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b. Given the rate from Part a and the initial concentrations of acetone, H* ion, and I₂ in the reaction mixture, write Equation 3 as it would apply to the mixture. rate= c. What are the unknowns that remain in the equation in Part b?

b. Given the rate from Part a and the initial concentrations of acetone, H* ion, and I₂ in the reaction mixture, write Equation 3 as it would apply to the mixture. rate= c. What are the unknowns that remain in the equation in Part b?

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.BCP
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Please help with question 2b) and 2c)

1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture. 1.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M I2 + 2.0 mL H₂O a. Calculate the initial (diluted) concentration of acetone in the reaction mixture. Mole's =4.0.001 =0.004 mole s ImL ЧМ, Moles (1+1+1e2) ml = 5mL 0.004 mol 0.001 0.005 litre = 0.8M 41= [acetone]ini = 0.8M b. Calculate the initial (diluted) concentration of the hydrogen ion, H+, in the reaction mixture. 1.0.001 = 0.001 mol 0-001 mole 0.005 TIFFe <0.2M [H*]ini = 0.2 M c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture. Iml 0.005 M/₂ 0.005.0.001 = 5×10-s e moles 5 x 10 0.005 litte = 0.001M [12]ini = 0.001 M 2. Using the reaction mixture in Problem 1, a student found that it took 300 seconds for the color of the 12 to disappear. a. What was the rate of the reaction? 0.0050M 0.001 L 0.600005 mol C 10|0|12)=5.0ml rate= 0.001 M 300 S 3.33·10-6m/5 0.0011 b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture, write Equation 3 as it would apply to the mixture. 0.000005 6.005 3.33010-6 rate= c. What are the unknowns that remain in the equation in Part b?
Transcribed Image Text:1. In a reaction involving the iodination of acetone, the following volumes were used to make up the reaction mixture. 1.0 mL 4.0 M acetone + 1.0 mL 1.0 M HCl + 1.0 mL 0.0050 M I2 + 2.0 mL H₂O a. Calculate the initial (diluted) concentration of acetone in the reaction mixture. Mole's =4.0.001 =0.004 mole s ImL ЧМ, Moles (1+1+1e2) ml = 5mL 0.004 mol 0.001 0.005 litre = 0.8M 41= [acetone]ini = 0.8M b. Calculate the initial (diluted) concentration of the hydrogen ion, H+, in the reaction mixture. 1.0.001 = 0.001 mol 0-001 mole 0.005 TIFFe <0.2M [H*]ini = 0.2 M c. Calculate the initial (diluted) concentration of iodine, I2, in the reaction mixture. Iml 0.005 M/₂ 0.005.0.001 = 5×10-s e moles 5 x 10 0.005 litte = 0.001M [12]ini = 0.001 M 2. Using the reaction mixture in Problem 1, a student found that it took 300 seconds for the color of the 12 to disappear. a. What was the rate of the reaction? 0.0050M 0.001 L 0.600005 mol C 10|0|12)=5.0ml rate= 0.001 M 300 S 3.33·10-6m/5 0.0011 b. Given the rate from Part a and the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture, write Equation 3 as it would apply to the mixture. 0.000005 6.005 3.33010-6 rate= c. What are the unknowns that remain in the equation in Part b?
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