234 Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction bel NaHCO3(aq) + CH3COOH(aq) → NACH3CO0(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 000 grams of baking soda to the beaker. 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 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: B.76 Mass of empty beaker 1. 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) 9. पिछा 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. 1.
234 Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction bel NaHCO3(aq) + CH3COOH(aq) → NACH3CO0(aq) + H2O(1) + CO2(aq) Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and electronic balance. Procedure: 000 grams of baking soda to the beaker. 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 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: B.76 Mass of empty beaker 1. 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) 9. पिछा 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. 1.
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Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability
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I need help with questions 2-5 with guided steps.... I only got help with the first one which I understood.
Transcribed Image Text:234
Purpose: To determine the limiting reactant and the percent yield of carbon dioxide in the reaction bel
NaHCO3(aq) + CH3COOH(aq) → NACH3CO0(aq) + H2O(1) + CO2(aq)
Materials: Baking Soda (NaHCO3), Acetic Acid (CH3COOH), 1 beaker, scoop, graduated cylinder, and
electronic balance.
Procedure:
000
grams of baking soda to the beaker.
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
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:
B.76
Mass of empty beaker
1.
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)
9.
पिछा
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.
1.
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