Estimate the normal boiling temperature of propan-1-ol, C3H7OH, given that its vapour pressure is 2701 Pa at 298 K and 9129 Pa at 318 K.

A) 393 K B) 323 K C) 367 K D) 420 K A) 393 K B) 323 K C) 367 K D) 420 K C

Estimate the change in the normal boiling temperature of an aqueous solution made by dissolving 12.6 g of phenol, C6H5OH, in 250 cm3 of water. The ebullioscopic constant of water is 0.51 K kg mol-1.

A) +0.27 K B) +0.068 K C) -1.6 K D) -0.65 K A) +0.27 K B) +0.068 K C) -1.6 K D) -0.65 K

The Henry's law constant for pentan-3-one, C2H5COC2H5, in aqueous solution may be expressed in terms of concentration as 19.6 mol dm-3 kPa-1. Calculate the vapour pressure of pentan-3-one above an aqueous solution that contains 5.23 g of pentan-3-one in 250 cm3 of solution.

A) 12.4 kPa B) 51.0 kPa C) 31.1 kPa D) 3.00 kPa A) 12.4 kPa B) 51.0 kPa C) 31.1 kPa D) 3.00 kPa

For the equilibrium CaCO3(s) ∏ CaO(s) + CO2(g) How many phases are present?

A) 1 B) 2 C) 3 D) The number of phases cannot be determined A) 1 B) 2 C) 3 D) The number of phases cannot be determined

Exam 4: Physical Transformations

When 15.0 cm³ of benzene, C₆H₆, is added to 125 cm³ of water, H₂O, at 20°C, the final volume of the liquid mixture is 137 cm³. Calculate the partial molar volume of benzene in dilute aqueous solutions given that the density of benzene and of water are 0.879 g cm^-3 and 0.998 g cm^-3 respectively, and the partial molar volume of water is 17.8 cm³ mol^-1 at this temperature.

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Question 1

Correct Answer:

Verified

Estimate the normal boiling temperature of propan-1-ol, C₃H₇OH, given that its vapour pressure is 2701 Pa at 298 K and 9129 Pa at 318 K.

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

Calculate the change in the chemical potential of a perfect gas when its partial pressure doubles at a temperature of 200°C.

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Question 3

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The molar entropy of 1,3-dioxane, C₄H₈O₂, is 196.6 J K^-1 mol^-1. What is the change in the molar Gibbs energy of 1,3-dioxane when it is heated from 298 K to 323 K?

(Multiple Choice)

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Question 4

At a temperature of 214 K, carbon disulfide, CS₂, and acetone, CH₃COCH₃, are not fully miscible and, instead, form separate liquid phases with mole fractions of carbon disulfide of 0.403 and 0.833. Use the lever rule to calculate the relative amounts of the two phases when 10.0 g of carbon disulfide and 10.0 g of acetone are mixed together at this temperature.

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Question 5

What partial pressure of hydrogen, H₂, is required above an aqueous solution in order to ensure that the concentration of hydrogen in the solution is 1.00 mmol dm^-3? The Henry's law constant for hydrogen is 7.78 10^-3 mol m^-3kPa^-1.

(Multiple Choice)

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Question 6

The normal boiling temperature of liquid bromine, Br₂, is 332 K and the standard enthalpy of vaporization is 29.45 kJ mol^-1. Use the Clausius-Clapeyron equation to determine the vapour pressure of liquid bromine at a temperature of 298 K.

(Multiple Choice)

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Question 7

The molar Gibbs energy of tribromomethane, CHBr₃, decreases by 4.44 kJ mol^-1 when the temperature is increased from 288 to 308 K. Determine the molar entropy of tribromomethane.

(Multiple Choice)

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Question 8

Estimate the change in the normal boiling temperature of an aqueous solution made by dissolving 12.6 g of phenol, C₆H₅OH, in 250 cm³ of water. The ebullioscopic constant of water is 0.51 K kg mol^-1.

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Question 9

The Henry's law constant for pentan-3-one, C₂H₅COC₂H₅, in aqueous solution may be expressed in terms of concentration as 19.6 mol dm^-³ kPa^-1. Calculate the vapour pressure of pentan-3-one above an aqueous solution that contains 5.23 g of pentan-3-one in 250 cm³ of solution.

(Multiple Choice)

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Question 10

The densities of white and red phosphorus are 1.823 and 2.340 g cm^-3 respectively. Calculate the change in the molar volume for the transformation of white into red phosphorus.

