Chloromethane, , arises from microbial fermentation and is found throughout the environment. it is also produced industrially and is used in the manufacture of various chemicals and has been used as a topical anesthetic. calculate how much energy is required to convert 90.6 g liquid to a vapor at its boiling point, –24.09 °c. (the heat of vaporization of is 21.40 kj/mol.)

The energy is required to convert 90,6 g liquid to a vapor is 38,4 kJ

Explanation:

The transformation you need is:

Chloromethane (l) → Chloromethane (g)

This process need an energy of 21,40 kJ/mol.

In 90,6 g of chloromethane (molar mass of 50,49 g/mol) you have:

= 1,79 moles of chloromethane.

Thus, energy is required to convert 90,6 g liquid to a vapor is:

= 38,4kJ

I hope it helps!

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