the oxidation and half-reaction of a redox reaction is Sn*2+ --> Sn *4 +2e- and the reduction half-reaction is Au*3+ +3e- -->Au
what minimum numbers of tin (II) ions and gold (III) ions would have to react in order to have no electrons left over???
2006-12-12 08:28:56 · 3 answers · asked by babycakez 3 in Science & Mathematics ➔ Chemistry
Phys... is indeed correct. You multiply the equations by his numbers and add them up:
3Sn*2+ ===> 3Sn*4+ + 6e-
2Au*3+ +6e- ===> 2Au
draw a line under the bottom
With respect to gatorboi, it is obvious that tin in the oxidation state of +2 will react vigorously with gold in the oxidation state of +3. This is because gold is a very unreactive metal. Given a chance, gold(III) will take electrons from almost anything to get back to gold(0).
2006-12-12 09:06:21 · answer #1 · answered by steve_geo1 7 · 2⤊ 0⤋
3 Sn 2+ and 2 Au 3+ need to react.
3 Sn2+ will donate a total of 6 e-. 2 Au 3+ will accept a total of 6 e-.
2006-12-12 08:35:32 · answer #2 · answered by physandchemteach 7 · 3⤊ 0⤋
Hey Bebe,
You do not seem novice because the questions you are asking are obvious. You answered you own question. and I think that if you did the electron loss sentences then you must know to mutlitpy the electrons. also if you know this much you know that Tin and Gold are not likely to react with each other.
2006-12-12 08:42:14 · answer #3 · answered by gatorboi19884870 3 · 0⤊ 1⤋