Fe3O4 reacts with CO according to the equation
Fe3O4 + 4CO => 4CO2 + 3Fe
If 478.9 g Fe3O4 is reacted with excess CO, what mass of CO2 will be produced?
mols Fe3O4 = grams/molar mass
Convert mols Fe3O4 to mols CO2.
g CO2 = mols x molar mass
799
Well, it's time for some chemical comedy! Let's calculate the mass of CO2, but I promise I won't react too much.
First, we need to find the molar mass of Fe3O4. Fe has a molar mass of approximately 55.85 g/mol, and O has a molar mass of approximately 16 g/mol.
So, the molar mass of Fe3O4 would be:
(3 x 55.85 g/mol) + (4 x 16 g/mol) = 231.65 g/mol
Now, let's calculate the number of moles of Fe3O4 by dividing the given mass by the molar mass:
478.9 g / 231.65 g/mol = 2.07 mol
According to the balanced equation, the ratio of Fe3O4 to CO2 is 1:4. This means that 1 mol of Fe3O4 will produce 4 mol of CO2.
So, if we have 2.07 mol of Fe3O4, we can expect to produce:
2.07 mol x 4 mol CO2/mol Fe3O4 = 8.28 mol CO2
Finally, let's find the mass of CO2 by multiplying the number of moles by the molar mass of CO2. The molar mass of CO2 is approximately 44 g/mol.
8.28 mol x 44 g/mol = 364.32 g
Therefore, the mass of CO2 produced when 478.9 g Fe3O4 reacts with excess CO is approximately 364.32 g. Hope these calculations didn't make you "Fe"3"O"4 it!
To determine the mass of CO2 produced, we need to use the molar masses of Fe3O4 and CO2, as well as the stoichiometry of the reaction.
1. Calculate the molar mass of Fe3O4:
Fe = 55.845 g/mol
O = 16.00 g/mol
Molar mass of Fe3O4 = (3 * Fe) + (4 * O) = (3 * 55.845) + (4 * 16.00) = 231.675 g/mol
2. Determine the molar mass of CO2:
C = 12.01 g/mol
O = 16.00 g/mol
Molar mass of CO2 = (1 * C) + (2 * O) = 12.01 + (2 * 16.00) = 44.01 g/mol
3. Calculate the number of moles of Fe3O4:
moles of Fe3O4 = mass of Fe3O4 / molar mass of Fe3O4
= 478.9 g / 231.675 g/mol
= 2.07 mol
4. Use the stoichiometry of the balanced equation to determine the number of moles of CO2 produced:
From the balanced equation, we know that the molar ratio of Fe3O4 to CO2 is 1:4.
moles of CO2 = moles of Fe3O4 * (4 moles of CO2 / 1 mole of Fe3O4)
= 2.07 mol * (4 mol / 1 mol)
= 8.28 mol
5. Calculate the mass of CO2 produced:
mass of CO2 = moles of CO2 * molar mass of CO2
= 8.28 mol * 44.01 g/mol
= 364.04 g
Therefore, 478.9 g of Fe3O4 reacted with excess CO will produce 364.04 g of CO2.
To find the mass of CO2 produced, we need to use the stoichiometry of the balanced equation to convert mass of Fe3O4 to mass of CO2.
The molar mass of Fe3O4 is calculated as follows:
Fe: (55.845 g/mol) x 3 = 167.535 g/mol
O: (15.999 g/mol) x 4 = 63.996 g/mol
Total: 167.535 g/mol + 63.996 g/mol = 231.531 g/mol
Now let's calculate the number of moles of Fe3O4:
478.9 g / 231.531 g/mol = 2.0694 mol
According to the balanced equation, 1 mol of Fe3O4 reacts to produce 4 mol of CO2. Therefore, we can determine the number of moles of CO2 produced using the ratio of coefficients:
2.0694 mol Fe3O4 x (4 mol CO2 / 1 mol Fe3O4) = 8.2776 mol CO2
Finally, let's convert the moles of CO2 to mass using its molar mass:
8.2776 mol x 44.01 g/mol = 364.14 g
Therefore, 364.14 g of CO2 will be produced when 478.9 g of Fe3O4 reacts with excess CO.