I.) Steel wool, which is made of pure iron metal, burns with oxygen gas to produce ferric oxide (Fe2O3). 4 Fe + 3 O2 → 2 Fe2O3 If there are 1.25 moles of Fe and 1.25 moles of O2, how many moles of Fe2O3 will be produced? What is its mass? If the actual laboratory yield is 95.8 g Fe2O3, what is the reaction’s percent yield?
I.) Steel wool, which is made of pure iron metal, burns with oxygen gas to produce ferric oxide (Fe2O3).
4 Fe + 3 O2 → 2 Fe2O3
If there are 1.25 moles of Fe and 1.25 moles of O2,
- how many moles of Fe2O3 will be produced? What is its mass?
- If the actual laboratory yield is 95.8 g Fe2O3, what is the reaction’s percent yield?
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II.) Pure aluminum (Al) metal reacts with hydrochloric acid (HCl) to produce aluminum chloride (AlCl3) and hydrogen (H2) gas.
2 Al + 6 HCl → 2 AlCl3 + 3 H2
- If the expected mass of AlCl3 to be formed is 3.5 g, what should be the initial mass of the pure aluminum metal?
- If the actual mass of AlCl3 produced is 3.1 g, what is the percentage yield of the reaction?
III.) Your company manufactures nylon from adipic acid (H2C6H8O4). Adipic acid is produced from the reaction between liquid cyclohexane (C6H12) and oxygen gas. Another product of this combination is water as shown in the chemical equation below: (20 points)
2 C6H12 + 5 O2 = 2 H2C6H8O4 + 2 H2O
If your target percent yield is at least 85% of the 25.0 g theoretical yield, how much of the starting materials (cyclohexane and oxygen gas) should you have? Express both reactants in (a) moles and (b) grams.
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