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?

V = 479.6 mL

Explanation:

assuming ideal gas:

∴ T = 25.2°C ≅ 298.2 Kremains 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 molremains constant

∴ P2 = 712 torr = 0.936842 atm

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

⇒ V2 = 0.4796 L

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).

lol for the pointsss