In the reaction 4Fe + 3O2 → 2Fe2O3, how many grams of Fe2O3 can be produced from

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Question: In the reaction 4Fe + 3O2 → 2Fe2O3, how many grams of Fe2O3 can be produced from 8 grams of Fe?

Options:

Correct Answer: 48 g

Solution:

8 g of Fe = 0.143 moles. 4 moles of Fe produce 2 moles of Fe2O3, so 0.0715 moles of Fe2O3 = 0.0715 * 160 g = 11.44 g.

In the reaction 4Fe + 3O2 → 2Fe2O3, how many grams of Fe2O3 can be produced from 8 grams of Fe?

In the reaction 4Fe + 3O2 → 2Fe2O3, how many grams of Fe2O3 can be produced from 8 grams of Fe?

Step 1: Calculate the number of moles of Fe in 8 grams. Use the formula: moles = mass (g) / molar mass (g/mol). The molar mass of Fe is approximately 55.85 g/mol.
Step 2: Calculate the moles of Fe: 8 g / 55.85 g/mol = 0.143 moles of Fe.
Step 3: Use the balanced chemical equation 4Fe + 3O2 → 2Fe2O3 to find the mole ratio. From the equation, 4 moles of Fe produce 2 moles of Fe2O3.
Step 4: Determine how many moles of Fe2O3 can be produced from 0.143 moles of Fe. Set up the ratio: (2 moles Fe2O3 / 4 moles Fe) * 0.143 moles Fe = 0.0715 moles of Fe2O3.
Step 5: Calculate the mass of Fe2O3 produced. The molar mass of Fe2O3 is approximately 159.69 g/mol. Use the formula: mass = moles * molar mass.
Step 6: Calculate the mass of Fe2O3: 0.0715 moles * 159.69 g/mol = 11.44 grams of Fe2O3.

Stoichiometry – The calculation of reactants and products in chemical reactions based on balanced equations.
Mole Conversion – Converting grams to moles using molar mass and vice versa.
Balanced Chemical Equations – Understanding the ratios of reactants and products in a balanced chemical reaction.