C. 1. The enthalpy of vaporization, (symbol ... On the other hand, the molecules in liquid water are held together by relatively strong hydrogen bonds, and its enthalpy of vaporization, 40.65 kJ/mol, is more than five times the energy required to heat the same quantity of water from 0 °C to 100 °C (c p = 75.3 J K −1 mol −1). If enthalpy of vaporisation of water is 1 8 6. 5. The enthalpy of vaporization, (symbol Δ v H), also known as the heat of vaporization or heat of evaporation, is the energy required to transform a given quantity of a substance into a gas.It is measured at the normal boiling point of the substance, although tabulated values are usually corrected to 298 K: the correction is small, and is often smaller than the uncertainty in the measured value. 0. The enthalpy of vaporization, (symbol ∆H vap) also known as the (latent) heat of vaporization or heat of evaporation, is the enthalpy change required to transform a given quantity of a substance from a liquid into a gas at a given pressure (often atmospheric pressure, as in STP).. 5 k J / m o l, the entropy of its vaporisation will be: A. November 22, 2019 Vinithagupta Shahdadpuri. Answer. The experiment was conducted with tap water, and not distilled water, and as such the actual enthalpy of vaporization might be higher than the enthalpy of vaporization of water (due to the presence of other compounds that increase the intermolecular attractions of the water). D. 2. On the other hand, the molecules in liquid water are held together by relatively strong hydrogen bonds, and its enthalpy of vaporization, 40.65 kJ/mol, is more than five times the energy required to heat the same quantity of water from 0 °C to 100 °C (c p = 75.3 J K − 1 mol − 1). The enthalpy of vaporization, in kJ/mol, of water 20.4 kJ Heat needed to vaporize 0.500 moles of H 2 O can be determined by using following steps: First step is to define the enthalpy of vaporization; Enthalpy of vaporization (ΔH vap) is the amount of heat added to … 5. 0.
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