The normal boiling point of mercury (Hg) is 356.7 °C. What is the vapor pressure of mercury at 322 °C? (∆Hvap = 58.51 kJ/mol)

The vapor pressure of mercury at 322°C is 0.521 atm

Explanation:

To calculate the final pressure, we use the Clausius-Clayperon equation, which is:

where,

= initial pressure which is the pressure at normal boiling point = 1 atm

= final pressure which is vapor pressure of mercury = ?

= Enthalpy of vaporization = 58.51 kJ/mol = 58510 J/mol     (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314 J/mol K

= initial temperature which is normal boiling point =

= final temperature =

Putting values in above equation, we get:

Hence, the vapor pressure of mercury at 322°C is 0.521 atm

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.