Question

A certain mass of nitrogen gas occupies a volume of 4.67 L 4.67 L at a pressure of 4.94 bar 4.94 bar . Calculate the pressure of the sample if the volume is increased to 7.05 L 7.05 L . Assume constant temperature and ideal gas behavior.

Answer 1

Answer : The final pressure of gas is, 3.27 bar.

Explanation :

Boyle's Law : It is defined as the pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$

or,

$P_1V_1=P_2V_2$

where,

$P_1$ = initial pressure = 4.94 bar

$P_2$ = final pressure = ?

$V_1$ = initial volume = 4.67 L

$V_2$ = final volume = 7.05 L

Now put all the given values in the above equation, we get:

$4.94bar\times 4.67L=P_2\times 7.05L$

$P_2=3.27bar$

Therefore, the final pressure of gas is, 3.27 bar.