The ambient temperature is 85.0°F and the humidity of the surrounding air is reported to be 56.0%. Using the Clausius-Clapeyron equation and the boiling point of water as 100.0°C at 760 torr, calculate the vapor pressure (in torr) of water in the air. Use 40.7 kJ/mol as the ∆Hvap of water.

The vapor pressure is 748.77 torr

Explanation:

Using Clausius-Clapeyron equation:

where;

T₁ is the initial temperature = 85.0°F = 302.5 K

T₂ is the final temperature = 100 °C = 373 K

P₂ is the final pressure = 760 torr

P₁ is the initial pressure = vapor pressure = ?

R is gas constant = 8.314 J/K.mol

ΔHvap is the heat of vaporization of water = 40.7 kJ/mol

4.895(0.00331 - 0.00268) = 0.01489

= 1.015

P₁ = (760 torr)/(1.015) = 748.77 torr

Therefore, the vapor pressure is 748.77 torr

the answer is a. at the equator