Chemical Principles
8th Edition
ISBN: 9781337247269
Author: Steven S. Zumdahl; Donald J. DeCoste
Publisher: Cengage Learning US
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Chapter 9, Problem 117CP
Interpretation Introduction
Interpretation: The molar enthalpy of fusion for ice at 1 atm and 0.0 oC needs to be calculated.
Concept Introduction: Change in enthalpy is calculated using the following equation:
Where n represents number of moles, Cp is molar specific heat capacity and
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Sulfur dioxide is produced in enormous amounts for sulfuric acid production. It melts at −73.0°C and boils at −10.0°C. Its ΔHfus is 8.619 kJ/mol, and its ΔHvap is 25.73 kJ/mol. The specific heat capacities of the liquid and gas are 0.995 J/g·K and 0.622 J/g·K, respectively. How much heat is required to convert 5.000 kg of solid SO2 at the melting point to a gas at 60.0 degrees C?
Answer should be in J.
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 0.450 kg of water
decreased from 103 °C to 42.0 °C. NOTE: MOLAR specfic heat capacities (Cp,n) are given here!
Property
Value
Units
Melting point
°C
Boiling point
100.0
°C
ΔΗus
6.01
kJ/mol
ΔΗap
40.67
kJ/mol
o (s)
37.1
J/mol · °C
75.3
J/mol · °C
33.6
J/mol · °C
kJ
For water, ΔHfusion = 6.02 kJ/mol and ΔHvap = 40.65 kJ/mol. If 0.250 moles of water vaporizes at 100 oC due to heat from the surroundings that are at 135 oC, what is the change in entropy in the surroundings?
Chapter 9 Solutions
Chemical Principles
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