Find ΔUΔU for the change in state of 1.0 molH2O(l) at 80 ∘C to H2O(g) at 112∘C. The molar heat capacity of H2O(l) = 75.3 Jmol−1K-1, molar heat capacity of H2O(g) = 25.0 Jmol−1K−1, and the heat of vaporization of H2O is 40.7×103Jmol−1 at 100 ∘C. b) Find ΔHΔH for the change in state of 1.0 molH2O(l)molH2O(l) at 80 ∘C to H2O(g)H2O(g) at 112 ∘C. c)Find q for the change in state of 1.0
Find ΔUΔU for the change in state of 1.0 molH2O(l) at 80 ∘C to H2O(g) at 112∘C. The molar heat capacity of H2O(l) = 75.3 Jmol−1K-1, molar heat capacity of H2O(g) = 25.0 Jmol−1K−1, and the heat of vaporization of H2O is 40.7×103Jmol−1 at 100 ∘C. b) Find ΔHΔH for the change in state of 1.0 molH2O(l)molH2O(l) at 80 ∘C to H2O(g)H2O(g) at 112 ∘C. c)Find q for the change in state of 1.0
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.51QE: The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol...
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a) Find ΔUΔU for the change in state of 1.0 molH2O(l) at 80 ∘C to H2O(g) at 112∘C. The molar heat capacity of H2O(l) = 75.3 Jmol−1K-1, molar heat capacity of H2O(g) = 25.0 Jmol−1K−1, and the heat of vaporization of H2O is 40.7×103Jmol−1 at 100 ∘C.
b) Find ΔHΔH for the change in state of 1.0 molH2O(l)molH2O(l) at 80 ∘C to H2O(g)H2O(g) at 112 ∘C.
c)Find q for the change in state of 1.0 molH2O(l)molH2O(l) at 80 ∘C to H2O(g)H2O(g) at 112 ∘C
d)Find w for the change in state of 1.0 molH2O(l)molH2O(l) at 80 ∘C∘C to H2O(g)H2O(g) at 112 ∘C∘C.
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