The vapor pressure of dichloromethane, ch2cl2, at 0 ∘c is 134 mmhg. the normal boiling point of dichloromethane is 40. ∘c. calculate its molar heat of vaporization.

The molar heat of vaporization is 30.6 kJ/mol

Explanation:

To calculate the molar heat of vaporization, we use the equation given by  Clausius-Clapeyron, which is:

Where,  

= vapor pressure at temperature = 134 mmHg

= vapor pressure at temperature (atmospheric pressure) = 760 mmHg

= molar heat of vaporization

R = gas constant = 8.314 J/mol.K

= temperature of dichloromethane =

= normal boiling point of dichloromethane =

Putting values in above equation, we get:

Hence, the molar heat of vaporization is 30.6 kJ/mol

answer

i think the answer is a) as air pressure in an area increases, the density of the gas particles in that area decreases.

hope it