Oregon State University



CH 222 Exam 2 Practice with Key (Key follows the pristine Exam)

1. Which is the higher pressure?

A. 2000 torr

B. 2.5 atm

C. 265 kPa

D. 2 × 103 mm Hg

E. The pressure on the top of Mt. Everest.

2. Which of the following statements about gases is TRUE?

A. If the amount of a sample of an ideal gas is doubled while the pressure and temperature remain constant, its volume will halve.

B. Boyle’s Law applies to conditions of constant temperature, volume and pressure.

C. Molecules of any ideal gas have the same velocity at the same temperature, regardless of the identity of the gas.

D. The volume of an ideal gas will drop by approximately (1/273) of its value if its temperature drops by 1 °C .

E. Standard temperature and pressure is 1 atm and 25 °C.

4. A bunch of bored, crazy college students hiked to the top of Mt. Hood where they blew up a balloon and calculated its volume to be 0.080 m3. They noted the temperature to be −20 ºC and the air pressure to be 634 torr. Upon driving to Salem (34 ºC, 765 torr) they measured the volume of the balloon again. What was it?

A. 0.020 m3

B. 0.050 m3

C. 0.080 m3

D. 0.11 m3

E. 0.16 m3

5. “Halothane” is a common anesthetic inhalant used for surgical purposes. The partial pressure of halothane in the lungs must be maintained within a critical range of 4.0 torr - 8.0 torr for successful anesthetization. The halothane mol fraction = 0.010 in the lungs of a certain patient. Is this within the target range? (Assume operating room pressure to be 760 torr.)

A. No, the mol fraction is too low; patient may wake.

B. No, the mol fraction is too high; patient respiration is dangerously low.

C. Yes, it is within the safe range, but on the high side.

D. Yes, it is within the safe range, but on the low side.

E. There is not enough information to answer the question.

6. A mixture of 3 gases has a total pressure of 1,200 Torr. The mixture is analyzed and found to contain 6.0 mol CO2, 4.0 mol CO and 2.0 mol Ar. What is the partial pressure of Ar?

A. 1200 torr

B. 200 torr

C. 7,200 torr

D. 2,400 torr

E. 600 torr

7. 1.00 mole of HCl(l) is reacted with an excess of Mg(s). What volume of hydrogen gas will result if the reaction is conducted at STP?

A. 22.4 L

B. 44.8 L

C. 273 L

D. 11.2 L

E. 0.082 L

8. Using the graph below, determine the gas that has the lowest density at STP.

[pic]

A) A

B) B

C) C

D) D

E) All of the gases have the same density at STP.

9. Which of the following gas samples would be most likely to behave ideally under the stated conditions?

A) Ne at STP

B) CO at 200 atm and 25°C

C) SO2 at 2 atm and 0 K

D) N2 at 1 atm and -70°C

E) O2 at 400 atm and 25°C

12. Place the following compounds in order of decreasing strength of intermolecular forces.

HF O2 CO2

A) HF > CO2 > O2

B) HF > O2 > CO2

C) O2 > CO2 > HF

D) CO2 > HF > O2

E) CO2 > O2 > HF

13. In liquid propanol, CH3CH2CH2OH, which intermolecular forces are present?

A) Dispersion, hydrogen bonding and dipole-dipole forces are present.

B) Only dipole-dipole and ion-dipole forces are present.

C) Only dispersion and dipole-dipole forces are present.

D) Only hydrogen bonding forces are present.

E) Only dispersion forces are present.

17. Assign the appropriate labels to the phase diagram shown below.

[pic]

A) A = liquid, B = solid, C = gas, D = critical point

B) A = gas, B = solid, C = liquid, D = triple point

C) A = gas, B = liquid, C = solid, D = critical point

D) A = solid, B = gas, C = liquid, D = supercritical fluid

E) A = liquid, B = gas, C = solid, D = triple point

18. Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature)?

[pic]

A) condensation, followed by vaporization

B) sublimation, followed by deposition

C) vaporization, followed by deposition

D) fusion, followed by vaporization

E) No phase change will occur under the conditions specified.

19. What precipitate is most likely formed from a solution containing Ba2+, Na+, OH-, and CO32-.

A) NaOH

B) BaCO3

C) Na2CO3

D) Ba(OH)2

E) No precipitate will form.

20. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed.

A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s)

B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)

C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s)

D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3 (s)

E) No reaction occurs.

