Mount Everest rises to a height of 8,850 m above sea level. At a base camp on the mountain the atmospheric pressure is measured to be 311.0 mm Hg. At what temperature (in °C) will water boil at base camp ? The vapor pressure of water at 373 K is 760.0 mm Hg.

The boiling point at the base camp is 152.6 K

Explanation:

Step 1: data given

The atmospheric pressure at the base camps = 311.0 mmHg

The vapor pressure of water at 373 K is 760.0 mm Hg

Step 2: Calculate the boiling temperature at the basecamps

P1/T1 = P2/T2

⇒with P1 = The atmospheric pressure at the base camps = 311.0 mmHg

⇒with T1 = The boiling point at the base camp = TO BE DETERMINED

⇒with P2 = The vapor pressure of water at 373 K is 760.0 mm Hg

⇒with T2 = the boiling temperature of water = 373 K

311.0 mmHg / T1 = 760.0 mmHg / 373 K

T1 = 310.0 mmHg / (760.0 mmHg / 373 K)

T1 = 152.6 K

The boiling point at the base camp is 152.6 K