Identify the oxidizing and reducing agents in each of the following redox reactions: (4 points) a) 2 H2O (l) + Al (s) + MnO4 -1(aq) ---→ Al(OH)4 -1(aq) + MnO2 (s)
Al (s) is a Reducig agent
MnO4^- (aq) is an Oxidation agent
2 H2O (l) + Al (s) + MnO4 -1(aq) ---→ Al(OH)4 -1(aq) + MnO2 (s)
Oxidation is the loss of electrons.
Reduction is the gain of electrons.
There is a mnemonic for that. "LEO the lion says GER"
LEO (loss electrons oxidation). GER (gain of electrons reduction).
Then you just remember that
The oxidizing agent is the one reduced.
The reducing agent is the one oxidized.
Here is how you do part of it. I'll leave the rest for you.
First you must determine the oxidation state of each of the elements in the equation. Initially that can be time consuming but with a little practice you will see that most of the elements are often the same.
If you don't know how to determine oxidation states or if you just need some practice or clarification, go to google and type in "chem team redox" and read #2 tutorial.
2 H2O (l) + Al (s) + MnO4 -1(aq) ---→ Al(OH)4 -1(aq) + MnO2 (s)
Al is zero on the left and +3 on the right; therefore, it has lost electrons. That makes it oxidized so it must be the reducing agent. Simple, huh?
Look at MnO4^- ==> MnO2 for the rest of it. Post your work if you get stuck or if you want to ask for clarification on an issue.
To identify the oxidizing and reducing agents, we need to determine which species is being oxidized and which is being reduced in the given redox reaction.
In the reaction:
2 H2O (l) + Al (s) + MnO4 -1(aq) → Al(OH)4 -1(aq) + MnO2 (s)
The species that is undergoing oxidation is the reducing agent, and the species that is undergoing reduction is the oxidizing agent.
In this case, the Al (s) is being oxidized to Al(OH)4 -1(aq), so Al (s) is the reducing agent.
The MnO4 -1(aq) is being reduced to MnO2 (s), so MnO4 -1(aq) is the oxidizing agent.
To summarize:
Reducing agent: Al (s)
Oxidizing agent: MnO4 -1(aq)
To identify the oxidizing and reducing agents in a redox reaction, you need to understand the concept of oxidation and reduction.
Oxidation is the process where a substance loses electrons, while reduction is the process where a substance gains electrons.
In the given redox reaction:
2 H2O (l) + Al (s) + MnO4 -1(aq) → Al(OH)4 -1(aq) + MnO2 (s)
Let's break down the reaction into half-reactions to identify the oxidizing and reducing agents.
Half-reaction 1: Oxidation of aluminum (Al):
Al (s) → Al(OH)4 -1(aq)
In this half-reaction, aluminum (Al) is oxidized from Al to Al(OH)4 -1. It loses electrons and increases its oxidation state from 0 to -1. Therefore, aluminum (Al) is the reducing agent.
Half-reaction 2: Reduction of manganese (Mn):
MnO4 -1(aq) → MnO2 (s)
In this half-reaction, the manganese ion (MnO4 -1) is reduced to manganese dioxide (MnO2). It gains electrons and decreases its oxidation state from +7 to +4. Therefore, the manganese ion (MnO4 -1) is the oxidizing agent.
To summarize:
- The reducing agent is aluminum (Al)
- The oxidizing agent is the manganese ion (MnO4 -1)