Question 1

The standard entropy of diamond is 2.4 J/mol · K. Calculate the entropy per carbon atom in diamond and the number of microstates for each atom. Discuss the number of microstates in terms of the molecular motions accessible to each carbon atom.

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Question 2

The standard molar enthalpy of fusion for xenon is 2.30 kJ mol^-¹. Calculate the standard molar entropy for the freezing of liquid xenon given that its normal freezing point is -112°C.

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Question 3

The standard entropy of N₂(g) is 191.5 J/mol · K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

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Question 4

The entropy of fusion for ice at 0°C and 1 atm is 22 J/mol · K. How many joules of heat are required to melt a typical ice cube at 0°C and 1 atm? Assume an ice cube is about 1 oz or 28
g.

Accepted Answer

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Question 5

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

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Question 6

What is a microstate and how are microstates quantitatively related to entropy?

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Question 7

Determine the normal melting point of benzoic acid in degrees centigrade given the following data.
$\Delta$ H  = 18.02 kJ/mol
$\Delta$ S  = 45.56 J/mol · K

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Question 8

Carbon monoxide has a very weak dipole moment. In the formation of solid carbon monoxide some molecules will be reversed in their orientation from C  O - - - C  O to C  O - - - O  C. What do you expect the absolute entropy of carbon monoxide solid to be at 0 K, and why?

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Question 9

Carbon atoms can be found in a variety of elemental forms. At sufficiently high temperature, carbon is an atomic gas. At room temperature, both tetrahedral networks in diamond and trigonal planar networks in graphite can be found. Trigonal planar networks of carbon atoms are also found in Buckminsterfullerene (C₆₀). How does the standard entropy of these forms vary per mole of carbon?

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Question 10

The change in standard molar entropy, $\Delta$S$\degree$ for the following reaction is 494.6 J/mol · K at 25$\degree$C. 2KClO₃(s) $\rightleftarrows$ 2KCl(s) + 3O₂(g) What is the standard molar entropy of O₂(g) at 25$\degree$C? S°(KClO₃, s)= 143.1 J/mol · K S°(KCl, s)= 82.6 J/mol · K

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Question 11

Only one substance has a standard entropy of 0 J/K, and that is H⁺(aq). Why is this so?

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Question 12

Considering the tabulated values for the thermodynamic properties of oxygen gas, why is the standard entropy nonzero but the standard enthalpy and free energy of formation are zero?

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Question 13

What are the signs of $\Delta$H°, $\Delta$S°, and $\Delta$G° for the conversion of liquid water to ice at 10°C and 1 atm? Briefly explain each answer.

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Question 14

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

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Question 15

Give an example of a spontaneous and a nonspontaneous chemical process and the sign of the entropy change for the universe for each.

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Question 16

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at -5°C? Comment on the sign.

Accepted Answer

The answer of The heat of fusion for water is...

Question 17

What is the overall standard free-energy change for the following two reactions in terms of $\Delta$G₁and $\Delta$G₂? A + B $\rightarrow$ 2C $\Delta$G = $\Delta$G₁ C + D $\rightarrow$ E $\Delta$G = $\Delta$G₂

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Question 18

Hydrogen iodide can theoretically be made by the reaction of hydrogen gas and iodine by the following reaction. H₂(g) + I₂(s)$\rightarrow$2HI(g) What temperature conditions are required for the formation of HI to be favored at standard pressure? S°(H₂, g) = 130.6 J/mol · K S°(I₂, s) = 116.1 J/mol · K S°(HI, g) = 206.6 J/mol · K $\Delta$ H (HI, g) = 26.5 kJ/mol · K

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Question 19

Name and state the first three laws of thermodynamics.

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Quiz 14: Thermodynamics: Spontaneous Processes, Entropy, and Free Energy

The standard entropy of diamond is 2.4 J/mol · K. Calculate the entropy per carbon atom in diamond and the number of microstates for each atom. Discuss the number of microstates in terms of the molecular motions accessible to each carbon atom.

The standard molar enthalpy of fusion for xenon is 2.30 kJ mol^-¹. Calculate the standard molar entropy for the freezing of liquid xenon given that its normal freezing point is -112°C.