21. Which of the following solutions will have the highest concentration of chloride ions?

A) 0.10 M NaCl

B) 0.10 M MgCl2

C) 0.10 M AlCl3

D) 0.05 M CaCl2

E) All of these solutions have the same concentration of chloride ions.

23. Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.

A) 7.79 M

B) 10.7 M

C) 12.8 M

D) 9.35 M

E) 13.9 M

24. Choose the statement below that is TRUE.

A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.

B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions.

C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions.

D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions.

E) None of the above are true.

25. What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?

A) 2.02 g

B) 4.94 g

C) 1.19 g

D) 8.42 g

E) 1.90 g

28. Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.

A) 130°C

B) 92°C

C) 108°C

D) 70°C

E) 8.3°C

29. Identify the solute with the lowest van't Hoff factor.

A) nonelectrolyte

B) NaCl

C) MgSO4

D) MgCl2

E) FeCl3

30. A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?

A) 223 g/mol

B) 294 g/mol

C) 341 g/mol

D) 448 g/mol

E) 195 g/mol

31. The cubic form for the fictitious element Oregonium is FCC. The atomic radius is

132.0 pm and the density is 34.2 g/cm3. The molar mass of Oregonium is:

(A) 267.4 g/mol

(B) 167.4 g/mol

(C) 367.4 g/mol

(D) 467.4 g/mol

(E) 67.4 g/mol

1 m = 1 x 1012 pm

1 m = 100 cm

For Simple Cubic: l = 2r

For BCC: l = 4r/√3

For FCC: l = 4r/√2

 

34. Consider a fixed amount of gas. Which of the following is FALSE?

 

(a) When the volume is increased at constant temperature, the pressure increases.

(b) When the temperature is increased at constant volume, the pressure increases.

(c) When the temperature is decreased at constant pressure, the volume decreases.

(d) When the pressure is increased at constant temperature, the volume decreases.

 

35. A student places 0.050 mol of CO and 0.025 mol of CO2 into a 1.0 liter balloon at 20 C.

 

(a) The partial pressure of the CO is LESS THAN the partial pressure of CO2.

(b) The partial pressure of the CO is THE SAME AS the partial pressure of CO2.

(c) The partial pressure of the CO is GREATER THAN the partial pressure of CO2.

(d) The mole fraction of CO is LESS THAN the mole fraction the mole fraction of CO2.

 

37. Consider the following five gases: O2 (g) Br2 (g) C2H6 (g) H2 (g) CO (g)

Of these, the gas molecule with the greatest velocity at room temperature is:

  (a) O2 (g).

(b) Br2 (g).

(c) C2H6 (g).

(d) H2 (g).

(e) CO (g).

38. A student places 3.388 g of a noble gas into a 2.00-L container at 293 K and measures the pressure to be 1.02 atm. This noble gas is:

(A) He.

(B) Ne.

(C) Ar.

(D) Kr.

(E) Xe.

39. A student obtains a glass bottle at 24.1 ºC and 0.989 atm. The student closes the bottle containing air [78% N2 (g); 21% O2 (g); 1% other gases]. The student places the bottle over a Bunsen burner so the bottle and the air heat up to 30.5 ºC. Which of the following is true?

A) The gases inside the bottle are traveling faster at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is higher at the higher temperature than at the lower temperature.

(B) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is higher at the higher temperature than at the lower temperature.

(C) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is the same at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

(D) The gases inside the bottle are traveling faster at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

(E) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is lower at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

40. The root-mean-square speed of Ar (g) at 1.07 atm and 301.4 K is:

(A) 434 m/s.

(B) 741 m/s.

(C) 514 m/s.

(D) 7.296 x 10-6 m/s.

(E) 1220 m/s.

41. Shown below is the balanced equation for the combustion of butane (molar mass = 58.12 g/mol). What is the volume (liters) of CO2 (g) produced at 1.500 atm and 298.0 K from the combustion of 116.24 g of butane in excess O2 (g)?

2 C4H10 (g) + 13 O2 (g) ( 8 CO2 (g) + 10 H2O (g)

(A) 125.5 L CO2

(B) 28.08 L CO2

(C) 112.3 L CO2

(D) 224.0 L CO2

(E) 130.5 L CO2

43. Consider dimethyl ether, CH3OCH3. The intermolecular forces present in CH3OCH3 are:

[pic]

(A) Dispersion forces only.

