For a certain amount of gas at constant temperature, the pressure and volume hav

Question

For a certain amount of gas at constant temperature, the pressure and volume have an inverse relationship (Figure 1). This is called Boyle's law: P_1 V_1 = P_2 V_2 A sample of ideal gas at room temperature occupies a volume of 28.0 L at a pressure of 622 torr . If the pressure changes to 3110 torr, with no change in the temperature or moles of gas, what is the new volume, V_2? Express your answer with the appropriate units. If the volume of the original sample in Part A (P_1 = 622 torr, V_1 = 28.0 L) changes to 70.0 L, without a change in the temperature or moles of gas molecules, what is the new pressure, P_2? Express your answer with the appropriate units.

Explanation / Answer

Part A 1atm=760 torr 1 torr = 1/760 atm 0.00132 1 torr = 0.00132 atm Temparature = Constant P1 = 622 torr P1 = 622 *0.00132 0.82104 P1 = 0.8214 atm V1 = 28.0 L P2 = 3110 torr P2 = 3110*0.00132 atm 4.1052 P2= 4.1052 atm V2= ? According to Boyels Law P1V1 =P2V2 V2 = P1V1 /P2 V2 = 0.8214*28/4.1052 5.602455422 V2 = 5.60 L Part B 1atm=760 torr 1 torr = 1/760 atm 0.00132 1 torr = 0.00132 atm Temparature = Constant P1 = 622 torr P1 = 622 *0.00132 0.82104 P1 = 0.8214 atm V1 = 28.0 L given here volume is V2= 70.0 L According to Boyels Law P1V1 =P2V2 P2 = P1V1 /V2 P2 = 0.8214*28/70.0 0.32856 P2 = 0.328 atm

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