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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.)

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Answer:

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:

[tex]90,6g * \frac{1mol}{50,49g}[/tex] = 1,79 moles of chloromethane.

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

[tex]1,79 mol * \frac{21,40kJ}{1mol}[/tex] = 38,4kJ

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