Iron (III) oxide reacts with solid carbon in the followed reaction: 2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g) What mass of Fe2O3 is n

Question

3 years ago

5

ecessary to produce 100. L of CO2 at 300. K and 2.10 atm?
823 g Fe2O3
908 g Fe2O3
1,110 g Fe2O3
1,360 g Fe2O3

2 answers:

Veseljchak [2.6K] · Answer 1 · 2022-09-10T15:19:15+03:00

953.6 g of iron (III) oxide (Fe₂O₃)

Explanation:

We have the following chemical reaction:

2 Fe₂O₃ (s) + 3 C (s) → 4 Fe (s) + 3 CO₂ (g)

We calculate the number of moles of CO₂ by using the following formula:

pressure × volume = number of moles × gas constant × temperature

number of moles = (pressure × volume) / (gas constant × temperature)

number of moles of CO₂ = (2.1 × 100) / (0.082 × 300)

number of moles of CO₂ = 8.54 moles

Taking in account the chemical reaction we devise the following reasoning:

if 2 mole of Fe₂O₃ produces 3 mole of CO₂

then X moles of Fe₂O₃ produces 8.54 mole of CO₂

X = (2 × 8.54) / 3 = 5.69 moles of Fe₂O₃

number of moles = mass / molar weight

mass = number of moles × molar weight

mass of Fe₂O₃ = 5.69 × 160 = 953.6 g

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Dahasolnce [82] · Answer 2 · 2022-09-10T17:04:18+03:00

4 0

The answer is B. 908 g Fe2O3