How do I find the answer to this??
Cu metal displaces Ag+(aq) from an aqueous solution. Which of the following is correct?
Ag is easier to oxidize than Cu
Ag is a better reducing agent than Cu
Cu2+ is a better oxidizing agent than Ag+
Ag+ is easier to reduce than Cu2+
so thinking, you have silver ions in solution, and they are able to grab the electrons from the copper atoms, putting the copper into solution, where it exists without that electron.
silver gained electron: reduced, oxidizing agent
Copper atom lost electron, oxidized
Ag+ is easier to reduce than Cu2+
Ag+ is easier to reduce than Cu2+
If Cu displaces Ag^+ from solution then
Cu(s) + 2Ag^+*(aq) ==> Cu^2+|(aq) + 2Ag(s))
Oxidation is the loss of electrons and is the reducing agent.
Reduction is the gain of electrons and is the oxidizing agent.
So Cu changes from zero on the left to +2 on the right.
Ag changes from +1(for each) on the left to zero on the right.
Can you go from there?
To find the correct answer to the given statement, we can examine the standard reduction potentials of Cu and Ag and determine which species is easier to oxidize or reduce.
The standard reduction potential values are used to compare the ease of oxidation or reduction of different species. The more positive the standard reduction potential, the easier the species can be reduced (better reducing agent). The more negative the standard reduction potential, the easier the species can be oxidized (better oxidizing agent).
Based on the given statement, Cu metal displaces Ag+(aq) from an aqueous solution. Therefore, Cu is oxidized, and Ag+ is reduced.
Comparing the standard reduction potentials:
- The standard reduction potential for the reduction of Cu2+ is +0.34 V.
- The standard reduction potential for the reduction of Ag+ is +0.80 V.
From these values, we can see that Ag+ has a more positive standard reduction potential than Cu2+. This means that Ag+ is easier to reduce than Cu2+, making Ag+ a better reducing agent than Cu.
Therefore, the correct option is:
Ag is a better reducing agent than Cu.
To find the answer to this question, you need to understand the concept of displacement reactions and the reactivity series of metals. The reactivity series arranges metals in order of their reactivity, with the most reactive metal at the top and the least reactive metal at the bottom.
In a displacement reaction, a more reactive metal can displace a less reactive metal from its compound in aqueous solution. Looking at the given reaction, Cu metal is displacing Ag+ from an aqueous solution. Based on this information, we can make the following observations:
1. Ag is being displaced by Cu, indicating that Cu is more reactive than Ag.
2. Cu is oxidizing Ag+ to Ag since Ag is being reduced.
3. Cu is acting as the reducing agent in this reaction, while Ag+ is the oxidizing agent.
Now, let's analyze the options:
A. Ag is easier to oxidize than Cu: This is incorrect. Cu is easier to oxidize since it is displacing Ag+ from solution.
B. Ag is a better reducing agent than Cu: This is incorrect. Cu is a better reducing agent, as it can reduce Ag+ to Ag.
C. Cu2+ is a better oxidizing agent than Ag+: This is incorrect. Ag+ is a better oxidizing agent, as it can oxidize Cu to Cu2+.
D. Ag+ is easier to reduce than Cu2+: This is correct. Ag+ is easier to reduce than Cu2+, as Cu can displace Ag+ from the solution.
Therefore, the correct answer is D. Ag+ is easier to reduce than Cu2+.