Question

A mixture containing 0.768 mol He(g), 0.286 mol Ne(g), and 0.116 mol Ar(g) is confined in a 10.00-L vessel at 25 ∘C.

Calculate the partial pressure of He in the mixture. P= atm

Calculate the partial pressure of Ne in the mixture. P= atm

Calculate the partial pressure of Ar in the mixture. P= atm

Calculate the total pressure of the mixture. P= atm

Answer #1

A mixture containing 0.770 mol He(g), 0.244 mol Ne(g), and 0.119
mol Ar(g) is confined in a 10.00-L vessel at 25 ∘C
Part A
Calculate the partial pressure of He in the mixture.
Part B
Calculate the partial pressure of Ne in the mixture
Part C
Calculate the partial pressure of Ar in the mixture.
Part D
Calculate the total pressure of the mixture

A mixture of three gases (Ar, Ne, and CO2) has a total pressure
of 1.2 atm. If the mixture of gases is composed of 25.0 g of each
gas, what is the partial pressure of Ne?

A 2.57-L flexible flask at 12°C contains a mixture of N2, He,
and Ne at partial pressures of 0.297 atm for N2, 0.157 atm for He,
and 0.455 atm for Ne. (a) Calculate the total pressure of the
mixture. (b) Calculate the volume in liters at STP occupied by He
and Ne if the N2 is removed selectively.

A) A mixture of He, Ar, and Xe has a total pressure of 2.80 atm
. The partial pressure of He is 0.400 atm , and the partial
pressure of Ar is 0.300 atm . What is the partial pressure of
Xe?
B) A volume of 18.0 L contains a mixture of 0.250 mole N2 ,
0.250 mole O2 , and an unknown quantity of He. The temperature of
the mixture is 0 ∘C , and the total pressure is...

A mixture containing 2.65 g each of CH4(g), C2H4(g) and C4H10(g)
is contained in a 1.50 L flask at a temperature of 25°C. (a)
Calculate the partial pressure of each of the gases in the mixture.
PCH4 = atm PC2H4 = atm PC4H10 = atm (b) Calculate the total
pressure of the mixture.

7. A) A mixture of He, Ar, and Xe has a total pressure of 2.70
atm . The partial pressure of He is 0.200 atm , and the partial
pressure of Ar is 0.250 atm . What is the partial pressure of
Xe?
B) A volume of 18.0 L contains a mixture of 0.250 mole N2 ,
0.250 mole O2 , and an unknown quantity of He. The temperature of
the mixture is 0 ∘C , and the total pressure...

A gas mixture contains 0.70 mol of N2, 0.25 mol of H2, and 0.35
mol of CH4. Calculate the pressure of the gas mixture and the
partial pressure of each constituent gas if the mixture is in a 7.0
L vessel at 27 degrees celsius.
A) Total pressure in the vessel (atm)
B) Pressure of H2 (atm)
C) Pressure of N2 (atm)
D) Pressure of CH4 (atm)

A vessel contained N2, Ar, He, and Ne. The total pressure in the
vessel was 987 torr. The partial pressures of nitrogen, argon, and
helium were 44.0, 486, and 218 torr, respectively. Calculate the
mole fraction of neon.

In a mixture of He, Ne, and Xe gases with a total pressure of
925 atm, if there is 10.5 g of each gas in the mixture, what is the
partial pressure of Xe?

Part A
A mixture of He, Ar, and Xe has a total pressure of 2.90 atm .
The partial pressure of He is 0.450 atm , and the partial pressure
of Ar is 0.250 atm . What is the partial pressure of Xe? Express
your answer to three significant figures and include the
appropriate units.
Part B
A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250
mole O2 , and an unknown quantity of He....

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