How many moles of carbon are needed to react with 5.6 moles of hematite (Fe2O3)?
2Fe2O3 + 3C ==> 3CO2 + 4Fe
5.6 mols Fe2O3 x (3 mols C/2 mol Fe2O3) = 5.6 x 2/3 = ?
To determine the number of moles of carbon needed to react with hematite (Fe2O3), we need to use the balanced chemical equation for the reaction.
The balanced equation for the reaction between carbon and hematite is:
Fe2O3 + 3C → 2Fe + 3CO
From the equation, we can see that 3 moles of carbon are required to react with 1 mole of Fe2O3.
Given that we have 5.6 moles of Fe2O3, we can set up the following proportion:
3 moles C / 1 mole Fe2O3 = X moles C / 5.6 moles Fe2O3
To solve for X (the number of moles of carbon), we can cross-multiply and divide:
3 moles C × 5.6 moles Fe2O3 = 1 mole Fe2O3 × X moles C
16.8 moles C = X moles C
Therefore, 16.8 moles of carbon are needed to react with 5.6 moles of hematite (Fe2O3).
To determine the number of moles of carbon needed to react with 5.6 moles of hematite (Fe2O3), we need to first find the balanced chemical equation for the reaction between carbon and hematite.
The balanced chemical equation for the reaction can be represented as:
Fe2O3 + 3C → 2Fe + 3CO
From the balanced equation, we can observe that for every 1 mole of Fe2O3, 3 moles of carbon (C) are needed.
Given that we have 5.6 moles of Fe2O3, we can set up a proportion to find the number of moles of carbon required:
(5.6 moles Fe2O3 / 1) x (3 moles C / 1 mole Fe2O3) = 16.8 moles C
Therefore, 16.8 moles of carbon are needed to react with 5.6 moles of hematite (Fe2O3).