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1. How many liters of CO2 are produced when 3.46 Fe2O3 is converted to cast Fe at STP?

Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)


a. 3.45 L

b. 1.45 L

c. 2.45 L

d. 4.45 L

Sagot :

SOLUTION:

Based on the balanced equation, 1 mole of Fe₂O₃ is stoichiometrically equivalent to 3 moles of CO₂.

The volume of 1 mole of any gas at STP is 22.4 L.

The molar mass of Fe₂O₃ is 160 g/mol.

[tex]\begin{aligned} \text{volume of} \: \text{CO}_2 & = \text{3.46 g} \: \text{Fe}_2\text{O}_3 \times \frac{\text{1 mol} \: \text{Fe}_2\text{O}_3}{\text{160 g} \: \text{Fe}_2\text{O}_3} \times \frac{\text{3 mol} \: \text{CO}_2}{\text{1 mol} \: \text{Fe}_2\text{O}_3} \times \frac{\text{22.4 L}}{\text{1 mol} \: \text{CO}_2} \\ & = \boxed{\text{1.45 L}} \end{aligned}[/tex]

Hence, the answer is b. 1.45 L.

[tex]\\[/tex]

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