The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ/mol. What is the ΔH at 373 K given the following values of the molar heat capacities at constant pressure? H2O(g) = 33.58 J K-1 mol-1; H2(g) = 29.84 J K-1 mol-1; O2(g) = 29.37 J K-1 mol-1 H2(g) + ½ O2(g) → H2O(g)
The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ/mol. What is the ΔH at 373 K given the following values of the molar heat capacities at constant pressure? H2O(g) = 33.58 J K-1 mol-1; H2(g) = 29.84 J K-1 mol-1; O2(g) = 29.37 J K-1 mol-1 H2(g) + ½ O2(g) → H2O(g)
Physical Chemistry
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Chapter2: The First Law Of Thermodynamics
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Problem 2.79E: The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C...
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The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ/mol. What is the ΔH at 373 K given the following values of the molar heat capacities at constant pressure?
H2O(g) = 33.58 J K-1 mol-1; H2(g) = 29.84 J K-1 mol-1; O2(g) = 29.37 J K-1 mol-1
H2(g) + ½ O2(g) → H2O(g)
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