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The molar enthalpy of vaporization of water at 373 K and 1.00 atm is 40.7 kJ/mol. What fraction of this energy is used to change the internal energy of the water, and what fraction is used to do work against the atmosphere? (Hint: Assume that water vapor is an ideal gas.)

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Patrick Suarez
Patrick SuarezLv10
26 Nov 2020

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Related questions

1.00 kg of water at 293 K is heated at a constant pressure of 1.00 atm until it completely evaporates. The heat capacity of water is 1.00 cal/(g*K). The molar enthalpy of vaporization is ΔHvapM = 40.7 kJ/mol. You may treat H2O vapor as an ideal gas.

What are ΔH, ΔU, q, and w for this process?

1 kcal = 4.1868 kJ

1.00 kg of water at 293 K is heated at a constant pressure of 1.00 atm until it completely evaporates. The heat capacity of water is 1.00 cal/(g*K). The molar enthalpy of vaporization is ΔHvapM = 40.7 kJ/mol.

You may treat H2O vapor as an ideal gas.

1 kcal = 4.1868 kJ

What are

a) ΔH in kJ

b) ΔU in kJ

c) q in kJ

d) w for this process?

Please explain each steps.

9. The normal boiling point of methanol is 64.7⁰C and the molar enthalpy of vaporization if 71.8kJ/mol. The value of ΔS when 1.95 mol of CH3OH(l) vaporizes at 64.7⁰C is

________ J/K

[A] 414 [B] 0.414 [C] 2.16 [D] 4.73 [E] 2.16

10. The normal boiling point of water is 100.0 °C and its molar enthalpy of vaporization is 40.67 kJ/mol. What is the change in entropy in the system in J/K when 22.1 grams of steam at 1 atm condenses to a liquid at the normal boiling point?

[A] -88.8 [B] -40.7 [C] 88.8 [D] 373 [E] -134

11. The normal boiling point of C2Cl3F3 is 47.6 °C and its molar enthalpy of vaporization is 27.49 kJ/mol. What is the change in entropy in the system in J/K when 20.2 grams of C2Cl3F3 vaporizes to a gas at the normal boiling point?

[A] 27.5 [B] -4.19 [C] 4.19 [D] 9.23 [E] -9.23

12. The thermodynamic quantity that expresses the extent of randomness in a system is __

[A] entropy [B] enthalpy [C] bond energy [D] heat flow [E] internal energy

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