How much heat energy is required to convert 62.8 g of liquid sulfur dioxide, SO2, at...
How much heat energy is required to convert 62.8 g of liquid sulfur dioxide, SO2, at 219.4 K to gaseous SO2 at 263.1 K if the molar heat of vaporization of SO2 is 24.9 kJ/mol, and the specific heat capacity (C) of liquid SO2 is 1.36 J/(g ·°C)?
Homework Answers
Supposing the boiling point of SO2 to be 263.1 K:
(1.36 J/(g ·°C)) x (62.8 g) x (263.1 K - 219.4 K) = 3578.59 J to
warm the liquid to its boiling point
(62.8 g SO2) / (64.0638 g SO2/mol) x (24.9 kJ/mol) = 24.41 kJ =
24410 J to vaporize the liquid
3578.59 J + 24410 J = 27988.59 J = 27.988 kJ Answer
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