Determine the normal boiling point of a substance whose vapor pressure is 55.1 mm hg at 35°c and has a δhvap of 32.1 kj/mol.

389.78681 K

Explanation:

= Initial pressure = 55.1 mmHg

= Final pressure = 1 atm = 760 mmHg

= Boiling point

= Initial temperature = 35°C

= Heat of vaporization = 32.1 kJ/mol

From the Clausius-Claperyon equation

The normal boiling point of the substance is 389.78681 K

pythagoras' theorem

square root (-5^2+9^2)

square root (25+81)

square root (106)

angle is tan^-1(9/5)

neg x, pos y

t = 1/400 h   ⇔ 0.0025 h ⇔ 9s ⇔ 0.15 m

any of the answers are correct.