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 60.0 g of ethyl chloride? A)24.6 kJ B)1584 kJ C)2.28 kJ D)1703 kJ

Question

Quizplus · Accepted Answer

First, calculate the molar mass of ethyl chloride (C2H5Cl): C (12.01 g/mol) * 2 + H (1.008 g/mol) * 5 + Cl (35.45 g/mol) = 64.51 g/mol. Then, use the formula q = m/M * ΔHvap, where m = 60.0 g, M = 64.51 g/mol, and ΔHvap = 26.4 kJ/mol. This gives q = (60.0 g / 64.51 g/mol) * 26.4 kJ/mol ≈ 24.6 kJ.

Ethyl Chloride,C2H5Cl,is Used as a Local Anesthetic

Ethyl Chloride,C₂H₅Cl,is Used as a Local Anesthetic