Which one of the following species will react with Sn at standard state conditions?
a) S
b) Ag+
c) Cu
d) Zn2+
This is not a confusing question. What is your question on this? Hint: it has to be able to absorb tin's electrons.
@bobpursley I don't understand what it means at standard state? Would it be Zn2+
To determine which of the species will react with Sn at standard state conditions, we can consider the reduction potentials (E°) of the species in question.
The reaction between two species is favorable if the reduction potential of the oxidizing agent is greater than the reduction potential of the reducing agent.
In this case, we are looking to see if Tin (Sn) can be oxidized by any of the given species.
Let's look at the reduction potentials of the given species:
a) S (Sulfur) - Sulfur does not typically exhibit a standard reduction potential as it is a non-metal element and is not commonly involved in redox reactions.
b) Ag+ (Silver ion) - The standard reduction potential (E°) of Ag+ is +0.80V.
c) Cu (Copper) - The standard reduction potential (E°) of Cu is +0.34V.
d) Zn2+ (Zinc ion) - The standard reduction potential (E°) of Zn2+ is -0.76V.
Comparing these values, we can see that the reduction potential of Sn (Tin) is higher than the reduction potential of Cu and Zn2+, but lower than the reduction potential of Ag+.
Therefore, the species that will react with Sn at standard state conditions is:
b) Ag+ (Silver ion)
To get this answer, we looked at the reduction potentials of the given species and compared them to the reduction potential of Sn.