Question

Denver, Colorado (altitude above sea level is 5,280 ft) has an atmospheric pressure of 633. mm Hg. Calculate the boiling point of water in Denver, Colorado. The heat of vaporization for water is 40.7 kJ/mol.

Answer 1

T2 = 94.6 C

Step-by-step explanation:

Use Clausius-Clayperyon equation.

ln P1/P2 = ∆Hvap/R (1/T2 - 1/T1) where R = 8.314 J/mol-K and T is in degrees K

P1 = 760 mmHg

P2 = 630 mmHg

T1 = 373 K

T2 = ?

∆Hvap = 40.7 kJ/mole

R = 0.008314 kJ/mole-K (NOTE: change R to units of kJ)

Plug in and solve for T2

ln 760 mmHg/630 mmHg = 40.7 kJ/mole (1/T2 - 1/373K)

T2 = 367.74 K = 94.6 C