Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C6H12O6) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

A) 27.8 Torr B) 16.9 Torr C) 28.8 Torr D) 36.9 Torr E) 24.9 Torr A) 27.8 Torr B) 16.9 Torr C) 28.8 Torr D) 36.9 Torr E) 24.9 Torr

Match the following. -0.050 mol kg-1 C6H12O6 (aqueous)

A) solution of ionic compound with highest freezing point. B) solution that is most strongly dependent upon pressure C) solution with ΔTb = 0.026 °C D) highest boiling point E) largest van't Hoff factor A) solution of ionic compound with highest freezing point. B) solution that is most strongly dependent upon pressure C) solution with ΔTb = 0.026 °C D) highest boiling point E) largest van't Hoff factor

Exam 12: Solutions

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L^-1 sucrose II. 0.00095 mol L^-¹ glucose III. 0.0060 mol L^-1 glycerin

(Multiple Choice)

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Question 141

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

(Multiple Choice)

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Question 142

What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

(Essay)

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Question 143

Define smoke as a colloid.

(Multiple Choice)

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Question 144

Identify the compound whose solubility is least affected by temperature.

(Multiple Choice)

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Question 145

Based on general trends in solubility, which of the following compounds is least soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?

(Multiple Choice)

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Question 146

Identify the major force between ethanol and water.

(Multiple Choice)

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Question 147

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

(Essay)

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Question 148

To make a 2.00 mol kg^-1 solution, one could take 2.00 moles of solute and add ________.

(Multiple Choice)

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Question 149

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

(Multiple Choice)

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Question 150

Identify the compound whose solubility decreases with increasing temperature.

(Multiple Choice)

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Question 151

What mass (in g) of NH₃ must be dissolved in 475 g of methanol to make a 0.250 mol kg^-1 solution?

(Multiple Choice)

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Question 152

Match the following. -0.050 mol kg^-1 C₆H₁₂O₆(aqueous)

(Multiple Choice)

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Question 153

A solution of methanol and water has a vapour pressure of 213 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively.

(Multiple Choice)

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Question 154

What mass of ethane (CH₃CH₃) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL^-1.

(Multiple Choice)

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Question 155

Twice as much pentane (C₅H₁₂) is mixed with hexane (C₆H₁₄) by mass. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

(Multiple Choice)

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Question 156

Identify the classification of whipped cream.

(Multiple Choice)

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Question 157

Which of the following concentration units are temperature dependent?

(Multiple Choice)

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Question 158

Four times as much pentane (C₅H₁₂) by mass is mixed with hexane (C₆H₁₄). Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

(Multiple Choice)

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Question 159

Which of the following ions should have the most exothermic Δ_hydrationH?

(Multiple Choice)

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Question 160

Showing 141 - 160 of 167

Exam 12: Solutions

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L-1 sucrose II. 0.00095 mol L-1 glucose III. 0.0060 mol L-1 glycerin

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

What happens to a supersaturated solution of potassium acetate once it is cooled and a small crystal of solid potassium acetate is added?

Define smoke as a colloid.

Identify the compound whose solubility is least affected by temperature.

Based on general trends in solubility, which of the following compounds is least soluble in hexane (CH3CH2CH2CH2CH2CH2CH3)?

Identify the major force between ethanol and water.

How does a solution of two volatile components with strong solute-solvent attractions deviate from Raoult's law? Why?

To make a 2.00 mol kg-1 solution, one could take 2.00 moles of solute and add ________.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C6H12O6) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

Identify the compound whose solubility decreases with increasing temperature.

What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 mol kg-1 solution?

Match the following. -0.050 mol kg-1 C6H12O6 (aqueous)

A solution of methanol and water has a vapour pressure of 213 Torr. What would you predict as the mole fractions of each component, assuming ideal behaviour? The vapour pressures of methanol and water are 256 Torr and 55.3 Torr, respectively.

What mass of ethane (CH3CH3) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL-1.

Twice as much pentane (C5H12) is mixed with hexane (C6H14) by mass. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Identify the classification of whipped cream.

Which of the following concentration units are temperature dependent?

Four times as much pentane (C5H12) by mass is mixed with hexane (C6H14). Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Which of the following ions should have the most exothermic ΔhydrationH?

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Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L^-1 sucrose II. 0.00095 mol L^-¹ glucose III. 0.0060 mol L^-1 glycerin

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

Based on general trends in solubility, which of the following compounds is least soluble in hexane (CH₃CH₂CH₂CH₂CH₂CH₂CH₃)?

To make a 2.00 mol kg^-1 solution, one could take 2.00 moles of solute and add ________.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

What mass (in g) of NH₃ must be dissolved in 475 g of methanol to make a 0.250 mol kg^-1 solution?

Match the following. -0.050 mol kg^-1 C₆H₁₂O₆(aqueous)

What mass of ethane (CH₃CH₃) is contained in 50.0 mL of a 13.9% by mass solution of ethane in hexane? The density of the solution is 0.611 g mL^-1.

Twice as much pentane (C₅H₁₂) is mixed with hexane (C₆H₁₄) by mass. Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Four times as much pentane (C₅H₁₂) by mass is mixed with hexane (C₆H₁₄). Calculate the vapour pressure of the resulting solution. The vapour pressures of pure pentane and hexane are 425 Torr and 151 Torr, respectively. Assume ideal behaviour.

Which of the following ions should have the most exothermic Δ_hydrationH?