Molten CuBr2 is electrolyzed.
Which reaction occurs at the anode?
2e– + Cu2+(l) → Cu(l)
Oxidation occurs at the anode. In oxidation, reactants gain electrons. In this reaction, Cu2+ gains electrons and becomes metallic Cu.
2Br–(l) → Br2(g) + 2e–
Oxidation occurs at the anode. In oxidation, reactants lose electrons. In this reaction, Br– loses electrons and becomes Br2 gas.
Br2(g) + 2e– → 2Br–(l)
Oxidation occurs at the anode. In oxidation, reactants gain electrons. In this reaction, Br2 gas gains electrons and becomes Br– ions.
Cu(l) → 2e– + Cu2+(l)
Oxidation occurs at the anode. In oxidation, reactants lose electrons. In this reaction, metallic Cu loses electrons and becomes Cu2+ ions.
Why don't you write out the equation of the electrolysis?
CuBr2 ==> Cu + 2Br^-
Cu changes oxidation state from 2+ to 0 so it gains electrons. Right?
2Br^- ==> Br2(l)
Br changes oxidation state from a total of 2- to 0 so it loses electrons. Right?
And the definition: Oxidation occurs at the anode.
ipso facto
The correct answer is "Br2(g) + 2e– → 2Br–(l)". In the electrolysis of molten CuBr2, the oxidation reaction occurs at the anode. In this specific reaction, Br2 gas gains electrons and becomes Br– ions.
The correct answer is: 2Br–(l) → Br2(g) + 2e–
In electrolysis, the anode is the positive electrode where oxidation occurs. Oxidation involves the loss of electrons. In this reaction, the bromide ions (Br–) lose electrons and are oxidized to form bromine gas (Br2).
To determine the correct answer, we need to understand the concept of oxidation and reduction in electrolysis. In electrolysis, an external electrical energy source is used to drive a non-spontaneous chemical reaction. The process involves the flow of electric current through an electrolyte solution or a molten salt.
At the anode, oxidation takes place, where reactants lose electrons. The anode is positive because it attracts negatively charged ions. In this case, CuBr2 is being electrolyzed, so the Cu2+ ions and the Br– ions are involved in the reaction.
We can analyze the reactions given to determine which one represents oxidation at the anode. Oxidation involves the loss of electrons, so we are looking for a reaction where the reactants lose electrons. The only reaction where this occurs is 2Br–(l) → Br2(g) + 2e–.
Therefore, the correct reaction that occurs at the anode during the electrolysis of molten CuBr2 is 2Br–(l) → Br2(g) + 2e–.