(Multiple Choice)

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Question 11

The vapour pressure p of liquid diethyl ether, (C₂H₅)₂O, may be calculated for different temperatures T using the expression Log (p/bar)=A-B/T Where, for the temperature range 24 to 48 °C, A = 4.743 and B = 1466.30 K. What is the vapour pressure of liquid diethyl ether at 25 °C?

(Multiple Choice)

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Question 12

An ideal solution is prepared by mixing 15.6 g of toluene, C₆H₅CH₃, and 136.2 g of butan-1-ol, C₄H₉OH at 25 °C. The vapour pressure of pure butan-1-ol is 885 Pa at this temperature. Calculate the partial pressure of butan-1-ol in the vapour above the mixture.

(Multiple Choice)

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Question 13

Determine the molar Gibbs energy of mixing for the formation of an equimolar mixture of two perfect gases at a temperature of 298 K.

(Multiple Choice)

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Question 14

The normal boiling temperature of benzene, C₆H₆, is 353.3 K, whilst the triple point occurs at a temperature of 278.5 K and pressure of 4813 Pa. Determine the average value for the enthalpy of vaporization of benzene over this range.

(Multiple Choice)

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Question 15

Calculate the mass of sodium chloride, NaCl, required to lower the freezing temperature of ice by 0.50 K. The cryoscopic constant of water is 1.86 K kgmol^-1.

(Multiple Choice)

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Question 16

For the equilibrium CaCO₃(s) ∏ CaO(s) + CO₂(g) How many phases are present?

(Multiple Choice)

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Question 17

Use the following data for the osmotic pressures of solutions of different mass concentrations of an enzyme in water at 298 K to determine the molar mass of the enzyme. / 2.00 4.00 6.00 8.00 10.0 \Pi/ 46 124 236 380 558

(Multiple Choice)

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Question 18

Calculate the change in the molar Gibbs energy of a perfect gas when it expands isothermally at a temperature of 25 °C from a molar volume of 1.00 dm³ to a molar volume of 10.0 dm³.

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Question 19

The density of liquid carbon disulfide, CS₂, is 1293 kg m^-3. Calculate the change in the molar Gibbs energy of carbon disulfide when it is compressed by a change in pressure from 1.00 bar to 2.00 bar.

(Multiple Choice)

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Question 20

Showing 1 - 20 of 20

Estimate the normal boiling temperature of propan-1-ol, C₃H₇OH, given that its vapour pressure is 2701 Pa at 298 K and 9129 Pa at 318 K.

Calculate the change in the chemical potential of a perfect gas when its partial pressure doubles at a temperature of 200°C.

The molar entropy of 1,3-dioxane, C₄H₈O₂, is 196.6 J K^-1 mol^-1. What is the change in the molar Gibbs energy of 1,3-dioxane when it is heated from 298 K to 323 K?

What partial pressure of hydrogen, H₂, is required above an aqueous solution in order to ensure that the concentration of hydrogen in the solution is 1.00 mmol dm^-3? The Henry's law constant for hydrogen is 7.78 10^-3 mol m^-3kPa^-1.

The normal boiling temperature of liquid bromine, Br₂, is 332 K and the standard enthalpy of vaporization is 29.45 kJ mol^-1. Use the Clausius-Clapeyron equation to determine the vapour pressure of liquid bromine at a temperature of 298 K.

The molar Gibbs energy of tribromomethane, CHBr₃, decreases by 4.44 kJ mol^-1 when the temperature is increased from 288 to 308 K. Determine the molar entropy of tribromomethane.

Estimate the change in the normal boiling temperature of an aqueous solution made by dissolving 12.6 g of phenol, C₆H₅OH, in 250 cm³ of water. The ebullioscopic constant of water is 0.51 K kg mol^-1.

The Henry's law constant for pentan-3-one, C₂H₅COC₂H₅, in aqueous solution may be expressed in terms of concentration as 19.6 mol dm^-³ kPa^-1. Calculate the vapour pressure of pentan-3-one above an aqueous solution that contains 5.23 g of pentan-3-one in 250 cm³ of solution.

The densities of white and red phosphorus are 1.823 and 2.340 g cm^-3 respectively. Calculate the change in the molar volume for the transformation of white into red phosphorus.

The vapour pressure p of liquid diethyl ether, (C₂H₅)₂O, may be calculated for different temperatures T using the expression Log (p/bar)=A-B/T Where, for the temperature range 24 to 48 °C, A = 4.743 and B = 1466.30 K. What is the vapour pressure of liquid diethyl ether at 25 °C?

