The heat of vaporization ΔHᵥ of diethyl ether ((CH₃)₂(CH₂)₂O) is 26.7 KJ/mol. Calculate the change in entropy Δs when 3.4 g of diethyl ether condenses at 34.6 °C.
Be sure your answer contains a unit symbol and the correct number of significant digits.

ΔS = 4.1 J/K

Explanation:

Enthalpy (H) is defined as the amount of energy released or absorbed during a chemical reaction.

Entropy (S) defines the degree of randomness or disorder in a system.

The relationship between both parameters is given as;

ΔS = ΔH / T

ΔH = 26.7 KJ/mol for 1 mol of diethyl ether

number of moles = mass / molar mass

number of moles = 3.4 / 72 = 0.04722

ΔH = 26700 * 0.04722 = 1260.77 J

T = 34.6 + 273 = 307.6 (upon converting to kelvin temperature)

ΔS = 1260.77 / 307.6

ΔS = 4.1 J/K

first one is the correct answer