What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?

A) 0.0 58 mol kg-1 B) 0. 068 mol kg-1 C) 0.85 mol kg-1 D) 61 mol kg-1 A) 0.0 58 mol kg-1 B) 0. 068 mol kg-1 C) 0.85 mol kg-1 D) 61 mol kg-1

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g mL-1) and 387 mL of CH3CH2CH2OH (d = 0.811 g mL-1).

A) 0.630 mol kg-1 B) 0.812 mol kg-1 C) 1.57 mol kg-1 D) 2.01 mol kg-1 E) 4.98 mol kg-1 A) 0.630 mol kg-1 B) 0.812 mol kg-1 C) 1.57 mol kg-1 D) 2.01 mol kg-1 E) 4.98 mol kg-1

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-1 and Kb = 0.512 °C m-1. Use 100 °C as the boiling point of water.

A) 108 °C B) 92 °C C) 130 °C D) 70 °C E) 8.3 °C A) 108 °C B) 92 °C C) 130 °C D) 70 °C E) 8.3 °C

Exam 12: Solutions

Calculate the mass of lactose, C₁₂H₂₂O₁₁, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

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Question 1

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Calculate the total solution volume required to produce an osmotic pressure of 4.87 mbar using 8.21 mg of a protein with a molar mass of 4450 g mol^-1 at 25.0 °C.

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Question 2

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Choose the aqueous solution below with the highest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

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Question 3

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What mass of NaCl is contained in 24.88 g of a 15.00% by mass solution of NaCl in water?

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Question 4

Identify the solute with the highest van't Hoff factor.

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Question 5

Which of the following should have the largest Henry's law constant (k_H) in water at 25 °C?

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Question 6

A solution is prepared by adding 40.00 g of lactose (milk sugar) to 110.0 g of water at The partial pressure of water above the solution is ________ Torr. The vapour pressure of pure water at 55 °C is 0.1553 bar. The MW of lactose is

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Question 7

Which of the following should have the smallest Henry's law constant (k_H) in water at 25 °C?

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Question 8

Which of the following statements is TRUE?

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Question 9

What molality of pentane is obtained by dissolving 15 g pentane, C₅H₁₂, in 245.0 g hexane, C₆H₁₄?

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Question 10

Define osmosis.

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Question 11

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g mL^-1) and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g mL^-1).

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Question 12

Identify the gas that is dissolved in carbonated sodas.

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Question 13

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1). Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

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Question 14

Give the preparation of rock candy.

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Question 15

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water.

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Question 16

Identify the classification of opal.

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Question 17

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol^-1) would be needed to dissolve in 500.0 g of water? K_b (water) = 0.512 °C m^-1.

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Question 18

When LiI is dissolved in water, the solution becomes hotter. Choose the situation below that best describes this change.

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Question 19

Define the Tyndall effect.

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Question 20

Showing 1 - 20 of 167

Exam 12: Solutions

Calculate the mass of lactose, C12H22O11, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Calculate the total solution volume required to produce an osmotic pressure of 4.87 mbar using 8.21 mg of a protein with a molar mass of 4450 g mol-1 at 25.0 °C.

Choose the aqueous solution below with the highest freezing point. These are all solutions of nonvolatile solutes and you should assume ideal van't Hoff factors where applicable.

What mass of NaCl is contained in 24.88 g of a 15.00% by mass solution of NaCl in water?

Identify the solute with the highest van't Hoff factor.

Which of the following should have the largest Henry's law constant (kH) in water at 25 °C?

A solution is prepared by adding 40.00 g of lactose (milk sugar) to 110.0 g of water at The partial pressure of water above the solution is ________ Torr. The vapour pressure of pure water at 55 °C is 0.1553 bar. The MW of lactose is

Which of the following should have the smallest Henry's law constant (kH) in water at 25 °C?

Which of the following statements is TRUE?

What molality of pentane is obtained by dissolving 15 g pentane, C5H12, in 245.0 g hexane, C6H14?

Define osmosis.

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d = 0.792 g mL-1) and 387 mL of CH3CH2CH2OH (d = 0.811 g mL-1).

Identify the gas that is dissolved in carbonated sodas.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g mol-1) dissolved in 722 mL of benzene (d = 0.877 g mL-1). Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m-1.

Give the preparation of rock candy.

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-1 and Kb = 0.512 °C m-1. Use 100 °C as the boiling point of water.

Identify the classification of opal.

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol-1) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512 °C m-1.

When LiI is dissolved in water, the solution becomes hotter. Choose the situation below that best describes this change.

Define the Tyndall effect.

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Calculate the mass of lactose, C₁₂H₂₂O₁₁, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Calculate the total solution volume required to produce an osmotic pressure of 4.87 mbar using 8.21 mg of a protein with a molar mass of 4450 g mol^-1 at 25.0 °C.

Which of the following should have the largest Henry's law constant (k_H) in water at 25 °C?

Which of the following should have the smallest Henry's law constant (k_H) in water at 25 °C?

What molality of pentane is obtained by dissolving 15 g pentane, C₅H₁₂, in 245.0 g hexane, C₆H₁₄?

Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH₃OH (d = 0.792 g mL^-1) and 387 mL of CH₃CH₂CH₂OH (d = 0.811 g mL^-1).

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1). Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water.

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol^-1) would be needed to dissolve in 500.0 g of water? K_b (water) = 0.512 °C m^-1.