Question about boiling point change when there is a pressure change?

The normal boiling point of liquid ethanol is 351 K at 1.00 atm. Assuming that its molar heat of vaporization is constant at 45.1 kJ/mol, so what is the boiling point of C2H5OH when the external pressure is 0.622 atm?

Answer:
This is a gas law question as we're talking of the temperature of the vapour which is equal to the liquid temperature at its boiling point and refers to Gay Lussac's law.

P1 x T2 = P2 X T1
1atm. x T2 = 0.622atm. x 351K.
T2 = 0.622 x 351
New boiling temperature (T2) = 218.3 K

(Molar heat of vaporisation is superfluous to the calculation as we are talking about boiling point).

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