Chemistry Stoichiometry and Reactions

Study Notes

Iron Reduction from Fe2O3

The reduction reaction for iron oxide can be represented as:
Fe2O3 + 3H2 → 2Fe + 3H2O*
Stoichiometry: For every 1 mole of Fe2O3, 2 moles of Fe are produced.
Molecular Weight of Fe2O3: Approximately 159.69 g/mol.
Iron Production:
- From 1 kg (1000 g) of Fe2O3, calculate moles:
  Moles of Fe2O3 = 1000 g / 159.69 g/mol ≈ 6.26 moles
- Each mole of Fe2O3 produces 2 moles of Fe:
  Total moles of Fe = 6.26 moles × 2 ≈ 12.52 moles
- Convert moles of Fe to grams using atomic weight of Fe (approximately 55.85 g/mol):
  Mass of Fe = 12.52 moles × 55.85 g/mol ≈ 700.24 g

Combustion of Methane (CH4)

Reaction equations for combustion:
- First equation:
CH4 + 2O2 → CO2 + 3H2O*
- Second equation (alternative stoichiometry):
2CH4 + 7O2 → 4CO2 + 6H2O*
Given data: 40 g of CH4.
Calculate the molar quantity from 40 g:
Moles of CH4 = 40 g / 16.04 g/mol (molar mass of CH4) ≈ 2.49 moles.
Using the first equation for stoichiometry, each mole of CH4 produces 1 mole of CO2:
Total moles of CO2 from 2.49 moles of CH4 = 2.49 moles.
Convert the moles of CO2 to grams using the molecular weight of CO2 (approximately 44.01 g/mol):
Mass of CO2 = 2.49 moles × 44.01 g/mol ≈ 109.56 g.
The number y is calculated based on an interpretation of combustion yields:
y* = 14.6 × 8 = 116.8 g can reference another context related to yield or multiples.

Description

This quiz covers stoichiometric calculations related to the reduction of iron from iron(III) oxide (Fe2O3) and the combustion of methane (CH4). Participants will balance chemical equations, analyze given data, and solve for unknown quantities. Test your knowledge of chemical reactions and stoichiometry.