(B) Dipole-dipole forces only.

(C) Dispersion forces and dipole-dipole forces.

(D) Dispersion forces, dipole-dipole forces, and hydrogen bonding.

(E) Hydrogen bonding only.

45. Which of the following has a hydrophilic end (polar, water-loving end) and a hydrophobic end (non-polar, water-fearing end) and has the ability to bridge water molecules to non-polar molecules?

(A) FCC Unit Cell

(B) Graphite

(C) Ethane, CH3CH3

(D) Soap

(E) He

46. The equivalent number of atoms in the FCC unit cell is:

(A) 1

(B) 2

(C) 3

(D) 4

(E) 6

47. The structure below represents:

[pic]

(A) An SC unit cell

(B) A BCC unit cell

(C) A FCC unit cell

(D) A cell phone

(E) A prokaryotic cell

48. The freezing point of 0.500 m aqueous AlCl3 is:

(A) -2.79 (C

(B) +2.79 (C

(C) +5.58 (C

(D) -5.58 (C

(E) -3.72 (C

49. Which of the following sets of compounds are expected to be soluble in water?

(A) CH4, CO2, CF4

(B) NaCl, CH4, CH3OCH3

(C) NaCl, CH3CH2OH, NH3

(D) NaCl, CCl4, C4H10

50. A student dissolves 12.000 g of an unknown polymer in 800 mL of water at 320 K. She measures the osmotic pressure to be 0.0677 mm Hg. What is the molar mass of the polymer?

(A) 2.71 x 106 g/mol

(B) 4.42 x 106 g/mol

(C) 1.73 x 105 g/mol

(D) 1.73 x 106 g/mol

(E) 2.26 x 106 g/mol

KEY FOLLOWS:

1. Which is the higher pressure?

A. 2000 torr

B. 2.5 atm

C. 265 kPa

D. 2 × 103 mm Hg

E. The pressure on the top of Mt. Everest.

2. Which of the following statements about gases is TRUE?

A. If the amount of a sample of an ideal gas is doubled while the pressure and temperature remain constant, its volume will halve.

B. Boyle’s Law applies to conditions of constant temperature, volume and pressure.

C. Molecules of any ideal gas have the same velocity at the same temperature, regardless of the identity of the gas.

D. The volume of an ideal gas will drop by approximately (1/273) of its value if its temperature drops by 1 °C .

E. Standard temperature and pressure is 1 atm and 25 °C.

4. A bunch of bored, crazy college students hiked to the top of Mt. Hood where they blew up a balloon and calculated its volume to be 0.080 m3. They noted the temperature to be −20 ºC and the air pressure to be 634 torr. Upon driving to Salem (34 ºC, 765 torr) they measured the volume of the balloon again. What was it?

A. 0.020 m3

B. 0.050 m3

C. 0.080 m3

D. 0.11 m3

E. 0.16 m3

5. “Halothane” is a common anesthetic inhalant used for surgical purposes. The partial pressure of halothane in the lungs must be maintained within a critical range of 4.0 torr - 8.0 torr for successful anesthetization. The halothane mol fraction = 0.010 in the lungs of a certain patient. Is this within the target range? (Assume operating room pressure to be 760 torr.)

A. No, the mol fraction is too low; patient may wake.

B. No, the mol fraction is too high; patient respiration is dangerously low.

C. Yes, it is within the safe range, but on the high side.

D. Yes, it is within the safe range, but on the low side.

E. There is not enough information to answer the question.

6. A mixture of 3 gases has a total pressure of 1,200 Torr. The mixture is analyzed and found to contain 6.0 mol CO2, 4.0 mol CO and 2.0 mol Ar. What is the partial pressure of Ar?

A. 1200 torr

B. 200 torr

C. 7,200 torr

D. 2,400 torr

E. 600 torr

7. 1.00 mole of HCl(l) is reacted with an excess of Mg(s). What volume of hydrogen gas will result if the reaction is conducted at STP?

A. 22.4 L

B. 44.8 L

C. 273 L

D. 11.2 L

E. 0.082 L

8. Using the graph below, determine the gas that has the lowest density at STP.

[pic]

A) A

B) B

C) C

D) D

E) All of the gases have the same density at STP.

