Identify the elements or compounds in the following reaction that are oxidized and reduced. 4 Hg + SnO2 -----> 2 Hg2O + Sn

Question

Then, identify the oxidizing agent and the reducing agent. Finally, identify the oxidation states of all elements in the reaction.

Answer 1

To find which elements/compound are oxidized and/or reduced, you want to determine the oxidation number of each element on both sides of the equation. Then see which ones increase or decrease and that will tell you which are oxidized and reduced.

4Hg + SnO₂ --> 2Hg₂O + Sn

0........4+...2-........1+..........0 ... oxidation numbers of each element

Hg on the left is zero and on the right it is 1+. This means Hg has been oxidized

Sn on the left is 4+ and on the right it is zero. This means Sn has been reduced

O on the left is 2- and on the right is 2-. It has not changed.

If you are not sure how to determine the oxidation numbers of elements, maybe you could submit a separate question asking for instruction on this aspect. We'd be glad to help.