<u>Answer:</u> The vapor pressure of mercury at 322°C is 0.521 atm
<u>Explanation:</u>
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
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Ans is B.Bromine. Only two elements are liquid at room temperature ( mercury and Bromine) . Helium and chlorine, arsenic are gases.