Consider the following substances: Fe2+(aq), Sn2+(aq), I-(aq). Identify the strongest reducing agent and the weakest reducing agent.

Video transcript

Hello in this problem we are asked given bromide calcium, MERCURY one and hydrogen gas to identify the weakest and the strongest reducing agent. So we call that the reducing agent is the element that's being oxidized. So if we arrange our reducing agent from strongest to weakest, then the element that has the greatest oxidation potential is going to be the strongest reducing agent. And the one with the lowest oxidation potential, who's gonna be the weakest reducing agent. So referring to an electrochemical series we are given than standard reduction potentials. So like for bro main being reduced to form bromide ions. Standard reduction potential Is equal to 1.09V. Find the standard oxidation potential. Then we are writing this reaction in reverse. So now we have the oxidation of bromide ions to form brewing And standard oxidation potential. Then since we changed the direction of the reaction is equal to the negative of the standard reduction potential. So this would be negative 1.09V. And so we can do the same thing for the other elements that are listed. So for calcium then calcium metal would be oxidized form calcium ions. Standard oxidation potential is 2.87V Mercury one then being oxidized to form mercury to as a standard oxidation potential of -0.92V. And our last one than hydrogen gas. His oxidized form howdy nines And the standard oxidation potential is 0V. So the one that has the most positive, then we'll be our strongest producing agent and the one that has the most negative oxidation potential will be the weakest producing agent. And so we have. Then calcium, with the more positive standard oxidation potential being the strongest reducing agent and bromine iron. That the standard oxidation potential of negative 1.09, which is the most negative, is the weakest reducing agent. Thanks for watching hope this help.