An ideal solution is prepared by mixing 15.6 g of toluene, C₆H₅CH₃, and 136.2 g of butan-1-ol, C₄H₉OH at 25 °C. The vapour pressure of pure butan-1-ol is 885 Pa at this temperature. Calculate the partial pressure of butan-1-ol in the vapour above the mixture.

Determine the molar Gibbs energy of mixing for the formation of an equimolar mixture of two perfect gases at a temperature of 298 K.

The normal boiling temperature of benzene, C₆H₆, is 353.3 K, whilst the triple point occurs at a temperature of 278.5 K and pressure of 4813 Pa. Determine the average value for the enthalpy of vaporization of benzene over this range.

Calculate the mass of sodium chloride, NaCl, required to lower the freezing temperature of ice by 0.50 K. The cryoscopic constant of water is 1.86 K kgmol^-1.

For the equilibrium CaCO₃(s) ∏ CaO(s) + CO₂(g) How many phases are present?

Use the following data for the osmotic pressures of solutions of different mass concentrations of an enzyme in water at 298 K to determine the molar mass of the enzyme. / 2.00 4.00 6.00 8.00 10.0 \Pi/ 46 124 236 380 558

Calculate the change in the molar Gibbs energy of a perfect gas when it expands isothermally at a temperature of 25 °C from a molar volume of 1.00 dm³ to a molar volume of 10.0 dm³.

The density of liquid carbon disulfide, CS₂, is 1293 kg m^-3. Calculate the change in the molar Gibbs energy of carbon disulfide when it is compressed by a change in pressure from 1.00 bar to 2.00 bar.

The Propertiesof Gases

The First Law of Thermodynamics

The Second Law of Thermodynamics

Chemical Change

Chemical Kinetics

Quantum Theory

Atomic Structure

The Chemical Bond

Molecular Interactions

Molecular Spectroscopy

Statistical Thermodynamics

Filters

Exam 4: Physical Transformations

Estimate the normal boiling temperature of propan-1-ol, C3H7OH, given that its vapour pressure is 2701 Pa at 298 K and 9129 Pa at 318 K.

Calculate the change in the chemical potential of a perfect gas when its partial pressure doubles at a temperature of 200°C.

The molar entropy of 1,3-dioxane, C4H8O2, is 196.6 J K-1 mol-1. What is the change in the molar Gibbs energy of 1,3-dioxane when it is heated from 298 K to 323 K?

What partial pressure of hydrogen, H2, is required above an aqueous solution in order to ensure that the concentration of hydrogen in the solution is 1.00 mmol dm-3? The Henry's law constant for hydrogen is 7.78 10-3 mol m-3 kPa-1.

The normal boiling temperature of liquid bromine, Br2, is 332 K and the standard enthalpy of vaporization is 29.45 kJ mol-1. Use the Clausius-Clapeyron equation to determine the vapour pressure of liquid bromine at a temperature of 298 K.

The molar Gibbs energy of tribromomethane, CHBr3, decreases by 4.44 kJ mol-1 when the temperature is increased from 288 to 308 K. Determine the molar entropy of tribromomethane.

Estimate the change in the normal boiling temperature of an aqueous solution made by dissolving 12.6 g of phenol, C6H5OH, in 250 cm3 of water. The ebullioscopic constant of water is 0.51 K kg mol-1.

The Henry's law constant for pentan-3-one, C2H5COC2H5, in aqueous solution may be expressed in terms of concentration as 19.6 mol dm-3 kPa-1. Calculate the vapour pressure of pentan-3-one above an aqueous solution that contains 5.23 g of pentan-3-one in 250 cm3 of solution.

The densities of white and red phosphorus are 1.823 and 2.340 g cm-3 respectively. Calculate the change in the molar volume for the transformation of white into red phosphorus.

The vapour pressure p of liquid diethyl ether, (C2H5)2O, may be calculated for different temperatures T using the expression Log (p/bar)=A-B/T Where, for the temperature range 24 to 48 °C, A = 4.743 and B = 1466.30 K. What is the vapour pressure of liquid diethyl ether at 25 °C?

An ideal solution is prepared by mixing 15.6 g of toluene, C6H5CH3, and 136.2 g of butan-1-ol, C4H9OH at 25 °C. The vapour pressure of pure butan-1-ol is 885 Pa at this temperature. Calculate the partial pressure of butan-1-ol in the vapour above the mixture.

Determine the molar Gibbs energy of mixing for the formation of an equimolar mixture of two perfect gases at a temperature of 298 K.

The normal boiling temperature of benzene, C6H6, is 353.3 K, whilst the triple point occurs at a temperature of 278.5 K and pressure of 4813 Pa. Determine the average value for the enthalpy of vaporization of benzene over this range.

