**Percent Yield of Carbon Dioxide** **Purpose:** To predict the amount of carbon dioxide gas that should be produced in a chemical reaction. Then, calculate the amount of carbon dioxide actually produced and determine the percent yield. The reaction is represented in the equation below: \[ \text{CH}_3\text{COOH} + \text{NaHCO}_3 \rightarrow \text{NaCH}_3\text{COO} + \text{H}_2\text{O} + \text{CO}_2 \] **Materials:** - Sodium bicarbonate (aka baking soda) - Acetic acid solution (aka vinegar) - Erlenmeyer flasks - Balance **Procedure:** 1. Measure and record the mass of a 250-mL Erlenmeyer flask. Label it as flask A. 2. Add approximately 7.5 g of sodium bicarbonate to flask A. 3. Measure and record the mass of a second 250-mL Erlenmeyer flask. Call it flask B. 4. Add approximately 75 g of acetic acid solution to flask B. 5. Slowly add acetic acid to flask A until the reaction has stopped. Do not add all of the vinegar; just enough to complete the reaction. 6. After the reaction has stopped, measure and record the masses of both flasks. **Calculation for Percent Yield:** \[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \] \[ \text{Percent Yield of CO}_2 = \left( \frac{\text{(Actual Yield - Theoretical Yield)}}{\text{Theoretical Yield}} \right) \times 100 \] **Data Table:** | # | Description | Data | Units | |----|-----------------------------------------|--------|-------| | 1 | Mass of Beaker A (empty) | 76.86 | g | | 2 | Mass of Beaker A + Baking Soda | 83.52 | g | | 3 | Mass of Baking Soda (2-1) | 6.96 | g | | 4 | Mass of Beaker B (empty) | 31.62 | g | | 5 | Mass of Beaker B Name: Period: **Discussion Questions:** 1. **What are the reactants in this experiment?** NaHCO₃ 2. **Which are the products in this experiment?** 3. **Identify the limiting reactant!** 4. **Identify the excess reactant!** NaHCO₃ CH₃COOH 5. **Using stoichiometry (i.e., mass of Baking Soda) calculate the theoretical yield of carbon dioxide:** 3.58g **Show Work:** \[ m_{\text{CO}_2} = \frac{6.96 \, \text{g NaHCO}_3}{84.02 \, \text{g NaHCO}_3} \times \left(\frac{1 \, \text{mol CO}_2}{1 \, \text{mol NaHCO}_3}\right) \times 44.01 \, \text{g CO}_2 \rightarrow 3.58 \, \text{g} \] 6. **What is the percent yield?** **Show Work:** 7. **What is the percent error?** **Show Work:** 8. **Matter cannot be created nor destroyed during a reaction. Does this apply to this lab? (Yes or No)** Explain your answer: Why not 100% yield?