How much energy is required to vaporize 48.7 g of dichloromethane (ch2cl2) at its boiling point, if its δhvap is 31.6 kj/mol? how much energy is required to vaporize 48.7 g of dichloromethane (ch2cl2) at its boiling point, if its δhvap is 31.6 kj/mol? 6.49 kj 15.4 kj 18.1 kj 55.1 kj 31.2 kj?

This energy required is the latent heat, which is required for physical transformations. Specifically, when it involves changing liquid to gas, this latent heat is called the heat of vaporization. The formula is:

Q = mΔHvap
The molar mass of the compound is 
Q = (48.7 g)(31.6 kJ/mol)(1 mol/84.93 g)
Q = 18.12 kJ

Answer) by studying proton collisions hope this : )