<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
482VP I think is the correct answer.
Answer:
Explanation:
A buffer pair consists of either
- A weak acid and its salt or
- A weak base and its salt
(a) Oxalic acid and sodium oxalate
Oxalic acid is an acid and lithium acid is a base. Together, they will neutralise each other and form the salt LiHC₂O₄.
A solution of LiHC₂O₄ is not a buffer.
The correct buffer pair is H₂C₂O₄ and LiHC₂O₄
(b) Carbonic acid and sodium carbonate
The carbonic acid and the sodium carbonate will neutralise each other and form the salt NaHCO₃.
A solution of NaHCO₃ is not a buffer.
The correct buffer pair is H₂CO₃ and NaHCO₃