In the reaction Fe2O3 + 3CO �¨ 2Fe + 3CO2
How much CO is used to produce 112 grams of iron?
To determine how much CO is used to produce 112 grams of iron, we need to use stoichiometry, which relates the amounts of reactants and products in a chemical reaction.
First, we need to balance the chemical equation:
Fe2O3 + 3CO -> 2Fe + 3CO2
This equation tells us that for every one mole of Fe2O3, we need three moles of CO to produce two moles of Fe.
Now, we can set up a proportion to solve for the amount of CO needed:
(3 moles CO / 2 moles Fe) = (x moles CO / 112 grams Fe)
To solve for x, we can use the molar mass of iron (Fe), which is 55.85 g/mol.
112 grams Fe * (1 mole Fe / 55.85 grams Fe) = 2 moles Fe
Using the proportion, we can now solve for x:
(3 moles CO / 2 moles Fe) = (x moles CO / 2 moles Fe)
3/2 = x/2
Cross-multiplying, we find:
3 * 2 = 2x
6 = 2x
Dividing both sides by 2, we find:
x = 3 moles CO
Therefore, 3 moles of CO is used to produce 112 grams of iron.