Consider the following table of standard electrode potentials for a series of hypothetical reactions in an aqueous solution: reduction half-reaction E °(V) (c) Which substance(s) can oxidize C2+?

Video transcript

Welcome back everyone. The falling table lists a series of hypothetical reactions in aqueous solutions with their standard electrode potentials. We need to identify the substances that can oxidize Z two plus. So we should recall the trend that when we have a more negative value for our reduction potential measure, this is going to mean that. So let's say more negative here. This is going to mean that the substance is likely to go likely to undergo oxidation, whereas if we have a reduction potential that is more positive in value, that means the substance is likely to undergo a reduction. So looking at our chart, we see that for our zinc four plus Cat or Z four plus Catalan rather we have a reduction potential of negative 1.42. And so if we just go along with the substances that have a reduction potential greater than this value here, negative 1.42, we know that those substances should be able to oxidize our Z two plus carry on, meaning that for our final answer, the substances that can oxidize the Z two plus carry on would be all of the above reduction potentials associated with these half reactions of our W plus Catalon, X two plus Catalon and Ry three plus Catalan. And so our final answers are going to be the W plus Catalon, The X two plus catty on. And then our Y three plus Catalan All will be able to oxidize the Z2 plus Catalan due to their more positive reduction potential values. So for our final answers we would have these three substances highlighted. If you have any questions, please leave them down below. Otherwise, I will see everyone in the next practice video.