Liquid water is vaporized at its normal boiling point (1 bar, 373K) where the heat of vaporization is 40.7 kJ/mol. Calculate won,âE,âH, q_p and âS. Next, what is âSenvironment?

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The human body obtains 1088 kJ from a candy bar. Part A If this energy were used to vaporize water at 100 âC, how much water in liters could be vaporized? (Assume that the density of water is 1.0 g/mL.) The heat of vaporization of water at 100 âC is 40.7 kJ/mole. Express your answer using two significant figures.

The following information is given for water, H₂O, at 1atm:

boiling point = 100 Â°C	deltaH_vap(100 Â°C) = 40.7 kJ/mol
specific heat liquid = 4.18 J/gÂ°C

At a pressure of 1 atm, what is deltaH in kJ for the process of condensing a 28.6 g sample of gaseous water at its normal boiling point of 100Â°C.

`Calculate the amount of water (M.W. = 18.02 g/mol) at its boiling point that would be vaporized by 180 Calories (note the capital C). The heat of fusion for water at its boiling point is 40.7 kJ/mol, and 1 calorie = 4.184 J. You must show all work in detail to receive credit.

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Liquid water is vaporized at its normal boiling point (1 bar, 373K) where the heat of vaporization is 40.7 kJ/mol. Calculate won,âE,âH, q_p and âS. Next, what is âSenvironment?

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Liquid water is vaporized at its normal boiling point (1 bar, 373K) where the heat of vaporization is 40.7 kJ/mol. Calculate won,âE,âH, q_p and âS. Next, what is âSenvironment?

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

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Liquid water is vaporized at its normal boiling point (1 bar, 373K) where the heat of vaporization is 40.7 kJ/mol. Calculate won,âE,âH, q_p and âS. Next, what is âSenvironment?