What is the change in entropy that occurs in the system when 1.00 mol of methanol (ch3oh) vaporizes from a liquid to a gas at its boiling point (64.6 ∘c)? for methanol, δhvap=35.21kj/mol. what is the change in entropy that occurs in the system when 1.00 of methanol () vaporizes from a liquid to a gas at its boiling point (64.6 )? for methanol, . -545 j/k 104 j/k -104 j/k 545 j/k?

104 J/K

Explanation:

First, we have to calculate the heat (Q) involved in the vaporization of 1.00 mol of methanol.

Q = n × ΔH°vap

Q = 1.00 mol × 35.21 kJ/mol = 35.2 kJ

Then, we have to convert the boiling point to Kelvin.

K = °C + 273.15

K = 64.6 + 273.15 = 337.8 K

Finally, we calculate the change in the entropy associated with this process.

ΔS = Q/T

ΔS = 35.2 kJ/337.8 K = 0.104 kJ/K = 104 J/K

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