How many grams of C are required to react with 43.8 g of Fez O3?
In order to determine the number of grams of C required to react with 43.8 g of Fe2O3, we need to write and balance the equation for the reaction.
The balanced equation for the reaction between C (carbon) and Fe2O3 (iron(III) oxide) is:
C + Fe2O3 -> CO2 + 2Fe
From the balanced equation, we can see that 1 mole of C reacts with 1 mole of Fe2O3 to produce 1 mole of CO2 and 2 moles of Fe.
Step 1: Calculate the molar mass of Fe2O3.
Fe2O3 = (2 * atomic mass of Fe) + (3 * atomic mass of O)
Fe2O3 = (2 * 55.845 g/mol) + (3 * 16.00 g/mol)
Fe2O3 = 111.69 g/mol + 48.00 g/mol
Fe2O3 = 159.69 g/mol
Step 2: Convert the mass of Fe2O3 to moles.
moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
moles of Fe2O3 = 43.8 g / 159.69 g/mol
moles of Fe2O3 = 0.274 moles
Step 3: Determine the number of moles of C required.
From the balanced equation, we know that 1 mole of C reacts with 1 mole of Fe2O3. Therefore, the number of moles of C required is also 0.274 moles.
Step 4: Convert moles of C to grams.
mass of C = moles of C * molar mass of C
mass of C = 0.274 moles * 12.01 g/mol
mass of C = 3.29 grams (rounded to two decimal places)
Therefore, approximately 3.29 grams of C are required to react with 43.8 g of Fe2O3.
To determine the number of grams of C required to react with 43.8 g of Fe2O3, we need to first balance the chemical equation for the reaction between carbon (C) and Fe2O3.
The balanced chemical equation is as follows:
3C + Fe2O3 → 2Fe + 3CO2
From the balanced equation, we can see that 3 moles of carbon (C) react with 1 mole of Fe2O3. In order to find the number of grams, we need to convert the grams of Fe2O3 to moles and then use the mole ratio from the balanced equation.
The molar mass of Fe2O3 (Iron(III) oxide) is:
2(55.85 g/mol) + 3(16.00 g/mol) = 159.69 g/mol
Moles of Fe2O3 = grams of Fe2O3 / molar mass of Fe2O3
Moles of Fe2O3 = 43.8 g / 159.69 g/mol ≈ 0.2747 mol
Using the mole ratio from the balanced equation, we can determine the moles of C required:
3 moles of C / 1 mole of Fe2O3 * 0.2747 mol of Fe2O3 ≈ 0.8241 mol of C
Finally, we can convert the moles of C to grams:
Grams of C = moles of C * molar mass of C
Grams of C = 0.8241 mol * 12.01 g/mol ≈ 9.89 g
Therefore, approximately 9.89 grams of C are required to react with 43.8 g of Fe2O3.
To determine the number of grams of carbon (C) required to react with 43.8 g of Fe2O3, we need to calculate the stoichiometry of the reaction. The balanced chemical equation represents the stoichiometry of the reaction, showing the molar ratios between reactants and products.
The balanced chemical equation for the reaction between carbon and Fe2O3 is:
3C + Fe2O3 -> 2Fe + 3CO2.
From the balanced equation, we can see that for every 3 moles of carbon (C), we need 1 mole of Fe2O3 in order to fully react.
Now we need to convert the mass of Fe2O3 to moles. To do this, we need to know the molar mass of Fe2O3. Using the atomic masses from the periodic table, we can find:
Molar mass of Fe2O3 = (2 x atomic mass of Fe) + (3 x atomic mass of O)
= (2 x 55.845 g/mol) + (3 x 16.00 g/mol)
= 159.69 g/mol.
Now we can calculate the moles of Fe2O3:
moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
= 43.8 g / 159.69 g/mol
≈ 0.274 mol.
According to the balanced equation, for every 1 mole of Fe2O3, we need 3 moles of carbon (C). Therefore, we need:
moles of C = 3 x moles of Fe2O3
= 3 x 0.274 mol
= 0.822 mol.
Finally, we can convert moles of C to grams using the molar mass of carbon (C), which is 12.01 g/mol.
grams of C = moles of C x molar mass of C
= 0.822 mol x 12.01 g/mol
≈ 9.87 g.
Therefore, approximately 9.87 grams of carbon (C) are required to react with 43.8 grams of Fe2O3.