1- Consider 4.90 L of a gas at 365 mmHg and 20. degrees celisus . If the contain
ID: 607911 • Letter: 1
Question
1- Consider 4.90 L of a gas at 365 mmHg and 20. degrees celisus . If the container is compressed to 3.00 L and the temperature is increased to 40.degrees celisus , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder. 2- A sample of gas in a cylinder as in the example in Part A has an initial volume of 52.0 L, and you have determined that it contains 1.10 moles of gas. The next day you notice that some of the gas has leaked out. The pressure and temperature remain the same, but the volume has changed to 13.0 L. How many moles of gas (n2) remain in the cylinder?Explanation / Answer
For a gas PV/T = constant
So P1*V1/T1 = P2*V2/T2
Given V1 = 4.9L,P1 = 365mmHg ,T1 = 20degree celsius = 273+20 = 293K
V2 = 3,T2=40degree celsius = 313K
P2 = 636.8mmHg
2)For a gas V/n remains constant
Given V1 = 52L,n1 = 1.1 , V2 = 13L,n2 = ?
n2 = (V2/V1)*n1 = 0.275moles of gas
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