Hematite,Fe2O3 is heated in furnace with carbon monoxide,CO qnd the products obtaines ,iron, Fe and Carbon dioxide ,CO2
1 )question is balanced the equation
2)if mass of hematite used is 8.00×10^4 g ,calculate mass of iron obtained.
Fe2O3 + 3 CO --> 2 Fe + 3 CO2
2 Fe ... 2 * 55.85 = 111.7
3 O ... 3 * 16.00 = 48.00
Fe yield ... 8.00E4 * [111.7 / (111.7 + 48.00)]
To balance the equation, we need to ensure that the number of atoms on both sides of the equation are equal.
1) Balancing the equation:
The unbalanced chemical equation is:
Fe2O3 + CO → Fe + CO2
Let's balance the equation step by step:
Step 1: Balance the number of atoms of each element except oxygen and hydrogen:
2 Fe2O3 + CO → Fe + CO2
Step 2: Balance oxygen by adding coefficient 2 in front of CO:
2 Fe2O3 + CO → Fe + 2 CO2
Step 3: Balance the number of atoms of each element except oxygen:
2 Fe2O3 + 3 CO → 4 Fe + 2 CO2
The balanced equation is:
2 Fe2O3 + 3 CO → 4 Fe + 2 CO2
2) Calculating the mass of iron obtained:
To calculate the mass of iron obtained, we need to use the concept of stoichiometry.
From the balanced equation:
2 mol Fe2O3 reacts to form 4 mol Fe
Molar mass of Fe2O3 = (2 × atomic mass of Fe) + (3 × atomic mass of O)
= (2 × 55.845 g/mol) + (3 × 16.00 g/mol)
= 111.69 g/mol + 48.00 g/mol
= 159.69 g/mol
Molar mass of Fe = 55.845 g/mol
Now, calculate the number of moles of Fe2O3:
Number of moles = Mass / Molar mass
= 8.00 × 10^4 g / 159.69 g/mol
≈ 500.41 mol
Using the stoichiometry from the balanced equation:
2 mol Fe2O3 ↔ 4 mol Fe
Therefore,
500.41 mol Fe2O3 ↔ (4 / 2) × 500.41 mol Fe
= 1000.82 mol Fe
Now, calculate the mass of iron obtained:
Mass = Number of moles × Molar mass
≈ 1000.82 mol × 55.845 g/mol
≈ 55,846.05 g
Therefore, the mass of iron obtained from 8.00 × 10^4 g of hematite is approximately 55,846.05 g.