Answer:
Total Pressure = 745.6 torr
Partial Pressure of He = 272.8 torr
Partial Pressure of Ar = 472.8 torr
Explanation:
Step 1: Data given
Volume of the flask helium = 265 mL
Pressure in the helium flask = 751 torr = 751/760 atm
Volume of the flask argon = 465 mL
Pressure in the argon flask = 727 torr = 727/760 atm
The total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture.
Step 2: Calculate total volume
Total volume = 265 mL + 465 mL = 730 mL = 0.730 L
Step 3: Boyle's Law:
P1V1=P2V2
⇒ with P1 = total pressure gas exerts in its own flask
⇒ with V1 = volume of flask with stopcock valve closed
⇒ with P2 = partial pressure of gas exerts on total volume of both flasks when stopcock valve is opened
⇒ with V2 = total volume of both flasks with stopcock valve opened
Helium using Boyle's Law equation from above:
P1V1=P2V2
⇒ with P1 = Pressure of helium = 751 /760 = 0.98816 atm
⇒ with V1 = volume of helium = 0.265 L
⇒ with P2 = The new partial pressure of helium
⇒ with V2 = total volume = 0.730 L
(0.98816 atm)(0.265L)=P2(0.730L)
P2=0.359 atm
Argon using Boyle's Law equation from above:
P1V1=P2V2
⇒ with P1 = Pressure of argon = 727/760 = 0.95658 atm
⇒ with V1 = volume of argon = 0.465 L
⇒ with P2 = The new partial pressure of argon
⇒ with V2 = total volume = 0.730 L
(0.95658 atm)(0.465L)=P2(0.730L)
P2=0.609 atm
Step 4: Convert pressure in atm to torr
Pressure helium = 0.359 atm = 272.8 torr
Pressure argon = 0.609 atm = 472.8 torr
Step 5: Calculate Total pressure
Ptotal = P(He)+P(Ar)
⇒ Pt = total pressure of the gas mixture
⇒ P(He) = partial pressure of Helium
⇒ P(Ar) = partial pressure of Argon
Pt = 272.8 torr + 472.8 torr
Pt = 745.6 torr
Total Pressure = 745.6 torr
Partial Pressure of He = 272.8 torr
Partial Pressure of Ar = 472.8 torr
