What is the oxidizing agent in the following reaction? Sn(s) + 2HCl(aq) → SnCl2(aq) + H2(aq)
HCl
H2
Sn
SnCl2
.
Question 2
The following is an oxidation-reduction reaction: H2CO3(aq) → CO2(g) + H2O(l)
True
False
in the first equaiton, H+ gains an electron, it is reduced, therefore it is the oxidizing agent.
False.
In the reaction Sn(s) + 2HCl(aq) → SnCl2(aq) + H2(aq), the oxidizing agent is HCl.
For the second question, the statement "The following is an oxidation-reduction reaction: H2CO3(aq) → CO2(g) + H2O(l)" is false. This reaction represents a decomposition reaction, where H2CO3 breaks down into CO2 and H2O. It does not involve any oxidation or reduction reactions.
To identify the oxidizing agent in a chemical reaction, we need to determine the species that gets reduced. In the given reaction: Sn(s) + 2HCl(aq) → SnCl2(aq) + H2(aq), we see that Sn(s) is being oxidized because its oxidation state increases from zero to +2 in SnCl2(aq). This means that Sn(s) is losing electrons, thus acting as the reducing agent.
Conversely, in an oxidation-reduction reaction: H2CO3(aq) → CO2(g) + H2O(l), we observe that the carbon in H2CO3(aq) undergoes a decrease in oxidation state from +4 to +2 in CO2(g). Therefore, carbon is being oxidized, indicating that H2CO3(aq) is the reducing agent.
So, in both reactions, neither HCl nor H2 is the oxidizing agent. The answer for question 1 is Sn, and for question 2, the statement is False.