if a sample of gas at 25.2°C has a volume of 536 ml at 637 torr, what will its volume be if the pressure is increased to 712 torr?

Question

Felix

Chemistry

5 February, 21:03

if a sample of gas at 25.2°C has a volume of 536 ml at 637 torr, what will its volume be if the pressure is increased to 712 torr?

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Answers (1)

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Quincy · Answer 1

V = 479.6 mL

Explanation:

assuming ideal gas:

PV = RTn

∴ T = 25.2°C ≅ 298.2 K ... remains constant

∴ P1 = 637 torr = 0.8382 atm

∴ V1 = 536 mL = 0.536 L

∴ R = 0.082 atm. L/K. mol

⇒ n = (P1V1) / (RT) = ((0.8382 atm) * (0.536 L)) / ((0.082 atmL/Kmol) * (298.2K))

⇒ n = 0.0184 mol ... remains constant

∴ P2 = 712 torr = 0.936842 atm

⇒ V2 = RTn/P2 = [ (0.082atmL/Kmol) * (298.2K) * (0.0184mol) ] / (0.936842atm)

⇒ V2 = 0.4796 L