CHM1046 Plicker Questions for Exam Review
Use these Plicker Questions from class to study for any upcoming exams - including the Final Exam
1. A solution of 0.400 g of a nonelectrolyte in 40.0 g of water freezes at -0.465oC. What is the molecular weight of the non-electrolyte? (Kf = -1.86oC/m).
A 36.0
B 40.0
C 44.0
D 80.0
2. What is the mole fraction of C6H12 in the vapor above a solution of 10.0 g of CH2Cl2 and 1.00 g C6H12 at 25oC if the vapor pressures of the pure solvents are 435 and 166 mm Hg respectively at 25oC?
(Atomic weights: C = 12.01, H = 1.008, Cl = 35.45).
A 0.0371
B 0.0730
C 0.0920
D 0.110
3. Which of the following solutions should have the lowest boiling point?
A 0.01 m NaCl
B 0.01 m sucrose
C 0.008 m CaCl2
D 0.006 m Mg(OH)2
4. A 1.00 g sample of Cr(NH3)4Cl4 is dissolved in 25.0 g of water and the freezing point of the solution is -0.85oC. How many ions are produced per mole of compound? The Kf of water is -1.86 oC/molal.
(Atomic weights: Cr = 52.00, N = 14.01, H = 1.008, Cl = 35.45).
A 4
B 3
C 2
D 1
5. A 0.0100 g sample of Co(NH2CH2CH2NH2)2Cl3 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 52.1 mm Hg at 25oC. How many moles of ions are produced per mole of compound?
(Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45).
A 4
B 3
C 2
D 1
6. Urea, NH2CONH2, is a nonvolatile nonelectrolyte. Calculate the freezing point of a solution of 30.0 g of urea in 250 g of water. (Kf = -1.86oC/m)
(Atomic weights: C = 12.01, H = 1.008, O = 16.00, N = 14.00).
A- -3.12
B -2.42
C -3.72
D -4.12
7. A solution of 2.00 g of a nonelectrolyte is dissolved in 10.0 g of water and the solution freezes at -3.72oC. What is the molecular weight of the nonelectrolyte? (Kf = -1.86oC/m).
A 75
B 100
C 125
D 150
8. A 0.100 m solution of NaCl in water freezes at -0.348oC. What is the van't Hoff factor (i) for NaCl? (Kf = -1.86oC/m).
A 1.81
B 1.84
C 1.87
D 1.90
9. Which of the following aqueous solutions should have the highest osmotic pressure?
A 0.02 M sucrose at 15oC
B 0.008 M CaCl2 at 50oC
C 0.01 M NaCl at 50oC
D 0.008 M CaCl2 at 25oC
1. A solution of 0.400 g of a nonelectrolyte in 40.0 g of water freezes at -0.465oC. What is the molecular weight of the non-electrolyte? (Kf = -1.86oC/m).
A 36.0
B 40.0
C 44.0
D 80.0
2. What is the mole fraction of C6H12 in the vapor above a solution of 10.0 g of CH2Cl2 and 1.00 g C6H12 at 25oC if the vapor pressures of the pure solvents are 435 and 166 mm Hg respectively at 25oC?
(Atomic weights: C = 12.01, H = 1.008, Cl = 35.45).
A 0.0371
B 0.0730
C 0.0920
D 0.110
3. Which of the following solutions should have the lowest boiling point?
A 0.01 m NaCl
B 0.01 m sucrose
C 0.008 m CaCl2
D 0.006 m Mg(OH)2
4. A 1.00 g sample of Cr(NH3)4Cl4 is dissolved in 25.0 g of water and the freezing point of the solution is -0.85oC. How many ions are produced per mole of compound? The Kf of water is -1.86 oC/molal.
(Atomic weights: Cr = 52.00, N = 14.01, H = 1.008, Cl = 35.45).
A 4
B 3
C 2
D 1
5. A 0.0100 g sample of Co(NH2CH2CH2NH2)2Cl3 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 52.1 mm Hg at 25oC. How many moles of ions are produced per mole of compound?
(Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45).
A 4
B 3
C 2
D 1
6. Urea, NH2CONH2, is a nonvolatile nonelectrolyte. Calculate the freezing point of a solution of 30.0 g of urea in 250 g of water. (Kf = -1.86oC/m)
(Atomic weights: C = 12.01, H = 1.008, O = 16.00, N = 14.00).
A- -3.12
B -2.42
C -3.72
D -4.12
7. A solution of 2.00 g of a nonelectrolyte is dissolved in 10.0 g of water and the solution freezes at -3.72oC. What is the molecular weight of the nonelectrolyte? (Kf = -1.86oC/m).
