Will Fan and medal: For the complete redox reaction given here a) break down each reaction into its half reactions b) Identify the oxidizing agent and c) Idenify te reducing agent. 2FeCl2+SnCl4->2FeCl3+SnCl2

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Will Fan and medal: For the complete redox reaction given here a) break down each reaction into its half reactions b) Identify the oxidizing agent and c) Idenify te reducing agent. 2FeCl2+SnCl4->2FeCl3+SnCl2

Chemistry
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c).2) Fe is losing electrons (1) 3) Sn is gaining electrons (2) 4) FeCl3 is reduced to FeCl2, as Fe's oxidation state goes from +3 to +2 5) SnCl2 is oxidised to SnCl4, as Sn's oxidation state goes from +2 to +4 6) Since SnCl2 donates the electrons to become oxidised, it's the reducing agent 7) Since FeCl2 gains electrons from another compound, it is oxidising the other one, so it's the oxidising agent
What is the half reaction? @parker.goodbar
2) and 3) are correct all the other are incorrect 4) FeCl3 is reduced to FeCl2, as Fe's oxidation state goes from +3 to +2 what you wrote is correct but doesnt match with the reaction.In the reaction is happening the opposite is FeCl2 -> FeCl3 5) SnCl2 is oxidised to SnCl4, as Sn's oxidation state goes from +2 to +4 here the same issue than in 4) 6) if you in 3 said that 3) Sn is gaining electrons you can not said in 6) Since SnCl2 donates the electrons to become oxidised, it's the reducing agent

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2FeCl2+SnCl4->2FeCl3+SnCl2 Cl- + FeCl2 -> FeCl3 + 1 e- (oxidation) 2 e- + SnCl4->SnCl2 + 2 Cl- (reduction)
then the oxidizing agent is FeCl2 and the reducing agent is SnCl2 right??? @Cuanchi
no the other way around, the one that get reduce is the oxidizing agent and the one that get oxidated is the reducing agent :)

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