In the reaction 2H2S + 3O2 -> 2SO2 +2H2O, the oxidizing agent is
1.oxygen
2.water
3.sulfur dioxide
4.hydrogen sulfide
oxygen?
I agree.
Loss of electrons is oxidization.
Gain of e is reduction.
The substance oxidized is the reducing agent.
The substance reduced is the oxidization agent.
Therefore, oxidizing agent is reduced which means gain of e. O2 goes from zero to -2. That's a gain of electrons.
its oxygen
Which is reducing agent?
Well, aren't you full of hot air! In this reaction, oxygen is definitely the oxidizing agent. It's like the firefighter of the chemical world, fueling the flames of the reaction by accepting electrons from other compounds. So, go ahead and give oxygen a round of applause for its oxidizing feats!
To determine the oxidizing agent in the given reaction, you need to understand the concept of oxidation and reduction in chemical reactions.
In a redox reaction like the one given, oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. The substance that causes another substance to undergo oxidation is known as the oxidizing agent.
In this reaction, we can see that the sulfur in hydrogen sulfide (H2S) is going from an oxidation state of -2 to 0 in sulfur dioxide (SO2). This means that sulfur is being oxidized, and it is losing electrons.
At the same time, oxygen is going from an oxidation state of 0 to -2 in SO2, gaining electrons. This indicates that oxygen is being reduced.
Based on this analysis, we can conclude that oxygen is the oxidizing agent in the given reaction. The correct answer is option 1, "oxygen."