4FeCr2O7 + 8K2C03 + O2 --> 2Fe2O3 + 8K2CrO4 + 8CO2

a). How many grams of FeCr2O7 are required to produce 44.0 g of CO2

To determine how many grams of FeCr2O7 are required to produce 44.0 g of CO2, we need to use stoichiometry, which involves the mole-to-mole ratios from the balanced chemical equation.

1. Write down the balanced chemical equation:
4FeCr2O7 + 8K2C03 + O2 -> 2Fe2O3 + 8K2CrO4 + 8CO2

2. Identify the mole-to-mole ratio from the balanced chemical equation:
From the equation, we see that for every 8 moles of CO2 produced, we need 4 moles of FeCr2O7.

3. Convert grams of CO2 to moles of CO2:
We can convert the given mass of CO2 (44.0 g) to moles by dividing by the molar mass of CO2, which is approximately 44.01 g/mol. Thus:
44.0 g CO2 / (44.01 g/mol CO2) = 1.000 mol CO2

4. Use the mole-to-mole ratio to find moles of FeCr2O7:
Using the mole-to-mole ratio from the balanced equation, we know that for every 8 moles of CO2 produced, we need 4 moles of FeCr2O7. Therefore:
1.000 mol CO2 x (4 mol FeCr2O7 / 8 mol CO2) = 0.500 mol FeCr2O7

5. Convert moles of FeCr2O7 to grams of FeCr2O7:
To find the mass of FeCr2O7 that corresponds to 0.500 moles, we need to multiply by the molar mass of FeCr2O7. The molar mass of FeCr2O7 is approximately 447.67 g/mol. Thus:
0.500 mol FeCr2O7 x (447.67 g/mol FeCr2O7) = 223.84 g FeCr2O7

Therefore, approximately 223.84 grams of FeCr2O7 are required to produce 44.0 grams of CO2.

To determine the number of grams of FeCr2O7 required to produce 44.0 g of CO2, we can follow these steps:

Step 1: Identify the molar masses of FeCr2O7 and CO2.
The molar mass of FeCr2O7 = (1 atom of Fe * molar mass of Fe) + (2 atoms of Cr * molar mass of Cr) + (7 atoms of O * molar mass of O)
The molar mass of CO2 = (1 atom of C * molar mass of C) + (2 atoms of O * molar mass of O)

Step 2: Calculate the molar mass of FeCr2O7 and CO2.
Using the periodic table, we find the molar masses:
Molar mass of FeCr2O7 = (1 * 55.845 g/mol) + (2 * 51.9961 g/mol) + (7 * 15.9994 g/mol) = 292.2386 g/mol
Molar mass of CO2 = (1 * 12.0107 g/mol) + (2 * 15.9994 g/mol) = 44.0098 g/mol

Step 3: Determine the molar ratio between FeCr2O7 and CO2.
Looking at the balanced chemical equation:
4FeCr2O7 + 8K2C03 + O2 → 2Fe2O3 + 8K2CrO4 + 8CO2
We can see that the molar ratio between FeCr2O7 and CO2 is 4:8 or 1:2.

Step 4: Calculate the number of moles of CO2.
Number of moles = given mass / molar mass
Number of moles of CO2 = 44.0 g / 44.0098 g/mol = 1.0000 mol

Step 5: Determine the number of moles of FeCr2O7.
Since the molar ratio between FeCr2O7 and CO2 is 1:2, the number of moles of FeCr2O7 is half the number of moles of CO2:
Number of moles of FeCr2O7 = 1.0000 mol / 2 = 0.5000 mol

Step 6: Calculate the mass of FeCr2O7 required.
Mass = number of moles * molar mass
Mass of FeCr2O7 = 0.5000 mol * 292.2386 g/mol = 146.1193 g

Therefore, approximately 146.1193 grams of FeCr2O7 are required to produce 44.0 g of CO2.

1. You have the balanced equation.

2. Convert 44.0 g CO2 to moles. moles = grams/molar mass.
3. Using the coefficients in the balanced equation, convert moles CO2 to moles FeCr2O7.
4. Now convert moles FeCr2O7 to grams. g = mols x molar mass.