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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

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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.

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.

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.)

1. The vapor pressure of a substance is measured over a range of temperatures. A plot of the natural log of the vapor pressure versus the inverse of the temperature (in Kelvin) produces a straight line with a slope of −3.54×103 K . Find the enthalpy of vaporization of the substance. Express your answer using three significant figures.

2. Determine the amount of heat (in kJ) required to vaporize 1.00 kg of water at its boiling point. For water, ΔHvap = 40.7 kJ/mol (at 100 ∘C). Express your answer to three significant figures and include the appropriate units.

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