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| Metal Alloys | 7 mins | 0 completed | Learn |
| Polyatomic Ions | 15 mins | 0 completed | Learn Summary |
| Naming Covalent Compounds | 6 mins | 0 completed | Learn |
| Naming Ionic Compounds | 36 mins | 0 completed | Learn |
| Naming Acids | 14 mins | 0 completed | Learn |
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| Balancing Chemical Equations | 8 mins | 0 completed | Learn |
| Functional Groups in Chemistry | 13 mins | 0 completed | Learn |
| Stoichiometry | 61 mins | 0 completed | Learn Summary |
| Additional Practice |
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| Ionic and Covalent Bonds |
| Molecular Models |
| Limiting Reagent |
| Percent Yield |
| Additional Guides |
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| Molecular Formula |
| Balancing Chemical Equations Worksheet |
| Theoretical Yield |
| Limiting Reactant |
In the reaction of 1.00 mole of O2 with 2.00 mole of H2, 2H2 + O2→ 2H2O
If 30.0g of H2O is formed, what is the percent yield?
a) 100%
b) 88.9%
c) 50.0%
d) 167%
e) 83.3%
We’re being asked to calculate the percent yield of H2O. The balanced chemical equation is:
2 H2 + O2 → 2 H2O
Recall that percent yield is given by:
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