Ethyl chloride, c2h5cl, is used as a local anesthetic. it works by cooling tissue as it vaporizes. the heat of vaporization is 26.4 kj/mol. how much heat could be removed by 10.0 g of ethyl chloride?

4.092 kJ

Explanation:

When a material vaporizes, it increases its own energy by absorbing energy from surroundings or a heat source. The specific molar heat of vaporization (kJ/mol) is the energy required to vaporize one mole of a substance. The total energy which can be absorbed by a given amount of material can be determined by multiplying the number of available moles by the specific molar heat of vaporization.

Step 1: Determine number of moles of ethyl chloride in 10.0g

a) Calculate molar mass of ethyl chloride

b) Divide mass of ethyl chloride by its molar mass to determine 'n', number of moles

Step 2: Determine heat removed by available moles of ethyl chloride based on its specific heat of vaporization (v = 26.4 kJ/mol)

a. they are both space stations

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