Question
Following question I need help with part b) Please verify my answer for part a) too if possible.
Consider the following reaction for silver tarnishing:
3Ag2S(s) + 2Al(s) -> 6Ag(s) + Al2S3(s)
a. State the oxidation number for each element in the reaction.
3Ag2S(s) + 2Al(s) -> 6Ag(s) + Al2S3(s)
(+1)+(-2)+(+3) -> (+1)+(+3)+(-2)
verify these please
b. Identify the oxidized reactant and the reduced reactant.
Please help me with b) above....
Consider the following reaction for silver tarnishing:
3Ag2S(s) + 2Al(s) -> 6Ag(s) + Al2S3(s)
a. State the oxidation number for each element in the reaction.
3Ag2S(s) + 2Al(s) -> 6Ag(s) + Al2S3(s)
(+1)+(-2)+(+3) -> (+1)+(+3)+(-2)
verify these please
b. Identify the oxidized reactant and the reduced reactant.
Please help me with b) above....
Answers
DrBob222
All of the oxidation numbers are right except for Al(s). All elements in the free state have an oxidation number of zero. (Note: I don't consider the reaction written as the reason silver tarnishes. Rather it is a way of removing the sulfide from silver that is tarnished.
For the part b, oxidation is the loss of electrons. Reduction is the gain of electrons. Which element/ion loses and which gains electrons.
For the part b, oxidation is the loss of electrons. Reduction is the gain of electrons. Which element/ion loses and which gains electrons.
Dexter
Yes that's right, free states have oxidation number of zero. Ok will work out reduction and oxidation, made it a bit clearer. Thanks for your help, very valuable :)