Question

According to the given equation, how many moles of iron are required to react with 0.85 moles oxygen? 4Fe+3O2⟶2Fe2O3 Your answer should have two significant figures.

Answer 1

Approximately 0.96 moles of iron (Fe) are required to react with 0.85 moles of oxygen (O2), based on the stoichiometric relationship from the balanced chemical equation 4Fe + 3O2 → 2Fe2O3.

Step-by-step explanation:

Stoichiometric Calculation of Moles of Iron

To determine how many moles of iron (Fe) are required to react with 0.85 moles of oxygen (O2), we use the balanced chemical equation 4Fe + 3O2 → 2Fe2O3. This equation tells us that 4 moles of Fe react with 3 moles of O2. We can set up a ratio to find the moles of Fe needed for 0.85 moles of O2:

(moles of Fe) / (moles of O2) = 4 / 3

Now, solve for moles of Fe:

moles of Fe = (4 moles Fe / 3 moles O2) × 0.85 moles O2

moles of Fe = (1.1333 moles Fe/moles O2) × 0.85 moles O2

moles of Fe = 0.96 moles of Fe (to two significant figures)

Therefore, it requires approximately 0.96 moles of iron to react with 0.85 moles of oxygen, based on the stoichiometric relationship from the balanced chemical equation.

Answer 2

To react with 0.85 moles of oxygen, 1.13 moles of iron are required according to the stoichiometric ratio derived from the balanced chemical equation: 4Fe + 3O2 → 2Fe2O3.

Step-by-step explanation:

• To determine the number of moles of iron required to react with 0.85 moles of oxygen, we start with the balanced chemical equation: 4Fe + 3O2 → 2Fe2O3.
• This equation indicates that 4 moles of iron react with 3 moles of oxygen, so we can set up a stoichiometric conversion to find the moles of iron needed for 0.85 moles of oxygen:

• (0.85 moles O2) × (4 moles Fe / 3 moles O2) = 1.13 moles Fe

Therefore, 1.13 moles of iron are required to react with 0.85 moles of oxygen, rounded to two significant figures.