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champagnetermite204Lv1

28 Sep 2019

How much energy (in kilojoules) is released when 16.8 g of steam at 123.0 âC is condensed to give liquid water at 73.0 âC? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(Kâ mol) for the liquid and 33.6 J/(Kâ mol) for the vapor.

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Keith LeannonLv2

28 Sep 2019

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Calculate change in heat when 18.80 g of water vapor steam at 100 C condenses to liquid water and then cools to 20.5. the molar heat capacity of water is 75.3 J/ (mol x C). Delta Hvap= 40.67 KJ/mol. Express answer using 4 significant figures. Also, should your answer be positive or negative?

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How much energy (in kilojoules) is released when 16.8 g of steam at 123.0 âC is condensed to give liquid water at 73.0 âC? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(Kâ mol) for the liquid and 33.6 J/(Kâ mol) for the vapor.

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How much energy (in kilojoules) is released when 16.8 g of steam at 123.0 âC is condensed to give liquid water at 73.0 âC? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(Kâ mol) for the liquid and 33.6 J/(Kâ mol) for the vapor.

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

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How much energy (in kilojoules) is released when 16.8 g of steam at 123.0 âC is condensed to give liquid water at 73.0 âC? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(Kâ mol) for the liquid and 33.6 J/(Kâ mol) for the vapor.