A sample of helium gas was placed in a cylinder with a sealed piston (a closed s

Question

A sample of helium gas was placed in a cylinder with a sealed piston (a closed system) and the volume of the gas was measured as the pressure was slowly increased at the constant temperature The results of this experiment are shown graphically. At what pressure does the gas occupy a volume of 5 L? What is the volume of the gas at a pressure of 5 atm? Calculate the Boyle's law constant at a volume of 2 L. Calculate the Boyle's law constant at a volume of 2 atm. The temperature of a gas is raised from 25 degreeC to 50 degreeC. Will the volume double if mass and pressure do not change? Why or why not? If 2.25 L of gas at 16 degreeC and 1.00 atm is compressed at a pressure of 125 atm at 20 degreeC, calculate the new volume of the gas. H_2O and CH_4 are gases at 150 degreeC. Which exhibits more ideal behavior? Why? A gas mixture has a total pressure of 0.56 atm and consists of He and Ne. If the partial pressure of the He in the mixture is 0.27 atm, what is the partial pressure of the Ne in the mixture?

Explanation / Answer

Boyles law states that PV= constnat ( when temperature and number of moles of gas are fixed)

At 5 L, from the chart, P=1 atm since PV=5atm.L

At 5 atm V= 1L and boyles law constant = 2*2.5= 5 atm.L

At 2 atm, P=2.5 atm and PV=2*2.5 =5 atm.L

2) from P1V1/T1= P2V2/T2

Since P1 and P2 are same V1/T1= V2/T2, V2/V1= T2/T1= (50+273.15)/925+273.15)=1.08

The volume does not get doubled.

3) from P1V1/T1= P2V2/T2

P1= 1atm V1= 2.25L T1= 16+273.15= 289.15K

P2=125 atm T2= 20+273.15= 293.15, V2= P1V1*T2/P2T1= 1*2.24*293.15/(125*289.15)=0.0182L

4) H2O and CH4 have near identical masses but H2O has strong hydrogen bonding. Hence CH4 behaves ideally since ideality refers to zero intermolecular forces of attraction due to hydrogen bonding.

5) total pressure = partial pressure of helium + partial pressure of Ne

0.56= 0.27+ partial pressure of Ne

Partial pressure of Ne= 0.56-0.27= 0.29 atm

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