9. Which of the following gas samples would be most likely to behave ideally under the stated conditions?

A) Ne at STP

B) CO at 200 atm and 25°C

C) SO2 at 2 atm and 0 K

D) N2 at 1 atm and -70°C

E) O2 at 400 atm and 25°C

12. Place the following compounds in order of decreasing strength of intermolecular forces.

HF O2 CO2

A) HF > CO2 > O2

B) HF > O2 > CO2

C) O2 > CO2 > HF

D) CO2 > HF > O2

E) CO2 > O2 > HF

13. In liquid propanol, CH3CH2CH2OH, which intermolecular forces are present?

A) Dispersion, hydrogen bonding and dipole-dipole forces are present.

B) Only dipole-dipole and ion-dipole forces are present.

C) Only dispersion and dipole-dipole forces are present.

D) Only hydrogen bonding forces are present.

E) Only dispersion forces are present.

17. Assign the appropriate labels to the phase diagram shown below.

[pic]

A) A = liquid, B = solid, C = gas, D = critical point

B) A = gas, B = solid, C = liquid, D = triple point

C) A = gas, B = liquid, C = solid, D = critical point

D) A = solid, B = gas, C = liquid, D = supercritical fluid

E) A = liquid, B = gas, C = solid, D = triple point

18. Consider the phase diagram below. If the dashed line at 1 atm of pressure is followed from 100 to 500°C, what phase changes will occur (in order of increasing temperature)?

[pic]

A) condensation, followed by vaporization

B) sublimation, followed by deposition

C) vaporization, followed by deposition

D) fusion, followed by vaporization

E) No phase change will occur under the conditions specified.

19. What precipitate is most likely formed from a solution containing Ba2+, Na+, OH-, and CO32-.

A) NaOH

B) BaCO3

C) Na2CO3

D) Ba(OH)2

E) No precipitate will form.

20. Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed.

A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s)

B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s)

C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s)

D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3 (s)

E) No reaction occurs.

21. Which of the following solutions will have the highest concentration of chloride ions?

A) 0.10 M NaCl

B) 0.10 M MgCl2

C) 0.10 M AlCl3

D) 0.05 M CaCl2

E) All of these solutions have the same concentration of chloride ions.

23. Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water. Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.

A) 7.79 M

B) 10.7 M

C) 12.8 M

D) 9.35 M

E) 13.9 M

24. Choose the statement below that is TRUE.

A) A solution will form between two substances if the solute-solvent interactions are of comparable strength to the solute-solute and solvent-solvent interactions.

B) A solution will form between two substances if the solute-solvent interactions are small enough to be overcome by the solute-solute and solvent-solvent interactions.

C) A solution will form between two substances if the solute-solute interactions are strong enough to overcome the solvent-solvent interactions.

D) A solution will form between two substances only if the solvent-solvent interactions are weak enough to overcome the solute-solvent interactions.

E) None of the above are true.

25. What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?

A) 2.02 g

B) 4.94 g

C) 1.19 g

D) 8.42 g

E) 1.90 g

28. Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86°C/m and Kb = 0.512°C/m. Use 100°C as the boiling point of water.

A) 130°C

B) 92°C

C) 108°C

D) 70°C

E) 8.3°C

29. Identify the solute with the lowest van't Hoff factor.

A) nonelectrolyte

B) NaCl

C) MgSO4

D) MgCl2

E) FeCl3

30. A 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. If the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?

A) 223 g/mol

B) 294 g/mol

C) 341 g/mol

D) 448 g/mol

E) 195 g/mol

31. The cubic form for the fictitious element Oregonium is FCC. The atomic radius is

132.0 pm and the density is 34.2 g/cm3. The molar mass of Oregonium is:

(A) 267.4 g/mol

(B) 167.4 g/mol

(C) 367.4 g/mol

(D) 467.4 g/mol

(E) 67.4 g/mol

1 m = 1 x 1012 pm

1 m = 100 cm

For Simple Cubic: l = 2r

For BCC: l = 4r/√3

For FCC: l = 4r/√2

 

34. Consider a fixed amount of gas. Which of the following is FALSE?

 

(a) When the volume is increased at constant temperature, the pressure increases.

(b) When the temperature is increased at constant volume, the pressure increases.

(c) When the temperature is decreased at constant pressure, the volume decreases.

(d) When the pressure is increased at constant temperature, the volume decreases.

 

35. A student places 0.050 mol of CO and 0.025 mol of CO2 into a 1.0 liter balloon at 20 C.

 

(a) The partial pressure of the CO is LESS THAN the partial pressure of CO2.