A 75
B 100
C 125
D 150
8. A 0.100 m solution of NaCl in water freezes at -0.348oC. What is the van't Hoff factor (i) for NaCl? (Kf = -1.86oC/m).
A 1.81
B 1.84
C 1.87
D 1.90
9. Which of the following aqueous solutions should have the highest osmotic pressure?
A 0.02 M sucrose at 15oC
B 0.008 M CaCl2 at 50oC
C 0.01 M NaCl at 50oC
D 0.008 M CaCl2 at 25oC
CHM1046 Plicker Questions for Exam Review - Answers
1. A solution of 0.400 g of a nonelectrolyte in 40.0 g of water freezes at -0.465oC. What is the molecular weight of the non-electrolyte? (Kf = -1.86oC/m).
B 40.0
2. What is the mole fraction of C6H12 in the vapor above a solution of 10.0 g of CH2Cl2 and 1.00 g C6H12 at 25oC if the vapor pressures of the pure solvents are 435 and 166 mm Hg respectively at 25oC?
(Atomic weights: C = 12.01, H = 1.008, Cl = 35.45).
A 0.0371
3. Which of the following solutions should have the lowest boiling point?
B 0.01 m sucrose
4. A 1.00 g sample of Cr(NH3)4Cl4 is dissolved in 25.0 g of water and the freezing point of the solution is -0.85oC. How many ions are produced per mole of compound? The Kf of water is -1.86 oC/molal.
(Atomic weights: Cr = 52.00, N = 14.01, H = 1.008, Cl = 35.45).
B 3
5. A 0.0100 g sample of Co(NH2CH2CH2NH2)2Cl3 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 52.1 mm Hg at 25oC. How many moles of ions are produced per mole of compound?
(Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45).
C 2
6. Urea, NH2CONH2, is a nonvolatile nonelectrolyte. Calculate the freezing point of a solution of 30.0 g of urea in 250 g of water. (Kf = -1.86oC/m)
(Atomic weights: C = 12.01, H = 1.008, O = 16.00, N = 14.00).
C -3.72
7. A solution of 2.00 g of a nonelectrolyte is dissolved in 10.0 g of water and the solution freezes at -3.72oC. What is the molecular weight of the nonelectrolyte? (Kf = -1.86oC/m).
B 100
8. A 0.100 m solution of NaCl in water freezes at -0.348oC. What is the van't Hoff factor (i) for NaCl? (Kf = -1.86oC/m).
C 1.87
9. Which of the following aqueous solutions should have the highest osmotic pressure?
B 0.008 M CaCl2 at 50oC
B 40.0
2. What is the mole fraction of C6H12 in the vapor above a solution of 10.0 g of CH2Cl2 and 1.00 g C6H12 at 25oC if the vapor pressures of the pure solvents are 435 and 166 mm Hg respectively at 25oC?
(Atomic weights: C = 12.01, H = 1.008, Cl = 35.45).
A 0.0371
3. Which of the following solutions should have the lowest boiling point?
B 0.01 m sucrose
4. A 1.00 g sample of Cr(NH3)4Cl4 is dissolved in 25.0 g of water and the freezing point of the solution is -0.85oC. How many ions are produced per mole of compound? The Kf of water is -1.86 oC/molal.
(Atomic weights: Cr = 52.00, N = 14.01, H = 1.008, Cl = 35.45).
B 3
5. A 0.0100 g sample of Co(NH2CH2CH2NH2)2Cl3 is dissolved in 25.0 ml of water and the osmotic pressure of the solution is 52.1 mm Hg at 25oC. How many moles of ions are produced per mole of compound?
(Atomic weights: Co = 58.93, C = 12.01, N = 14.01, H = 1.008, Cl = 35.45).
C 2
6. Urea, NH2CONH2, is a nonvolatile nonelectrolyte. Calculate the freezing point of a solution of 30.0 g of urea in 250 g of water. (Kf = -1.86oC/m)
(Atomic weights: C = 12.01, H = 1.008, O = 16.00, N = 14.00).
C -3.72
7. A solution of 2.00 g of a nonelectrolyte is dissolved in 10.0 g of water and the solution freezes at -3.72oC. What is the molecular weight of the nonelectrolyte? (Kf = -1.86oC/m).
B 100
8. A 0.100 m solution of NaCl in water freezes at -0.348oC. What is the van't Hoff factor (i) for NaCl? (Kf = -1.86oC/m).
C 1.87
9. Which of the following aqueous solutions should have the highest osmotic pressure?
B 0.008 M CaCl2 at 50oC