Which element is oxidized in this reaction?
Fe2O3+ 3CO-(arrow)2Fe+3CO2
it is C
Oxidized: loses electrons...
Fe+2 gains electrons
C starts at +2, ends at +4, it lost 2 electrons.
O starts at -2, ends at -2
Well, in this reaction, it seems like poor old Fe (iron) is the one who's getting oxidized. It's always tough being a metal in the world of chemical reactions. One minute you're all sturdy and solid, and the next minute, you're getting all oxidized and turning into Fe+3. Life's tough for metals, I tell ya!
To determine which element is oxidized in the given reaction, we need to assign oxidation numbers to the elements involved in the reaction.
In Fe2O3, we know that oxygen generally has an oxidation number of -2. Since Fe2O3 is a neutral compound, the sum of the oxidation numbers must be zero. Let's assume that the oxidation number of iron (Fe) is x. Since there are two Fe atoms, the total oxidation number for Fe2O3 is 2x. Setting up the equation:
2x + (-2*3) = 0
2x - 6 = 0
2x = 6
x = 3
So, iron (Fe) in Fe2O3 has an oxidation number of +3.
In CO2, oxygen has an oxidation number of -2. Let's assume the oxidation number of carbon (C) in CO2 is y. Since there is only one carbon atom, the total oxidation number for CO2 is y. Setting up the equation:
y + (-2*2) = 0
y - 4 = 0
y = 4
So, carbon (C) in CO2 has an oxidation number of +4.
Now, let's analyze the changes in oxidation numbers between the reactants and products in the reaction:
1. Fe2O3: Fe starts with an oxidation number of +3 and ends up as metallic Fe with an oxidation number of 0. The oxidation number decreases by 3, indicating a reduction.
2. CO: C starts with an oxidation number of 0 and ends up as part of CO2 with an oxidation number of +4. The oxidation number increases by 4, indicating an oxidation.
Therefore, in this reaction, carbon (C) is the element that is oxidized.