Textbook Question
Indicate whether each of the following statements is true or false: (b) For the reaction Fe3+(aq) + Co2+(aq) → Fe2+(aq) + Co3+(aq), Fe3+(aq) is the reducing agent and Co2+(aq) is the oxidizing agent.
6. Chemical Quantities & Aqueous Reactions
Redox Reactions
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Consider the reaction: Sn(s) + 4HNO3(aq) → SnO2(s) + 4NO2(g) + 2H2O(g). Use oxidation states to identify the element that is being oxidized in the redox reaction.
A
N
B
H
C
O
D
Sn
Verified step by step guidance1
Identify the oxidation states of each element in the reactants and products. For Sn(s), the oxidation state is 0 because it is in its elemental form.
Determine the oxidation state of Sn in SnO2. Oxygen typically has an oxidation state of -2. Since there are two oxygen atoms, the total oxidation state for oxygen is -4. To balance this, Sn must have an oxidation state of +4 in SnO2.
Compare the oxidation states of Sn in the reactants and products. Sn goes from an oxidation state of 0 in Sn(s) to +4 in SnO2.
Recognize that an increase in oxidation state indicates oxidation. Therefore, Sn is being oxidized in this reaction.
Conclude that Sn is the element being oxidized, as its oxidation state increases from 0 to +4 during the reaction.
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