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Heat of Vaporization and Heat of Fusion Learning Goal: To calculate the total energy required to convert a solid to agas using heat capacity, heat of fusion, and heat ofvaporization. The amount of heat required to melt one mole of a solid is calledthe heat of fusion (ΔHfus). The amount of heatrequired to vaporize (boil) one mole of a liquid is called theheat of vaporization (ΔHvap). The heat of fusionand the heat of vaporization can be used to calculate the amount ofheat needed to melt or vaporize, respectively, a given amount ofsubstance. For example, the heat of fusion for H2O is 6.02 kJ/mol, whichmeans that 6.02 kJ of heat is needed to melt a mole of ice. Twiceas much heat is needed to melt twice as much ice, as shownhere: 2.00 mol×6.02 kJ/mol=12.0 kJ

Constants Heat of fusion (ΔHfus) is used for calculationsinvolving a phase change between solid and liquid, with notemperature change. For H2O, ΔHfus=6.02 kJ/mol. Specific heat capacity (C) is used for calculationsthat involve a temperature change, but no phase change. For liquidwater, C=4.184 J/(g⋅∘C). Heat of vaporization (ΔHvap) is used for calculationsinvolving a phase change between liquid and gas, with notemperature change. For H2O, ΔHvap=40.7 kJ/mol. Part A How much heat is required to melt 52.5 g of ice at its meltingpoint? Express your answer numerically in kilojoules. 17.5   kJ   SubmitHintsMyAnswersGive UpReviewPart Correct Part B How much heat is required to raise the temperature of52.5 g of water from its melting point to its boilingpoint? Express your answer numerically inkilojoules. 158.0775   kJ   SubmitHintsMy AnswersGive UpReview Part Incorrect; Try Again; 4 attempts remaining; no pointsdeducted ****NEED HELP PLEASE PART B ANSWER IS WRONG****