A sample of ideal gas at room temperature occupies a volume of 39.0 L and pressu

Question

A sample of ideal gas at room temperature occupies a volume of 39.0 L and pressure of 542 torr. If the pressure changes to 2710 torr, with no change in the temperature or moles of gas, what is the new volume of, V2?
V2= ? L
Volume of the original sample in part A (p1 = 542 torr v1 = 39.0 l) changed to 63.0 L, without a change in the temperature or moles of gas molecules, what is the new pressure, p2
P2= ? Torr A sample of ideal gas at room temperature occupies a volume of 39.0 L and pressure of 542 torr. If the pressure changes to 2710 torr, with no change in the temperature or moles of gas, what is the new volume of, V2?
V2= ? L
Volume of the original sample in part A (p1 = 542 torr v1 = 39.0 l) changed to 63.0 L, without a change in the temperature or moles of gas molecules, what is the new pressure, p2
P2= ? Torr
V2= ? L
Volume of the original sample in part A (p1 = 542 torr v1 = 39.0 l) changed to 63.0 L, without a change in the temperature or moles of gas molecules, what is the new pressure, p2
P2= ? Torr

Explanation / Answer

Case1: Given data,

Initial Pressure, P1 = 542 torr

Final Pressure, P2 = 2710 torr

Initial Volume, V1 = 39.0 L

Final Volume, V2 = ?

We know that, according to Boyle's law,

P1V1 = P2V2     (at constant temperature and no.of moles)

542 X 39 = 2710 X V2

V2 = (542 X 39)/2710

V2 = 7.8 L

Case2: Given data,

Initial Volume, V1 = 39 L

Final Volume, V2 = 63 L

Initial Pressure, P1 = 542 torr

Final Pressure, P2 = ?

We know that, according to boyle's law,

P1V1 = P2V2        (at constant temperature and no.of moles)

542 X 39 = P2 X 63

P2 = (542 x 39)/63

P2 = 335.5 torr.

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