Problem 10.67 A piece of solid carbon dioxide with a mass of 5.70 g is placed in
ID: 691880 • Letter: P
Question
Problem 10.67
A piece of solid carbon dioxide with a mass of 5.70 g is placed in a 10.0-L vessel that already contains air at 715 torr and 22 C .
Part A
After the carbon dioxide has totally vaporized, what is the partial pressure of carbon dioxide in the container at 22 C ?
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Part B
After the carbon dioxide has totally vaporized, what is the total pressure in the container at 22 C ?
Express your answer using four significant figures.
Problem 10.67
A piece of solid carbon dioxide with a mass of 5.70 g is placed in a 10.0-L vessel that already contains air at 715 torr and 22 C .
Part A
After the carbon dioxide has totally vaporized, what is the partial pressure of carbon dioxide in the container at 22 C ?
SubmitMy AnswersGive Up
Incorrect; Try Again
Part B
After the carbon dioxide has totally vaporized, what is the total pressure in the container at 22 C ?
Express your answer using four significant figures.
PCO2 = atm Ptotal = atmExplanation / Answer
Pressure of air = P= 715 torr= 0.941 atm 1 torr= 0.00131579atm
T=22C= 22+273= 295K
R= 0.0821 L-atm/mole-K
Volume of air= V= 10.0L
PV= nRT
n= PV/RT= 0.941x10.0/0.0821x295 = 0.388moles
number of moles of air= 0.388 moles
mass of CO2= 5.7 grams
molar mass of CO2=44 grams
number of moles of CO2 = 5.7/44= 0.1295 moles
Total number of moles= 0.388 + 0.1295= 0.5175 moles
mole fraction of CO2 = number of moles of CO2/total numbe of moles
mole fraction of CO2= 0.1295/0.5175= 0.25
PartB
Total pressure
PV= nRT
P= nRT/V = 0.5175x0.0821x295/10 = 1.25 atm
Total pressure = 1.25 atm
Part-A
partial pressure of CO2 = Total pressure x molefraction of CO2
= 1.25x0.25= 0.3125 atm
Partial pressure of CO2= 0.3125 atm= 0.313 atm.
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