Dry ice is solid carbon dioxide. A 1.75−g sample of dry ice is placed in an evacuated 4.57−L vessel at 20.0°C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas.
i) Determine the number of moles of CO2
Dry ice is solid form of CO2
number of moles = Mass /Molar mass
mass of CO2 = 1.75g
Molar mass of CO2 = 44.01g
substituting the values
Number of moles of CO2 = 12.01g/44.01g/mol = 0.27289mol
ii) Detemine the pressure of CO2 using ideal gas law
Ideal gas law is follows
PV = nRT
where,
P = Pressure, ?
V = Volume , 4.57 L
T = Temperature, 293.15K ( ℃ should be converted into Kelvin unit while applying Ideal gas equation , 0℃ = 273.15K)
n = Number of moles , as calculated above it is 0.27289mol
R = gas constant, 0.082057(L atm/mol K)
rearranging ideal gas equation
P = nRT /V
substituting the values
P = 0.27289mol × 0.082057(L atm/mol K) × 293.15K/4.57L
P = 1.44atm
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