Question

5. Base your answer to the following question on the

reaction below
2 Cr(s) + 3 Cu2+ (aq) + 2 Cr3+ (aq) + 3 Cu(s)
The electronic equation that represents the oxidation
reaction that occurs is
A) 2Crº – 6e- →2Cr3+
B) 2Crº + 6e- + 2Cr3+
C) 2Cr3+ - 6e + 2Cro
D) 2Cr3+ + 6e + 2Crº​

Answer 1

The answer is B) is the correct answer

Answer 2

B) 2Crº + 6e- --> 2Cr3+

Step-by-step explanation:

The process of oxidation is where electrons are lost. Thus, out of the 2 ions that change charge(Cr and Cu), we must choose the one where the oxidation number increases(which means electrons are lost). Cr goes from an oxidation number of 0 to an oxidation number of 3+, while Cu goes from an oxidation number of 2+ to 0. Thus, we are looking at the half reaction for Cr. Half reactions never have subtracting electrons, so the answer must be B. I am assuming that last plus should be a -->