Identify the Oxidizing agent and the reducing agent for Al(s)+3Ag^+(aq)--->Al^3+(aq)+3Ag(s)
Express your answers as chemical formulas serperated by a comma.
I tried putting in Al,3Ag^+
and 3Ag,Al^3+
I keep getting it wrong and only have one attempt left I need help please.
Ag^+ is the oxidizing agent.
Al is the reducing agent.
So I would write Ag^+,Al
Remember, oxidation is the loss of electrons. Al goes from zero to +3 which is a loss of electrons; therefore, Al is oxidized which makes it the reducing agent.
Reduction is the gain of electrons. Ag^+ goes from +1 (each) to zero which is a gain of electrons. This is reduction so it is the oxidizing agent. You don't need the coefficients to identify the formula.
Oh no, it seems like you're in a bit of a pinch!
Alright, let's sort this out. In a redox reaction like this one, the oxidizing agent is the species that gets reduced, while the reducing agent is the species that gets oxidized.
In the given reaction:
Al(s) + 3Ag^+(aq) ---> Al^3+(aq) + 3Ag(s)
We see that Al is going from its elemental form (Al(s)) to the Al^3+ ion. This means it's losing electrons and undergoing oxidation. So, Al is the reducing agent.
On the other side, Ag^+ is going from the Ag^+ ion to its elemental form (Ag(s)). It's gaining electrons and undergoing reduction. Therefore, Ag^+ is the oxidizing agent.
So, the correct answer is Al,Ag^+. You've got this!
To identify the oxidizing agent and the reducing agent, we need to determine which species is being reduced and which one is being oxidized.
In the given reaction:
Al(s) + 3Ag+(aq) → Al^3+(aq) + 3Ag(s)
The Ag+ ions (Ag+(aq)) gain electrons and are reduced to Ag(s), so Ag+ is the oxidizing agent (that causes the oxidation of Al).
On the other hand, Al(s) loses electrons and is oxidized to Al^3+, so Al is the reducing agent (that causes the reduction of Ag+).
To summarize:
Oxidizing agent: Ag+
Reducing agent: Al
So, the correct answer is Ag+, Al.
To identify the oxidizing and reducing agents in a chemical reaction, we need to analyze the changes in oxidation states of the elements involved.
In the given reaction: Al(s) + 3Ag^+(aq)→ Al^3+(aq) + 3Ag(s)
First, let's determine the oxidation states.
The oxidation state of elemental aluminum (Al) is 0 since it is uncombined, and the oxidation state of silver (Ag) is +1 in the Ag+ ion and 0 in the elemental form.
Analyzing the reaction, we see that the aluminum (Al) is oxidized from 0 to +3 since it loses three electrons, and the silver ions (Ag+) are reduced from +1 to 0 since they gain three electrons.
From this analysis, we can conclude that aluminum (Al) is the reducing agent, as it causes the silver ions to undergo reduction. On the other hand, the silver ions (Ag+) are the oxidizing agent since they cause aluminum to undergo oxidation.
Therefore, the answers in chemical formulas are:
Oxidizing agent: Ag+
Reducing agent: Al
Make sure to write the formulas correctly, using appropriate chemical symbols and correct charge notations.