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Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction below. NaHCO3(aq) + CH3COOH(aq) → NACH3COO(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 1. Obtain and record the mass of a 100 mL beaker. 2. With beaker A still on the balance, add approximately Record the mass accurately 3. Obtain 50.0 mL of vinegar. Be sure to take your measurement at eye level. 4. Place the filled graduated cylinder and the beaker of baking soda on the balance. Record the combined 5.00 grams of baking soda to the beaker. mass. 5. Performing the reaction: a. Slowly add vinegar to the beaker. Gently swirl the contents before adding more. Use all 50.0 mL of vinegar. b. Place the beaker and empty graduated cylinder on the balance and record their combined mass. Data: .76 Mass of empty beaker Mass of beaker plus baking soda Mass of baking soda (2-1) Mass of full graduated cylinder and beaker of baking soda Mass of beaker and empty graduated cylinder at the end Mass of carbon dioxide that escaped (4-5) 1 3 4 2956 6. Calculations and Analysis: 1. If vinegar is 5% acetic acid and the density of vinegar is 1.05 g/mL, how many grams of acetic acid where in your 50.0 mL of vinegar? 2. Determine the limiting reactant and theoretical yield of carbon dioxide. 3. Determine the percent yield of carbon dioxide. 4. Calculate the percent error for this experiment. 5. If you did this experiment a second time, what would you do differently.

Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction below. NaHCO3(aq) + CH3COOH(aq) → NACH3COO(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 1. Obtain and record the mass of a 100 mL beaker. 2. With beaker A still on the balance, add approximately Record the mass accurately 3. Obtain 50.0 mL of vinegar. Be sure to take your measurement at eye level. 4. Place the filled graduated cylinder and the beaker of baking soda on the balance. Record the combined 5.00 grams of baking soda to the beaker. mass. 5. Performing the reaction: a. Slowly add vinegar to the beaker. Gently swirl the contents before adding more. Use all 50.0 mL of vinegar. b. Place the beaker and empty graduated cylinder on the balance and record their combined mass. Data: .76 Mass of empty beaker Mass of beaker plus baking soda Mass of baking soda (2-1) Mass of full graduated cylinder and beaker of baking soda Mass of beaker and empty graduated cylinder at the end Mass of carbon dioxide that escaped (4-5) 1 3 4 2956 6. Calculations and Analysis: 1. If vinegar is 5% acetic acid and the density of vinegar is 1.05 g/mL, how many grams of acetic acid where in your 50.0 mL of vinegar? 2. Determine the limiting reactant and theoretical yield of carbon dioxide. 3. Determine the percent yield of carbon dioxide. 4. Calculate the percent error for this experiment. 5. If you did this experiment a second time, what would you do differently.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction below. NaHCO3(aq) + CH3COOH(aq) → NACH3COO(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 1. Obtain and record the mass of a 100 mL beaker. 2. With beaker A still on the balance, add approximately Record the mass accurately 3. Obtain 50.0 mL of vinegar. Be sure to take your measurement at eye level. 4. Place the filled graduated cylinder and the beaker of baking soda on the balance. Record the combined 5.00 grams of baking soda to the beaker. mass. 5. Performing the reaction: a. Slowly add vinegar to the beaker. Gently swirl the contents before adding more. Use all 50.0 mL of vinegar. b. Place the beaker and empty graduated cylinder on the balance and record their combined mass. Data: .76 Mass of empty beaker Mass of beaker plus baking soda Mass of baking soda (2-1) Mass of full graduated cylinder and beaker of baking soda Mass of beaker and empty graduated cylinder at the end Mass of carbon dioxide that escaped (4-5) 1 3 4 2956 6. Calculations and Analysis: 1. If vinegar is 5% acetic acid and the density of vinegar is 1.05 g/mL, how many grams of acetic acid where in your 50.0 mL of vinegar? 2. Determine the limiting reactant and theoretical yield of carbon dioxide. 3. Determine the percent yield of carbon dioxide. 4. Calculate the percent error for this experiment. 5. If you did this experiment a second time, what would you do differently.
Transcribed Image Text:Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction below. NaHCO3(aq) + CH3COOH(aq) → NACH3COO(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 1. Obtain and record the mass of a 100 mL beaker. 2. With beaker A still on the balance, add approximately Record the mass accurately 3. Obtain 50.0 mL of vinegar. Be sure to take your measurement at eye level. 4. Place the filled graduated cylinder and the beaker of baking soda on the balance. Record the combined 5.00 grams of baking soda to the beaker. mass. 5. Performing the reaction: a. Slowly add vinegar to the beaker. Gently swirl the contents before adding more. Use all 50.0 mL of vinegar. b. Place the beaker and empty graduated cylinder on the balance and record their combined mass. Data: .76 Mass of empty beaker Mass of beaker plus baking soda Mass of baking soda (2-1) Mass of full graduated cylinder and beaker of baking soda Mass of beaker and empty graduated cylinder at the end Mass of carbon dioxide that escaped (4-5) 1 3 4 2956 6. Calculations and Analysis: 1. If vinegar is 5% acetic acid and the density of vinegar is 1.05 g/mL, how many grams of acetic acid where in your 50.0 mL of vinegar? 2. Determine the limiting reactant and theoretical yield of carbon dioxide. 3. Determine the percent yield of carbon dioxide. 4. Calculate the percent error for this experiment. 5. If you did this experiment a second time, what would you do differently.
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