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

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

Chemistry
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At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

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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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