Multiple Choice
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.
6. Chemical Quantities & Aqueous Reactions
Redox Reactions
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The reaction Cu(s) + 2 AgNO3(aq) → Cu(NO3)2(aq) + 2 Ag(s) is best classified as a(n):
A
precipitation reaction
B
acid-base reaction
C
combustion reaction
D
redox reaction
Verified step by step guidance1
Identify the type of reaction by analyzing the reactants and products. In this case, we have copper (Cu) reacting with silver nitrate (AgNO3) to form copper(II) nitrate (Cu(NO3)2) and silver (Ag).
Recognize that a redox reaction involves the transfer of electrons between species. In this reaction, copper (Cu) is oxidized to copper(II) ions (Cu^2+), and silver ions (Ag^+) are reduced to silver metal (Ag).
Determine the oxidation states of the elements involved. Copper starts with an oxidation state of 0 and changes to +2 in Cu(NO3)2, indicating it loses electrons. Silver starts with an oxidation state of +1 in AgNO3 and changes to 0 in Ag, indicating it gains electrons.
Confirm that the reaction involves both oxidation and reduction processes. Copper is oxidized (loses electrons), and silver is reduced (gains electrons), which is characteristic of a redox reaction.
Conclude that the reaction is best classified as a redox reaction because it involves the transfer of electrons between copper and silver ions, resulting in changes in their oxidation states.
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