(b) The partial pressure of the CO is THE SAME AS the partial pressure of CO2.

(c) The partial pressure of the CO is GREATER THAN the partial pressure of CO2.

(d) The mole fraction of CO is LESS THAN the mole fraction the mole fraction of CO2.

 

37. Consider the following five gases: O2 (g) Br2 (g) C2H6 (g) H2 (g) CO (g)

Of these, the gas molecule with the greatest velocity at room temperature is:

  (a) O2 (g).

(b) Br2 (g).

(c) C2H6 (g).

(d) H2 (g).

(e) CO (g).

38. A student places 3.388 g of a noble gas into a 2.00-L container at 293 K and measures the pressure to be 1.02 atm. This noble gas is:

(A) He.

(B) Ne.

(C) Ar.

(D) Kr.

(E) Xe.

39. A student obtains a glass bottle at 24.1 ºC and 0.989 atm. The student closes the bottle containing air [78% N2 (g); 21% O2 (g); 1% other gases]. The student places the bottle over a Bunsen burner so the bottle and the air heat up to 30.5 ºC. Which of the following is true?

B) The gases inside the bottle are traveling faster at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is higher at the higher temperature than at the lower temperature.

(B) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is higher at the higher temperature than at the lower temperature.

(C) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is the same at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

(D) The gases inside the bottle are traveling faster at the higher temperature than at the lower temperature; the pressure inside the bottle is higher at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

(E) The gases inside the bottle are traveling the same velocity at the higher temperature than at the lower temperature; the pressure inside the bottle is lower at the higher temperature than at the lower temperature; the number of moles of gas present inside the bottle is the same at the higher temperature than at the lower temperature.

40. The root-mean-square speed of Ar (g) at 1.07 atm and 301.4 K is:

(A) 434 m/s.

(B) 741 m/s.

(C) 514 m/s.

(D) 7.296 x 10-6 m/s.

(E) 1220 m/s.

41. Shown below is the balanced equation for the combustion of butane (molar mass = 58.12 g/mol). What is the volume (liters) of CO2 (g) produced at 1.500 atm and 298.0 K from the combustion of 116.24 g of butane in excess O2 (g)?

2 C4H10 (g) + 13 O2 (g) ( 8 CO2 (g) + 10 H2O (g)

(A) 125.5 L CO2

(B) 28.08 L CO2

(C) 112.3 L CO2

(D) 224.0 L CO2

(E) 130.5 L CO2

43. Consider dimethyl ether, CH3OCH3. The intermolecular forces present in CH3OCH3 are:

[pic]

(A) Dispersion forces only.

(B) Dipole-dipole forces only.

(C) Dispersion forces and dipole-dipole forces.

(D) Dispersion forces, dipole-dipole forces, and hydrogen bonding.

(E) Hydrogen bonding only.

45. Which of the following has a hydrophilic end (polar, water-loving end) and a hydrophobic end (non-polar, water-fearing end) and has the ability to bridge water molecules to non-polar molecules?

(A) FCC Unit Cell

(B) Graphite

(C) Ethane, CH3CH3

(D) Soap

(E) He

46. The equivalent number of atoms in the FCC unit cell is:

(A) 1

(B) 2

(C) 3

(D) 4

(E) 6

47. The structure below represents:

[pic]

(A) An SC unit cell

(B) A BCC unit cell

(C) A FCC unit cell

(D) A cell phone

(E) A prokaryotic cell

48. The freezing point of 0.500 m aqueous AlCl3 is:

(A) -2.79 (C

(B) +2.79 (C

(C) +5.58 (C

(D) -5.58 (C

(E) -3.72 (C

49. Which of the following sets of compounds are expected to be soluble in water?

(A) CH4, CO2, CF4

(B) NaCl, CH4, CH3OCH3

(C) NaCl, CH3CH2OH, NH3

(D) NaCl, CCl4, C4H10

50. A student dissolves 12.000 g of an unknown polymer in 800 mL of water at 320 K. She measures the osmotic pressure to be 0.0677 mm Hg. What is the molar mass of the polymer?

(A) 2.71 x 106 g/mol

(B) 4.42 x 106 g/mol

(C) 1.73 x 105 g/mol

(D) 1.73 x 106 g/mol

(E) 2.26 x 106 g/mol

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