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

Considering ideal gas:

PV = RTn

T = 25.2°C = 298.2 K

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) x (0.536 L)) /

((0.082 atmL/Kmol) x (298.2K))

:. n = O. 0184 mol

Then,

P2 = 712 torr = 0.936842 atm

V2 = RTn/P2 = [ (0.082atmL/

Kmol) x (298.2K) x (0.0184mol) ] / (0.936842atm)

:. V2 = 0.4796 L

OR

V2 = 479.6 ml