| Sections | |||
|---|---|---|---|
| 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 |
| Empirical Formula | 14 mins | 0 completed | Learn Summary |
| Combustion Analysis | 13 mins | 0 completed | Learn |
| Mass Percent Formula | 17 mins | 0 completed | Learn Summary |
| 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 |
|---|
| Ionic and Covalent Bonds |
| Molecular Models |
| Limiting Reagent |
| Percent Yield |
| Additional Guides |
|---|
| Molecular Formula |
| Balancing Chemical Equations Worksheet |
| Theoretical Yield |
| Limiting Reactant |
Ammonia can be prepared by the Haber process, shown in this equation.
N2 + 3 H2 ⇌ 2 NH3
If 2 mol of N2 and 3 mol of H2 are combined, the amount of NH 3 that would be formed if all of the limiting reactant were used up is known as the
a) limited yield.
b) percent yield.
c) product yield.
d) theoretical yield.
Enter your friends' email addresses to invite them:
Join thousands of students and gain free access to 46 hours of Chemistry videos that follow the topics your textbook covers.