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12. Compare your experimental % yield of n-propyl propanoate to the predicted equilibrium yield. Were you successful in driving the reaction to the right?

12. Compare your experimental % yield of n-propyl propanoate to the predicted equilibrium yield. Were you successful in driving the reaction to the right?

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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8:53 l LTE Gmail a bartleby.com SEARCH ASK h CHAT VX MATH SOLV Question wt of flask = 98.4669 wt of product = 20.7868 wt of flask and product = 119.2537 weight of water collected = 4,4 mL wt of water expected 4.5 mL percent yeild of ester = 71.58% %3D 19.0 mL of 0.25 M n-propanol 18.5 mL propionic acid plz answer questions below 10. At room temperature, the equilibrium constant, Keq is approximately 3. Calculate the number of moles of reactants and products expected in the equilibrium mixture of this reaction. (Hint: Complete the ICE table below. Let X be the number of moles of each product fomed t equilibrium. Substue ino the equilibrium equation using the moles of each reactant and product at equilibrium, each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. Solve for X. You can then take the square root of both sides of the equation after cancelling like terms, i. te volumes.) Acid Alcohol + Ester H;0 Initial amount 25/0). (25/V) 33
Transcribed Image Text:8:53 l LTE Gmail a bartleby.com SEARCH ASK h CHAT VX MATH SOLV Question wt of flask = 98.4669 wt of product = 20.7868 wt of flask and product = 119.2537 weight of water collected = 4,4 mL wt of water expected 4.5 mL percent yeild of ester = 71.58% %3D 19.0 mL of 0.25 M n-propanol 18.5 mL propionic acid plz answer questions below 10. At room temperature, the equilibrium constant, Keq is approximately 3. Calculate the number of moles of reactants and products expected in the equilibrium mixture of this reaction. (Hint: Complete the ICE table below. Let X be the number of moles of each product fomed t equilibrium. Substue ino the equilibrium equation using the moles of each reactant and product at equilibrium, each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. Solve for X. You can then take the square root of both sides of the equation after cancelling like terms, i. te volumes.) Acid Alcohol + Ester H;0 Initial amount 25/0). (25/V) 33
8:48 l LTE Gmail a bartleby.com SEARCH & ASK CHAT VX MATH SOLV 10. At room temperature, the equilibrium constant, Keq is approximately 3. Calculate the number of moles of reactants and products expected in the equilibrium mixture of this reaction. (Hint: Complete the ICE table below. Let X be the number of moles of each product fomed at equilibrium. Substitute into the equilibrium equation using the moles of each reactant and product at equilibrium, each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. Solve for X. You can then take the square root of both sides of the equation after cancelling like terms, i.e. the volumes.) Acid Alcohol + Ester H;0 Initial amount (25/V) (25/V) Change At Equilibrium 11. What would the % yield of ester be if the reaction were simply allowed to equilibrate (i.e. no productsare removed)? 12. Compare your experimental % yield of n-propyl propanoate to the predicted equilibrium yield. Were you successful in driving the reaction to the right? Transcribed Image Text: 10. At room temperature, the 33
Transcribed Image Text:8:48 l LTE Gmail a bartleby.com SEARCH & ASK CHAT VX MATH SOLV 10. At room temperature, the equilibrium constant, Keq is approximately 3. Calculate the number of moles of reactants and products expected in the equilibrium mixture of this reaction. (Hint: Complete the ICE table below. Let X be the number of moles of each product fomed at equilibrium. Substitute into the equilibrium equation using the moles of each reactant and product at equilibrium, each divided by the total reaction volume. Leave the equilibrium concentrations as fractions. Solve for X. You can then take the square root of both sides of the equation after cancelling like terms, i.e. the volumes.) Acid Alcohol + Ester H;0 Initial amount (25/V) (25/V) Change At Equilibrium 11. What would the % yield of ester be if the reaction were simply allowed to equilibrate (i.e. no productsare removed)? 12. Compare your experimental % yield of n-propyl propanoate to the predicted equilibrium yield. Were you successful in driving the reaction to the right? Transcribed Image Text: 10. At room temperature, the 33
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