Calculate mass of iron, which will be converted into (Fe3O4) by the action of 18g of steam on it.
First we write the balanced chemical reaction involved:
3Fe + 4H2O -> Fe3O4 + 4H2
Since we have 18 g of steam, we have to convert this to moles and use the stoich ratios from the reaction to get amount of Fe needed to react with it. To convert mass to moles, we get the molecular weight (MW) of the substance (just get a periodic table and add the individual weights of elements in the chemical formula). Thus,
MW of H2O = 2*1 + 16 = 18 g/mol
MW of Fe = 55.85 g/mol
From the reaction, we can see that for every 4 moles of H2O reacted, 3 moles of Fe are also consumed. Therefore,
18 g * (1 mol H2O / 18 g) * (3 mol Fe / 4 mol H2O) * (55.85 g / mol Fe)
= 41.89 g Fe
Hope this helps~ :3
First we write the balanced chemical reaction involved:
3Fe + 4H2O -> Fe3O4 + 4H2
Since we have 18 g of steam, we have to convert this to moles and use the stoich ratios from the reaction to get amount of Fe needed to react with it. To convert mass to moles, we get the molecular weight (MW) of the substance (just get a periodic table and add the individual weights of elements in the chemical formula). Thus,
MW of H2O = 2*1 + 16 = 18 g/mol
MW of Fe = 55.85 g/mol
From the reaction, we can see that for every 4 moles of H2O reacted, 3 moles of Fe are also consumed. Therefore,
18 g * (1 mol H2O / 18 g) * (3 mol Fe / 4 mol H2O) * (55.85 g / mol Fe)
= 41.89 g Fe
To calculate the mass of iron required to be converted into Fe3O4 by the action of 18g of steam, we need to determine the molar ratios between iron, water, and Fe3O4.
First, we need to write a balanced chemical equation for the reaction:
3Fe(s) + 4H2O(g) -> Fe3O4(s) + 4H2(g)
From the equation, we can see that 3 moles of iron react with 4 moles of water to produce 1 mole of Fe3O4.
Now, we need to determine the molar mass of water (H2O) and Fe3O4. The molar mass of hydrogen (H) is 1 g/mol, the molar mass of oxygen (O) is 16 g/mol, and the molar mass of iron (Fe) is 56 g/mol.
The molar mass of water (H2O) = (2H × 1 g/mol) + (1O × 16 g/mol) = 18 g/mol
The molar mass of Fe3O4 = (3Fe × 56 g/mol) + (4O × 16 g/mol) = 232 g/mol
Now, we can calculate the moles of water (H2O) present:
Moles of H2O = Mass of H2O / Molar mass of H2O
Moles of H2O = 18 g / 18 g/mol = 1 mol
Based on the balanced equation, we know that 4 moles of water react with 1 mole of Fe3O4. Therefore, the moles of Fe3O4 formed is also 1 mol.
Finally, we can calculate the mass of iron required:
Mass of iron = Moles of Fe3O4 × Molar mass of Fe3O4
Mass of iron = 1 mol × 232 g/mol = 232 g
Therefore, the mass of iron required to be converted into Fe3O4 by the action of 18g of steam is 232 grams.
Write and balance the equation.
Convert 18 g steam to mols. mols = grams/molar mass
Using the coefficients in the balanced equation, convert mols H2O to mols Fe.
Now convert mols Fe to grams Fe. g = mols Fe x atomic mass Fe.