Q2) 90 proof bourbon is 45% ethanol (CH,CH2OH). Determine each of the following for this material. Youmay need to know that the density of this bourbon is 0.9227 g/ml (1), pure ethanol is 0.7893 g/mL (2),and water (assume the rest is just water) is 1.00 g/mL.a) What is the mole fraction ethanol?b) What is the molarity of the ethanol?c) What is the molality of the ethanol?Q3) Exercise #23 from your text has CO2 in a drink at 0.10 M concentration but only under high pressure.When you open a can, the pressure drops to 1.0 atm. How much (moles) CO, is released from the canwhen it is opened? [Note: think about how #23 was solved and then do that again for the changedquestion here. The difference should give you your answer..]Q4) Assuming ideal solution behavior, what is the boiling point of a solution of the sugar solution in Q1above? [You will need table 11.2 from the text for this)

Since you have posted multiple questions we will solve only the first question for you according to…

Q2) 90 proof bourbon is 45% ethanol (CH,CH,OH). Determine each of the following for this material, You may need to know that the density of this bourbon is 0.9227 g/ml (1), pure ethanol is 0.7893 g/mL (2), and water (assume the rest is just water) is 1.00 g/mL. a) What is the mole fraction ethanol? b) What is the molarity of the ethanol? c) What is the molality of the ethanol?

Q2) 90 proof bourbon is 45% ethanol (CH,CH,OH). Determine each of the following for this material, You may need to know that the density of this bourbon is 0.9227 g/ml (1), pure ethanol is 0.7893 g/mL (2), and water (assume the rest is just water) is 1.00 g/mL. a) What is the mole fraction ethanol? b) What is the molarity of the ethanol? c) What is the molality of the ethanol?

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...

See similar textbooks

Similar questions

please answer (: pls double check answer last one needed on aleks
0.0821 kg of biphenyl (C12H10) is dissolve in benzene (CHo) to create a solution with a total volume of 350.0 mL. (Assume the change in volume is negligible) a) What intermolecular forces are shared between biphenyl and benzene? b) If the boiling point of pure benzene is 80.1 °C, then what would be the boiling point of this solution in °C? (Kb for benzene is 2.53 °C/m and the density of benzene is 0.877 g/mL) c) If the vapor pressure of pure benzene is 24.4 kPa at 40.0 °C, then what will the vapor pressure of the solution be in kPa? (Consider biphenyl to be nonvolatile and the density of benzene is 0.877 g/mL) d) What would be the osmotic pressure (in atm) of this solution at 40.0 °C? Assume the density of the solution is the same as benzene, 0.877 g/mL.
A solution is made by mixing 121. g of heptane (C₁₂H₁6) and 107. g of chloroform (CHC13). Calculate the mole fraction of heptane in this solution. Round your answer to 3 significant digits. 0
Please help me with #2
oogle Chrome File Edit View History ! Q C 10 Exam3_Part1 app.aktiv.com 2 W S F2 X 30 command X #3 E 80 F3 D Bookmarks C Based only on intermolecular forces, which of the following would be the most soluble in CH₂OH? Aktiv Chemistry - Work 4 Profiles Tab Window 2,884 R F A) CH₂CH₂OCH₂CH₂ B) CH₂CH₂OH C) CH₂OCH₂ D) CH₂CH₂CH NOV 21 % X 5 V O F5 Help T Question 15 of 24 G 431 6 B tv MacBook Air F6 Y H S & 7 8 F7 U N Å * 8 ... DII F8 J O 9 M K E F9 O 3 L o F10 M Paused Relaunch to update : 80 P Tue Nov 21 9 L Submit + 11 {
None
Trichloroethylene, C2HCl3 is used as a dry cleaning solvent and an industrial extraction agent. The EPA (Environmental Protection Agency) has set a limit of 5.0 ppb trichloroethylene in drinking water. Assuming that the average person consumes 2.0 L of drinking water in a day, what is the maximum mass of trichloroethylene that a person could be exposed to through drinking water? Assume that drinking water has a density of 1.0 g/mL. µ g
Given the following mixture of two compounds 45.00 mL of X (MW =82.00 g/mol)(density 1.077 g/mL) and 710.00 mL of Y (91.00 g/mol))(density 0.907 g/mL). The boiling point of pure Y is -18.00 degrees C. The molal boiling constant is 2.049 degrees C/m. What is the boiling point of the solution, in degrees C?
The normal boiling point of a certain liquid X is 131.10°C, but when 32.9g of glycine (C2H5NO2) are dissolved in 600.g of X the solution boils at 132.1°C instead. Use this information to calculate the molal boiling point elevation constant Kb of X.Round your answer to 2 significant digits. Please do not round untill the end =Kb⋅°Ckgmol
With the given data, calculate the enthalpy of hydration for both lithium chloride (LiCl) and sodium chloride (NaCl). Which of the two cations, lithium or sodium, will establish the strongest ion-dipole interactions with water? Explain. Lithium chloride has a lattice energy of -834kJ/mol and ΔHsol = -37,0 kJ/mol sodium chloride has a lattice energy of -769kJ/mol and ΔHsol = +3,88 kJ/mol.
nolageiged thiot pnicee Data Activities 1 and 2 Data Table 1 20/11/11 Temperature (°C) Pure Lauric Acid Temperature (°C) Lauric Acid + 0.4 g Temperature (°C) Lauric Acid + 0.5 g Benzoic Acid Time (minutes) Benzoic Acid 65.0 0.0 60.0 65.0 0.5 57 59 58 55 1.0 57 52 1.5 50 48 47 2.0 49 46 47 2.5 48 45 46 3.0 42 44 45 3.5 41 43 42 4.0 43 4.5 40 41 5.0 나D 38 to 41 5.5 40 36 6.0 41 40 35 6.5 41 40 35 7.0 41 40 35 7.5 40 35 8.0 41 40 35 O 2016 Carolina Biological Supply Company
Please provide expl