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# Stoichiometry and Chemical Equations Study Guide (page 3)

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#### Example:

Identify the limiting reactant and how much ammonia gas can be produced when 8.0 g of nitrogen gas reacts with 8.0 g of hydrogen gas by the use of the Haber process: 3H2 + N2→ 2NH3.

#### Solution:

 1. Identify the amount given and needed: 3H2 + N2 → 2NH3 8.0 g + 8.0 g → ? 2. Use the molar masses and mole ratios (coeffi-cients) to set up the calculation: 3. The limiting reactant is nitrogen because it can produce the smallest amount of ammonia. The theoretical yield of ammonia is 9.7 g.

## Percent Yield

The percentage yield is a ratio of the actual yield of a product over the expected one, known as the theoretical yield.

#### Example:

From the previous example, what is the percent yield if only 8.2 g of ammonia is produced?

#### Solution:

Practice problems for these concepts can be found at -  Stoichiometry and Chemical Equations Practice Questions

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