Multiple Choice
What is the percent yield for a reaction in which 22.1 g Cu is isolated by reacting 45.5 g Zn with 70.1 g CuSO4?
Zn (s) + CuSO4 (aq) → Cu (s) + ZnSO4 (aq)
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6. Chemical Reactions & Quantities
Percent Yield
Multiple Choice
The reduction of iron (III) oxide creates the following reaction:
Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g)
If the above reaction only went to 75% completion, how many moles of Fe2O3 were require to produce 0.850 moles of Fe?
A
0.963 mol
B
2.27 mol
C
0.425 mol
D
0.567 mol
E
1.70 mol
Verified step by step guidance1
Understand the stoichiometry of the reaction: Fe2O3 reacts with H2 to produce Fe and H2O. The balanced equation is Fe2O3 + 3 H2 → 2 Fe + 3 H2O.
Identify the mole ratio between Fe2O3 and Fe from the balanced equation. For every 1 mole of Fe2O3, 2 moles of Fe are produced.
Since the reaction goes to 75% completion, calculate the effective moles of Fe produced. Multiply the given moles of Fe (0.850 moles) by 100/75 to find the moles of Fe that would be produced if the reaction went to full completion.
Use the mole ratio to find the moles of Fe2O3 required for the full completion moles of Fe. Divide the moles of Fe (from step 3) by 2 (from the stoichiometry) to find the moles of Fe2O3 needed.
Consider the options provided and identify the correct number of moles of Fe2O3 that matches your calculation from step 4.
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