carry it through the wires
B.
Sodium ions carry the current through the solution, while chloride ions carry it through the external circuit
C.
Positive and negative ions carry the current through the solution, while electrons carry it through the external circuit
D.
Chloride ions carry the current through the solution, while sodium ions carry it through the external circuit
In the electrolyte, charged ions migrate and transport charge: cations move towards the cathode and anions towards the anode. In the metallic wires and electrodes, charge is transported by electrons. The types of charge carriers therefore change at the electrode–electrolyte interface.
Right Answer: C
Quiz
Question 6/106/10
Electrolytic cells - Components and circuit operation
Electrolytic cells - Components and circuit operation
Electrolytic cells - Components and circuit operation
During setup of an electrolytic cell, a technician connects the negative terminal of a direct-current power supply to one electrode and the positive terminal to the other. Which statement correctly describes the electrode connected to the negative terminal?
Select the answer:Select the answer
1 correct answer
A.
It is the anode, where oxidation takes place
B.
It is the anode, where reduction takes place
C.
It is the cathode, where reduction takes place
D.
It is the cathode, where oxidation takes place
In an electrolytic cell, the external power supply drives a non-spontaneous reaction. Electrons are supplied to the negative electrode, making it the cathode, where reduction occurs. Oxidation occurs at the positive anode.
Right Answer: C
Quiz
Question 7/107/10
Electrolysis of molten ionic compounds
Electrolysis of molten ionic compounds
Electrolysis of molten ionic compounds
Molten lead(II) bromide is electrolysed using inert electrodes. Which combination correctly describes the products and the electrode reactions?
Select the answer:Select the answer
1 correct answer
A.
Lead forms at the anode by oxidation, while bromine forms at the cathode by reduction
B.
Lead forms at the cathode by reduction, while bromine forms at the anode by oxidation
C.
Bromine forms at both electrodes because bromide ions are present in the electrolyte
D.
Lead(II) bromide remains unchanged because its ions cannot move when molten
In the molten compound, Pb2+ ions move to the cathode and gain electrons to form lead: Pb2+ + 2e− → Pb. Br− ions move to the anode and lose electrons to form bromine: 2Br− → Br2 + 2e−. The other options reverse the electrode processes or incorrectly assume that molten ions cannot move.
Right Answer: B
Quiz
Question 8/108/10
Electrolysis of aqueous solutions - Predicting electrode products
Electrolysis of aqueous solutions - Predicting electrode products
Electrolysis of aqueous solutions - Predicting electrode products
An aqueous solution of copper(II) sulfate is electrolysed using inert electrodes. Which pair of products is expected at the cathode and anode, respectively?
Select the answer:Select the answer
1 correct answer
A.
Hydrogen and sulfur dioxide
B.
Copper and oxygen
C.
Copper and sulfur dioxide
D.
Hydrogen and oxygen
At the cathode, Cu²⁺ ions are preferentially reduced to copper because copper is less reactive than hydrogen. At the anode, sulfate ions are not readily discharged, so hydroxide ions from water are oxidised to form oxygen.
Right Answer: B
Quiz
Question 9/109/10
Electrode half-equations and overall cell equations
Electrode half-equations and overall cell equations
Electrode half-equations and overall cell equations
A student electrolyses aqueous copper(II) sulfate using inert electrodes. Which combination correctly gives the electrode half-equations and the overall ionic equation?
At the cathode, copper(II) ions gain electrons and are reduced to copper. At the inert anode, hydroxide ions are oxidised to oxygen. The half-equations balance to give 2Cu²⁺ + 2H₂O → 2Cu + O₂ + 4H⁺. Chloride ions are not present in copper(II) sulfate solution, so the chlorine equation is not applicable.
Right Answer: B
Quiz
Question 10/1010/10
Faraday's laws of electrolysis
Faraday's laws of electrolysis
Faraday's laws of electrolysis
A metal is deposited during electrolysis using a current of 1.5 A for 20 minutes. If the same electrolyte is electrolysed with a current of 3.0 A for 10 minutes, how will the mass of metal deposited compare, assuming the current efficiency is unchanged?
Select the answer:Select the answer
1 correct answer
A.
It will be half as great
B.
It will be twice as great
C.
It will be the same
D.
It will be four times as great
Faraday's first law states that the mass deposited is proportional to the quantity of electricity passed, Q = It. In the first case, Q = 1.5 × 20; in the second, Q = 3.0 × 10. The charges are equal, so the deposited masses are equal.
Electrolysis Practice Test Practice test unlocks all online simulator questions
Thank you for choosing the free version of the Electrolysis Practice Test practice test! Further deepen your knowledge on Assessment Test Simulator; by unlocking the full version of our Electrolysis Practice Test Simulator you will be able to take tests with over 783 constantly updated questions and easily pass your exam. 98% of people pass the exam in the first attempt after preparing with our 783 questions.
What to expect from our Electrolysis Practice Test practice tests and how to prepare for any exam?
The Electrolysis Practice Test Simulator Practice Tests are part of the Assessment Test Database and are the best way to prepare for any Electrolysis Practice Test exam. The Electrolysis Practice Test practice tests consist of 783 questions divided by 16 topics and are written by experts to help you and prepare you to pass the exam on the first attempt. The Electrolysis Practice Test database includes questions from previous and other exams, which means you will be able to practice simulating past and future questions. Preparation with Electrolysis Practice Test Simulator will also give you an idea of the time it will take to complete each section of the Electrolysis Practice Test practice test . It is important to note that the Electrolysis Practice Test Simulator does not replace the classic Electrolysis Practice Test study guides; however, the Simulator provides valuable insights into what to expect and how much work needs to be done to prepare for the Electrolysis Practice Test exam.
Electrolysis Practice Test Practice test therefore represents an excellent tool to prepare for the actual exam together with our Assessment Test practice test . Our Electrolysis Practice Test Simulator will help you assess your level of preparation and understand your strengths and weaknesses. Below you can read all the quizzes you will find in our Electrolysis Practice Test Simulator and how our unique Electrolysis Practice Test Database made up of real questions:
Info quiz:
Quiz name:Electrolysis Practice Test
Total number of questions:783
Number of questions for the test:50
Pass score:70%
Number of topics:16 Topics
Study topics:Number of questions:
Electrical energy, cell voltage and current efficiency:49 Questions
Electrode half-equations and overall cell equations:55 Questions
Electrode materials - Inert and active electrodes:50 Questions
Electrolysis of aqueous solutions - Predicting electrode products:55 Questions
Electrolysis of molten ionic compounds:57 Questions
Electrolysis safety and environmental impacts:40 Questions
Electrolytes and ionic conduction:59 Questions
Electrolytic cells - Components and circuit operation:21 Questions
Electrolytic extraction and purification of copper:44 Questions
Electroplating:39 Questions
Extraction of aluminium by electrolysis:44 Questions
Faraday's laws of electrolysis:60 Questions
Industrial electrolysis of brine:44 Questions
Quantitative electrolysis - Charge, current, time, mass and gas volume calculations:59 Questions
Redox reactions at the anode and cathode:58 Questions
Selective discharge of ions:49 Questions
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