How much energy is required tp vaporize 48.7 g pf dichloromethane at its boiling point, if tis Hvap is 31.6 kJ/mol?
Moles of CH2Cl2 = mass/molar mass
= 48.7/84.93 = 0.5734 mol
Energy required = moles x ΔHvap
= 0.5734 x 31.6 = 18.1 kJ
How much energy is required tp vaporize 48.7 g pf dichloromethane at its boiling point, if...
53) How much energy is required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point, if its AHvap is 31.6 kJ/mol? A) 31.2 kJ B) 6.49 kJ C) 18.1 kJ D) 55.1 kJ E) 15.4 kJ
5) How much more heat is required to vaporize 48.7 g of ethanol (C,H,OH) than to vaporize 48.7 g of dichloromethane (CH2Cl2) ethanol dichloromethane AHvap is 40.5 kJ/mol AHvap is 31.6 kJ/mol AHfus is 5.02 kJ/mol AHfus is 6.20 kJ/mol Cs=2.46 J/gºC Cs= 1.19 J/g°C
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