If 800 ml of dry gas @ a barometic pressure of 600 torr & 37C shrinks to 400 ml & 0C dry what is the pressure?

Question

Who's law?

Answer 1

800 mL = 0.800 L
600 torr = 0.789 atm
37 ° C = 310 K

400 mL = 0.400 L
0°C = 273 K

We have to use the equation

p1V1 / p2V2 = T1 /T2

0.789(0.800) /p2 (0.400 )= 310 / 273

0.631 / p2(0.400) =1.13

p2 = 1.4 atm>> 1061 torr

Answer 2

That's the combined gas law.

P1V1/T1 = P2V2/T2
P2 = P1V1T2/V2T1 = (600 torr)(800 ml)(273 K)/(400 ml * 310 K)
P2 = 1057 torr

Answer 3

Three.