To an evacuated 504.2 mL steel container is added 25 g CaCO 3 and the temperature is raised to 1500 K causing a complete decomposition of the salt. If the density of CaO formed is 3.3 g/cc, find the accurate pressure developed in the container using the vander Waals equation of state. The van der waals constants for CO 2 (g) are a = 4 
, b = 0.04 
. (Ca - 40, C - 12, O - 16). Report your answer as nearest whole number.
Text Solution
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(62 atm.)
CaCO 3 (s) 
CaO (s) + CO 2 (g)
Moles of CaCO 3 used = 
Moles of CaO formed = 
= moles of CO 2 formed
Mass of CaO formed = 
× 56 g = 14 g
Volume occupied by CaO = 
cc ≈ 4.2 mL
∴ Volume available for CO 2 (g) = 504.2 – 4.2 mL = 0.5 L
Now applying the vander Waals equation of state
(v – nb) = nRT
[0.5 – 0.25 × 0.04] = 0.25 × 0.082 × 1500
⇒ p = 62.83 – 
= 61.83 atm.
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