Calculate the mass of sodium chloride, NaCl, required to lower the freezing temperature of ice by 0.50 K. The cryoscopic constant of water is 1.86 K kg mol-1.

For the equilibrium CaCO3(s) ∏ CaO(s) + CO2(g) How many phases are present?

Use the following data for the osmotic pressures of solutions of different mass concentrations of an enzyme in water at 298 K to determine the molar mass of the enzyme. / 2.00 4.00 6.00 8.00 10.0 \Pi/ 46 124 236 380 558

Calculate the change in the molar Gibbs energy of a perfect gas when it expands isothermally at a temperature of 25 °C from a molar volume of 1.00 dm3 to a molar volume of 10.0 dm3.

The density of liquid carbon disulfide, CS2, is 1293 kg m-3. Calculate the change in the molar Gibbs energy of carbon disulfide when it is compressed by a change in pressure from 1.00 bar to 2.00 bar.

The Propertiesof Gases

The First Law of Thermodynamics

The Second Law of Thermodynamics

Chemical Change

Chemical Kinetics

Quantum Theory

Atomic Structure

The Chemical Bond

Molecular Interactions

Molecular Spectroscopy

Statistical Thermodynamics

Filters

Estimate the normal boiling temperature of propan-1-ol, C₃H₇OH, given that its vapour pressure is 2701 Pa at 298 K and 9129 Pa at 318 K.

The molar entropy of 1,3-dioxane, C₄H₈O₂, is 196.6 J K^-1 mol^-1. What is the change in the molar Gibbs energy of 1,3-dioxane when it is heated from 298 K to 323 K?

What partial pressure of hydrogen, H₂, is required above an aqueous solution in order to ensure that the concentration of hydrogen in the solution is 1.00 mmol dm^-3? The Henry's law constant for hydrogen is 7.78 10^-3 mol m^-3kPa^-1.

The normal boiling temperature of liquid bromine, Br₂, is 332 K and the standard enthalpy of vaporization is 29.45 kJ mol^-1. Use the Clausius-Clapeyron equation to determine the vapour pressure of liquid bromine at a temperature of 298 K.

The molar Gibbs energy of tribromomethane, CHBr₃, decreases by 4.44 kJ mol^-1 when the temperature is increased from 288 to 308 K. Determine the molar entropy of tribromomethane.

Estimate the change in the normal boiling temperature of an aqueous solution made by dissolving 12.6 g of phenol, C₆H₅OH, in 250 cm³ of water. The ebullioscopic constant of water is 0.51 K kg mol^-1.

The Henry's law constant for pentan-3-one, C₂H₅COC₂H₅, in aqueous solution may be expressed in terms of concentration as 19.6 mol dm^-³ kPa^-1. Calculate the vapour pressure of pentan-3-one above an aqueous solution that contains 5.23 g of pentan-3-one in 250 cm³ of solution.

The densities of white and red phosphorus are 1.823 and 2.340 g cm^-3 respectively. Calculate the change in the molar volume for the transformation of white into red phosphorus.

The vapour pressure p of liquid diethyl ether, (C₂H₅)₂O, may be calculated for different temperatures T using the expression Log (p/bar)=A-B/T Where, for the temperature range 24 to 48 °C, A = 4.743 and B = 1466.30 K. What is the vapour pressure of liquid diethyl ether at 25 °C?

An ideal solution is prepared by mixing 15.6 g of toluene, C₆H₅CH₃, and 136.2 g of butan-1-ol, C₄H₉OH at 25 °C. The vapour pressure of pure butan-1-ol is 885 Pa at this temperature. Calculate the partial pressure of butan-1-ol in the vapour above the mixture.

The normal boiling temperature of benzene, C₆H₆, is 353.3 K, whilst the triple point occurs at a temperature of 278.5 K and pressure of 4813 Pa. Determine the average value for the enthalpy of vaporization of benzene over this range.

Calculate the mass of sodium chloride, NaCl, required to lower the freezing temperature of ice by 0.50 K. The cryoscopic constant of water is 1.86 K kgmol^-1.

For the equilibrium CaCO₃(s) ∏ CaO(s) + CO₂(g) How many phases are present?

Calculate the change in the molar Gibbs energy of a perfect gas when it expands isothermally at a temperature of 25 °C from a molar volume of 1.00 dm³ to a molar volume of 10.0 dm³.

The density of liquid carbon disulfide, CS₂, is 1293 kg m^-3. Calculate the change in the molar Gibbs energy of carbon disulfide when it is compressed by a change in pressure from 1.00 bar to 2.00 bar.