A piece of dry ice (solid carbon dioxide) with a mass of 5.50 g is placed in a 10.0-l vessel that already contains air at 705 torr and 24 °c. after the carbon dioxide has totally sublimed, what is the partial pressure of the resultant co2 gas, and the total pressure in the container at 24 °c?

The partial pressure of resultant CO₂ gas is 231.5 torr

The total pressure = 936.5 torr

calculation

The partial for CO₂ is calculated using the ideal gas equation

That is PV=nRT

where;

p (pressure = ?

V (volume) = 10.0 l

n (number of moles) = mass:molar mass

from periodic table the molar mass of CO₂ = 12 + (16 x2) = 44 g/mol

moles = 5.50 g:44 g/mol = 0.125 moles

R (gas constant) = 62.36 torr

T (temperature) = 24°c into Kelvin = 24 + 273 = 297 K

make P the subject of the formula by diving both side of equation by V

P = nRT/V

P = { (0.125 moles x 62.36 L. torr/Mol. K x297 K) / 10 L} = 231.5 torr

Total pressure = partial pressure for air + partial pressure for CO₂

= 705 torr + 231.5 torr = 936.5 torr