The energy required to vaporize 48.7 g of dichloromethane at its boiling point: 18.3 kJ
<h3>Further explanation</h3>
Enthalpy is the amount of system heat at constant pressure.
The enthalpy is symbolized by H, while the change in enthalpy is the difference between the final enthalpy and the initial enthalpy symbolized by ΔH.
Delta H reaction (ΔH) is the amount of heat change between the system and its environment
(ΔH) can be positive (endothermic = requires heat) or negative (exothermic = releasing heat)
The standard unit is kilojoules (kJ)
The enthalpy change symbol (ΔH) is usually written behind the reaction equation.
Change in Standard Evaporation Enthalpy (ΔH vap) is a change in enthalpy at the evaporation of 1 mol liquid phase to the gas phase at its boiling point and standard pressure.
Examples of water evaporation:
H₂O (l) ---> H₂O (g); ΔH vap = + 44kJ
The enthalpy of evaporation is positive because its energy is needed to break the attraction between molecules in a liquid
48.7 g of dichloromethane
relative molecular mass of dichloromethane (CH₂Cl₂) = 1.12 + 2.1 + 2.35.5= 84 gram / mol
mole = 0.579
Since the heat of vaporization for dichloromethane is 31.6 kj/mol ,the energy needed to evaporate 0.580 moles of dichloromethane is:
31.6 kJ / mol x 0.579 mol = 18.3 kJ
<h3>Learn more</h3>
the heat of vaporization
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The latent heat of vaporization
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Keywords: the heat of vaporization, dichloromethane, mole, gram, exothermic, endothermic