The enthalpy of formation of water vapor is −241.8 kJ/mol. The standard enthalpy of formation of liquid water is −285.8 kJ/mol. When water vapor condenses to liquid water, the decrease in entropy is about 105 J/K·mol, which more than compensates for the increase in enthalpy. As a result, the net amount of energy released when one mole of liquid water is produced from water vapor is about −241.8 kJ/mol.
Other related questions:
Q: How much energy is released during the formation of one mole of h2o G?
A: The answer to this question depends on the specific heat of water.
Q: How much energy is absorbed or released when 1 mole of product is produced?
A: The answer to this question depends on the specific reaction in question. For example, if the reaction is exothermic (releases energy), then the amount of energy released will be greater than the amount of energy required to break the bonds of the reactants. Conversely, if the reaction is endothermic ( absorbs energy), then the amount of energy required to break the bonds of the reactants will be greater than the amount of energy released.
Q: How much energy in kJ is released per mole of o2 consumed?
A: The energy released per mole of oxygen consumed is approximately 574 kJ.
Q: How much energy is released when 2 moles of co2 are formed?
A: When 2 moles of carbon dioxide are formed, 44.0 kJ of energy are released.