A piece of solid carbon dioxide with a mass of 5.50 g is placed in a 10.0-L vessel that already contains air at 710 torr and 25 ∘C.?
After the carbon dioxide has totally vaporized, what is the partial pressure of carbon dioxide in the container at 25 ∘C ?
After the carbon dioxide has totally vaporized, what is the total pressure in the container at 25 ∘C?
Express your answer using four significant figures.
- Roger the MoleLv 72 months ago
P = nRT / V = (5.50 g CO2 / (44.00964 g CO2/mol)) x (62.36367 L torr/K mol) x
(25 + 273) K / (10.0 L) = 232.3 torr CO2
232.3 torr + 710 torr = 942.3 torr total
[There are the requested four significant digits, but they are not all justified.]