In electrolysis of aqueous CuCl2, the metal deposited at the cathode is:
Correct answer: D. Cu
- A. Na
- B. Al
- C. Pb
- D. Cu
Explanation
Copper deposits at cathode and chlorine is liberated at anode.During the electrolysis of aqueous CuCl2, Cu²⁺ ions and H⁺ ions are present in the solution. At the anode, Cl⁻ ions are oxidized to Cl₂ gas:2Cl⁻ → Cl₂ + 2e⁻At the cathode, Cu²⁺ ions are reduced to Cu metal:Cu²⁺ + 2e⁻ → CuTherefore, the metal deposited at the cathode is copper (Cu).
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Electrochemistry
Electrochemistry describes electron transfer through oxidation and reduction, identifies oxidizing and reducing agents, and applies oxidation numbers to balance redox equations. It also covers electrode potential and the standard hydrogen electrode, which provides the reference for comparing the reduction tendencies of other electrodes.
Practise Electrochemistry
696 free Electrochemistry MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Electrochemistry questions
Study the following facts:Zn → Zn+2 + 2e― Eo = +0.76 VCu → Cu+2 + 2e― Eo = - 0.34 V
By accepting an electron, a Hydronium ion is converted into:
In metal hydrides the oxidation number of hydrogen is:
In MgCl2, the oxidation state of 'Cl' is :
In electrolytic cell, a salt bridge is used in order to:
In all oxidation reactions, atoms of an element in a chemical species lose electrons and increase their: