20. What is the mole fraction of hydrogen in a gaseous mixture that consists of
ID: 571617 • Letter: 2
Question
20. What is the mole fraction of hydrogen in a gaseous mixture that consists of 8.00 g of hydrogen and 12.00 g of neon in a 3.50 liter container maintained at 35.20 "C? a. 0.150 b. 0.400 c. 0.660 d. 0.870 e. 0.930 21. A sealed glass container contains 0.2 moles of O gas and 0.3 moles of N2 gas. If the total pressure inside the container is 0.75 atm what is the partial pressure of O; in the glass container? a. 0.20 atm b. 0.30 atm c. 0.50 atm d. 0.75 atm e. 0.45 atm 22. A sealed glass container contains partial pressures of 0.24 atm O, gas and 0.46 atm H2 gas. What is the mole fraction of H2 in the glass container? a. 0.70 b. 0.24 c. 0.46 d. 0.65 e. 0.34 23. A sealed glass container contains partial pressures of 0.80 atm CO2 gas and 0.35 atm N2 gas. What is the mole fraction of N2 in the glass container? a. 0.35 b. 1.15 c. 0.70 d. 0.80 e. 0.30 24. A sealed glass container contains partial pressures of 0.24 atm O2, 0.45 atm CO2, 0.64 atm N2. and 0.46 atm H2 gas in a 3.5 L container at 30.5 C. What is the total pressure exerted on the walls of the container? a. 1.79 atm b. 6.27 atm c. 0.51 atm d. 1902 atm e. 0.64 atmExplanation / Answer
All the questions are based on Dalton's law of partial pressures.
According to this law when two or more non-reacting gases are present in a container, the total pressure of the mixture is equal to the sum of partial pressure of the gases.
And partial pressure of a gas = mole fraction x total pressure of mixture
20) moles of H2 = mass/ molar mass
= 8g/2g/mol = 4
moles of Ne = 12g/ 20g/mol
= 0.6
total moles = 4+0.6 =4.6
Thus mole fraction of H2 = moles of H2 / total moles
= 4/4.6 = 0.8695
= 0.87
Thus option D
21) moles of O2 = 0.2
moles of N2 = 0.3
total moles = 0.2 + 0.3 = 0.5
total pressure = 0.75
partial pressure of O2 = moles fraction x total pressure
= [0.2/0.5] x0.75 atm
= 0.3 atm
OPTION B
22)Partial pressure of O2 = 0.24 atm
partial pressure of H2 = 0.46
Total pressure = 0.24 + 0.46 = 0.70 atm
Mole fraction of H2 = partial pressure / total pressure
= 0.46atm/0.70atm
= 0.6570
OPTION D
23)
parital presssure of CO2 = 0.80 atm
partial pressre of N2 = 0.35 atm
total pressure = 0.80+0.35 = 1.15 atm
mole fraction of N2 = PN2/P total
= 0.35/1.15
= 0.304
OPTION E
24)
Partial pressure of O2= 0.26atm
Partial pressure of CO2= 0.45atm
Partial pressure of N2= 0.64atm
Partial pressure of H2= 0.46atm
Thus total pressure = ).26 + 0.45+ 0.64 + 0.46 atm
= 1.799 atm
OPtion A
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