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)
2242
views
5
rank
8. Quantities in Chemical Reactions
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
Identify the stoichiometry of the reaction: Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g). This tells us that 1 mole of Fe2O3 produces 2 moles of Fe.
Determine the moles of Fe that would be produced if the reaction went to 100% completion. Since the reaction only goes to 75% completion, calculate the moles of Fe that would be produced at full completion by dividing the given moles of Fe (0.850 moles) by 0.75.
Use the stoichiometry of the reaction to find the moles of Fe2O3 required for the full completion moles of Fe. Since 1 mole of Fe2O3 produces 2 moles of Fe, divide the moles of Fe (from step 2) by 2 to find the moles of Fe2O3 needed.
Consider the options provided and compare the calculated moles of Fe2O3 to the options to find the closest match.
Verify the calculation by checking the stoichiometry and the percentage completion to ensure the correct understanding of the problem.
Related Videos
Related Practice
