What mass of CO is required to react with 146 g of iron (|||) oxide?
1. Write and balanced the equation.
2. Convert mass Fe to mols. mols = grams/molar mass = ?
3. Using the Coefficients in the balanced equation, convert mols Fe to mols CO.
4. Now convert mols CO to g. g = mols x molar mass.
Print this page. This four step procedure will work almost all of your stoichiometry problems.
To determine the mass of CO required to react with 146 g of iron (III) oxide (Fe2O3), you need to balance the chemical equation for the reaction between CO and Fe2O3, and then use stoichiometry to calculate the mass.
The balanced chemical equation for the reaction is as follows:
3CO + Fe2O3 → 3CO2 + 2Fe
From the balanced equation, you can see that the molar ratio between CO and Fe2O3 is 3:1. This means that for every 3 moles of CO, 1 mole of Fe2O3 is required.
To calculate the mass of CO, you need to convert the given mass of Fe2O3 into moles first. The molar mass of Fe2O3 is calculated as follows:
2(55.85 g/mol) + 3(16.00 g/mol) = 159.69 g/mol
Using this molar mass, you can convert 146 g of Fe2O3 into moles:
146 g Fe2O3 × (1 mol Fe2O3 / 159.69 g Fe2O3) = 0.914 mol Fe2O3
Since the molar ratio between CO and Fe2O3 is 3:1, you can set up a proportion to determine the number of moles of CO required:
3 mol CO / 1 mol Fe2O3 = x mol CO / 0.914 mol Fe2O3
Cross-multiplying, you get:
3 mol CO × 0.914 mol Fe2O3 = x mol CO × 1 mol Fe2O3
2.742 mol CO = x mol CO
Therefore, 2.742 mol of CO is required to react with 146 g of Fe2O3.
To determine the mass of CO, use its molar mass, which is 28.01 g/mol:
2.742 mol CO × 28.01 g/mol ≈ 76.75 g CO
Therefore, approximately 76.75 grams of CO is required to react with 146 g of Fe2O3.
To determine the mass of CO required to react with iron (III) oxide (Fe2O3), we need to balance the chemical equation for the reaction.
The balanced equation for the reaction between CO and Fe2O3 is:
3CO + Fe2O3 -> 3CO2 + 2Fe
From the balanced equation, we can see that 3 moles of CO react with 1 mole of Fe2O3 to produce 3 moles of CO2 and 2 moles of Fe.
To calculate the mass of CO required, we need to follow these steps:
Step 1: Calculate the molar mass of Fe2O3
The molar mass of Fe2O3 (iron (III) oxide) is calculated by summing up the atomic masses of its constituent elements:
Molar mass of Fe2O3 = (2 x molar mass of Fe) + (3 x molar mass of O)
From the periodic table, the molar masses are:
Molar mass of Fe = 55.845 g/mol
Molar mass of O = 16.00 g/mol
Substitute these values into the equation:
Molar mass of Fe2O3 = (2 x 55.845 g/mol) + (3 x 16.00 g/mol)
Molar mass of Fe2O3 = 159.69 g/mol
Step 2: Convert the given mass of Fe2O3 to moles
To convert the mass of Fe2O3 to moles, divide the given mass by its molar mass:
Moles of Fe2O3 = Mass / Molar mass
Moles of Fe2O3 = 146 g / 159.69 g/mol
Step 3: Determine the moles of CO required
From the balanced equation, we know that the ratio of CO to Fe2O3 is 3:1. Therefore, the moles of CO required will be three times the moles of Fe2O3:
Moles of CO = 3 x Moles of Fe2O3
Step 4: Calculate the mass of CO required
To calculate the mass of CO required, multiply the moles of CO by its molar mass:
Mass of CO = Moles of CO x Molar mass of CO
Since we haven't been given the molar mass of CO, let's calculate it quickly.
CO is made up of carbon (C) and oxygen (O) atoms. From the periodic table:
Molar mass of C = 12.01 g/mol
Molar mass of O = 16.00 g/mol
Therefore, the molar mass of CO is:
Molar mass of CO = Molar mass of C + Molar mass of O
Molar mass of CO = 12.01 g/mol + 16.00 g/mol
Molar mass of CO = 28.01 g/mol
Now, substitute the values into our equation:
Mass of CO = Moles of CO x Molar mass of CO
Finally, calculate the mass of CO required.