Question

a. A sample of oxygen occupies a volume of 1.5 L at 95°C. What will be the temperature when the volume of oxygen is reduced to 1.0 L, keeping the pressure constant? Given: K (Temperature in Kelvin) = C (Temperature in Celsius) + 273.15

b. A container holds 400 mL of nitrogen at 20° C and 742 torr. What will be the volume of the nitrogen (in mL) if the pressure is increased to 795 torr at constant temperature? (Hint: Conversions not required in part b)

Answer 1

a) V1=1.5L

T1= 368.15k

V2=1.0L

T2=?

$V1T2=V2T1$

T2=(1*368.15)/1.5

T2=245.43K

b) V1=400ml

P1=742torr

V2=?

P2=795torr

$P1V1=P2V2$

V2=(742*400)/795

V2=373.33ml