Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 mol L-1 O2 at 25 °C.The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10-3 mol L-1 bar-1.

A) 1.9 bar B) 0.53 bar C) 0.24 bar D) 0.77 bar E) 0.32 bar A) 1.9 bar B) 0.53 bar C) 0.24 bar D) 0.77 bar E) 0.32 bar

What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane,C6H14?

A) 0.0715 B) 0.0770 C) 0.133 D) 0.154 A) 0.0715 B) 0.0770 C) 0.133 D) 0.154

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

A) 4.09 × 10-3 B) 7.80 × 10-2 C) 1.28 × 10-3 D) 7.23 × 10-2 E) 2.45 × 10-3 A) 4.09 × 10-3 B) 7.80 × 10-2 C) 1.28 × 10-3 D) 7.23 × 10-2 E) 2.45 × 10-3

Calculate the mole fraction of MgCl2 in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.

A) 0.00841 B) 0.0270 C) 0.00900 D) 0.0252 E) 0.0167 A) 0.00841 B) 0.0270 C) 0.00900 D) 0.0252 E) 0.0167

Determine the solubility of CO2 in soda water at 25 °C if the pressure of CO2 is 5.2 bar.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 mol L-1 bar-1.

A) 0.15 mol L-1 B) 0.57 mol L-1 C) 0.65 mol L-1 D) 0.18 mol L-1 E) 0.29 mol L-1 A) 0.15 mol L-1 B) 0.57 mol L-1 C) 0.65 mol L-1 D) 0.18 mol L-1 E) 0.29 mol L-1

Exam 12: Solutions

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4mol L^-1 O₂ at 25 °C.The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10^-3 mol L^-1 bar^-1.

(Multiple Choice)

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Question 121

What is the mole fraction of I₂ in a solution made by dissolving 55.6 g of I₂ in 245 g of hexane,C₆H₁₄?

(Multiple Choice)

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Question 122

A solution is prepared by adding 1.43 mol of KCl to 889 g of water.The concentration of KCl is ________ molal.

(Multiple Choice)

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Question 123

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

(Multiple Choice)

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Question 124

A solution is 0.0433 mol kg^-1 LiF.What is the molarity of the solution if the density is 1.10 g mL^-1?

(Multiple Choice)

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Question 125

A mixture of chloroform and acetone has a vapour pressure of 311 Torr.Calculate the mole fraction of acetone in the mixture.The vapour pressures of chloroform and acetone are 295 Torr and 332 Torr,respectively.Assume ideal behaviour.

(Multiple Choice)

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Question 126

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C₆H₁₂O₆,in 125.9 g of water?

(Multiple Choice)

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Question 127

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g mL^-1.

(Multiple Choice)

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Question 128

Determine the solubility of N₂ in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 mol L^-1bar^-1.

(Multiple Choice)

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Question 129

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

(Multiple Choice)

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Question 130

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C₂H₅OH,in 53.6 g of water?

(Multiple Choice)

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Question 131

Identify the gas that is dissolved in carbonated sodas.

(Multiple Choice)

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Question 132

Identify the classification of opal.

(Multiple Choice)

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Question 133

A solution is prepared by adding 40.00 g of lactose (milk sugar)to 110.0 g of water at $55 ^ { \circ } \mathrm { C }$ 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 $342.3 \mathrm {~g} \mathrm {~mol} ^ { - 1 }$

(Multiple Choice)

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Question 134

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 135

Calculate the mole fraction of MgCl₂ in an aqueous solution prepared by dissolving 0.400 moles of MgCl₂ in 850.0 g of water.

(Multiple Choice)

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Question 136

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 137

Define smoke as a colloid.

(Multiple Choice)

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Question 138

Choose the situation below that would result in a ?_solutionH near 0.

(Multiple Choice)

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Question 139

Determine the solubility of CO₂ in soda water at 25 °C if the pressure of CO₂ is 5.2 bar.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 mol L^-1 bar^-1.

(Multiple Choice)

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Question 140

Showing 121 - 140 of 153

Exam 12: Solutions

Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 mol L-1 O2 at 25 °C.The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10-3 mol L-1 bar-1.

What is the mole fraction of I2 in a solution made by dissolving 55.6 g of I2 in 245 g of hexane,C6H14?

A solution is prepared by adding 1.43 mol of KCl to 889 g of water.The concentration of KCl is ________ molal.

A solution is prepared by dissolving 38.6 g sucrose (C12H22O11)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

A solution is 0.0433 mol kg-1 LiF.What is the molarity of the solution if the density is 1.10 g mL-1?

A mixture of chloroform and acetone has a vapour pressure of 311 Torr.Calculate the mole fraction of acetone in the mixture.The vapour pressures of chloroform and acetone are 295 Torr and 332 Torr,respectively.Assume ideal behaviour.

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C6H12O6,in 125.9 g of water?

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g mL-1.

Determine the solubility of N2 in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10-4 mol L-1 bar-1.

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

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C2H5OH,in 53.6 g of water?

Identify the gas that is dissolved in carbonated sodas.

Identify the classification of opal.

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.

Calculate the mole fraction of MgCl2 in an aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.

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

Define smoke as a colloid.

Choose the situation below that would result in a ?solutionH near 0.

Determine the solubility of CO2 in soda water at 25 °C if the pressure of CO2 is 5.2 bar.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10-2 mol L-1 bar-1.

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Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4mol L^-1 O₂ at 25 °C.The Henry's law constant for oxygen in water at 25 °C is 1.3 × 10^-3 mol L^-1 bar^-1.

What is the mole fraction of I₂ in a solution made by dissolving 55.6 g of I₂ in 245 g of hexane,C₆H₁₄?

A solution is prepared by dissolving 38.6 g sucrose (C₁₂H₂₂O₁₁)in 495 g of water.Determine the mole fraction of sucrose if the final volume of the solution is 508 mL.

A solution is 0.0433 mol kg^-1 LiF.What is the molarity of the solution if the density is 1.10 g mL^-1?

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C₆H₁₂O₆,in 125.9 g of water?

A solution is prepared by dissolving 49.3 g of KBr in enough water to form 473 mL of solution.Calculate the mass % of KBr in the solution if the density is 1.12 g mL^-1.

Determine the solubility of N₂ in water exposed to air at 25 °C if the atmospheric pressure is 1.2 bar.Assume that the mole fraction of nitrogen is 0.78 in air and the Henry's law constant for nitrogen in water at this temperature is 6.1 × 10^-4 mol L^-1bar^-1.

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

What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol,C₂H₅OH,in 53.6 g of water?

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.

Calculate the mole fraction of MgCl₂ in an aqueous solution prepared by dissolving 0.400 moles of MgCl₂ in 850.0 g of water.

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

Choose the situation below that would result in a ?_solutionH near 0.

Determine the solubility of CO₂ in soda water at 25 °C if the pressure of CO₂ is 5.2 bar.The Henry's law constant for carbon dioxide in water at this temperature is 3.4 × 10^-2 mol L^-1 bar^-1.