Question

a sample of Nitrogen gas occupies a volume of 1.1 litre at a pressure of. 5 bar at 40 degree Celsius calculate the pressure if the gas is compressed to 0.225 ML at minus 6 degree Celsius

Answer 1

given is P1=5 bar,T1=313K,V1=1.1L=1.1×1000=1100ML
P2=?,T2=267K,V2=0.225
Now,use the relation P1V1÷T1=P2V2÷T2

Answer 2

Answer: The pressure when the volume and temperature has changed is $2.10\times 10^3bar$

Explanation:

To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law. The equation follows:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1,V_1\text{ and }T_1$ are the initial pressure, volume and temperature of the gas

$P_2,V_2\text{ and }T_2$ are the final pressure, volume, temperature of the gas

We are given:

$P_1=0.5bar\\V_1=1.1L\\T_1=40^oC=[273+40]K=313K\\P_2=?bar\\V_2=0.225mL=0.225\times 10^{-3}L\\T_2=-4^oC=[273-4]K=269K$

Putting values in above equation, we get:

$\frac{0.5bar\times 1.1L}{313K}=\frac{P_2\times 0.225\times 10^{-3}L}{269K}\\\\P_2=\frac{0.5\times 1.1\times 269}{313\times 0.225\times 10^{-3}}=2.10\times 10^3bar$

Hence, the pressure when the volume and temperature has changed is $2.10\times 10^3bar$