The standard entropy of N₂(g) is 191.5 J/mol · K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

The entropy of fusion for ice at 0°C and 1 atm is 22 J/mol · K. How many joules of heat are required to melt a typical ice cube at 0°C and 1 atm? Assume an ice cube is about 1 oz or 28 g.

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

What is a microstate and how are microstates quantitatively related to entropy?

Carbon monoxide has a very weak dipole moment. In the formation of solid carbon monoxide some molecules will be reversed in their orientation from C O - - - C O to C O - - - O C. What do you expect the absolute entropy of carbon monoxide solid to be at 0 K, and why?

Only one substance has a standard entropy of 0 J/K, and that is H⁺(aq). Why is this so?

Considering the tabulated values for the thermodynamic properties of oxygen gas, why is the standard entropy nonzero but the standard enthalpy and free energy of formation are zero?

What are the signs of $\Delta$ H°, $\Delta$ S°, and $\Delta$ G° for the conversion of liquid water to ice at 10°C and 1 atm? Briefly explain each answer.

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

Give an example of a spontaneous and a nonspontaneous chemical process and the sign of the entropy change for the universe for each.

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at -5°C? Comment on the sign.

Name and state the first three laws of thermodynamics.

Quiz 14: Thermodynamics: Spontaneous Processes, Entropy, and Free Energy

The standard entropy of diamond is 2.4 J/mol · K. Calculate the entropy per carbon atom in diamond and the number of microstates for each atom. Discuss the number of microstates in terms of the molecular motions accessible to each carbon atom.

The standard molar enthalpy of fusion for xenon is 2.30 kJ mol-1. Calculate the standard molar entropy for the freezing of liquid xenon given that its normal freezing point is -112°C.

The standard entropy of N2(g) is 191.5 J/mol · K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

The entropy of fusion for ice at 0°C and 1 atm is 22 J/mol · K. How many joules of heat are required to melt a typical ice cube at 0°C and 1 atm? Assume an ice cube is about 1 oz or 28 g.

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

What is a microstate and how are microstates quantitatively related to entropy?

Determine the normal melting point of benzoic acid in degrees centigrade given the following data. Δ\DeltaΔ H = 18.02 kJ/mol Δ\DeltaΔ S = 45.56 J/mol · K

Carbon monoxide has a very weak dipole moment. In the formation of solid carbon monoxide some molecules will be reversed in their orientation from C O - - - C O to C O - - - O C. What do you expect the absolute entropy of carbon monoxide solid to be at 0 K, and why?

Only one substance has a standard entropy of 0 J/K, and that is H+(aq). Why is this so?

Considering the tabulated values for the thermodynamic properties of oxygen gas, why is the standard entropy nonzero but the standard enthalpy and free energy of formation are zero?

What are the signs of Δ\DeltaΔ H°, Δ\DeltaΔ S°, and Δ\DeltaΔ G° for the conversion of liquid water to ice at 10°C and 1 atm? Briefly explain each answer.

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

Give an example of a spontaneous and a nonspontaneous chemical process and the sign of the entropy change for the universe for each.

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at -5°C? Comment on the sign.

What is the overall standard free-energy change for the following two reactions in terms of Δ\DeltaΔ G1 and Δ\DeltaΔ G2? A + B →\rightarrow→ 2C Δ\DeltaΔ G = Δ\DeltaΔ G1 C + D →\rightarrow→ E Δ\DeltaΔ G = Δ\DeltaΔ G2

Name and state the first three laws of thermodynamics.

The standard molar enthalpy of fusion for xenon is 2.30 kJ mol^-¹. Calculate the standard molar entropy for the freezing of liquid xenon given that its normal freezing point is -112°C.

The standard entropy of N₂(g) is 191.5 J/mol · K. Calculate the entropy per nitrogen molecule and the number of microstates for each molecule. Discuss the number of microstates in terms of the molecular motions accessible to each molecule.

Only one substance has a standard entropy of 0 J/K, and that is H⁺(aq). Why is this so?

What are the signs of $\Delta$ H°, $\Delta$ S°, and $\Delta$ G° for the conversion of liquid water to ice at 10°C and 1 atm? Briefly explain each answer.