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identify the oxidizing agent in the reaction SnO2(s) + 2C(s) > Sn(l) + 2CO(g)

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SnO2 -> Sn Sn oxidation states: +4 -> 0 So Sn is being reduced, thus SnO2 is the oxidizing agent.
thank you! one more question, how did you get the oxidation state on SnO2 as +4?
there are guidelines (look these up on google) to appoint oxidation states to certain elements according to their place on the periodic table.. per say, K and H are always +1, O is always -2, etc... then you add up the number to equal zero, unless they have a charge.. eg. NO ... since O is always -2, N must be +2. CO2 .. O is -2 but there are two of them, so -4, therefore C is +4. HCl.. H is +1, Cl must be -1 NH4+ .. H is +1, positive charge account for one H.. so you have +3, N is-3.

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okay I understand it now thank you so much!

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