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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.

Respuesta :

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.

[tex]P\propto \frac{1}{V}[/tex]

or,

[tex]P_1V_1=P_2V_2[/tex]

where,

[tex]P_1[/tex] = initial pressure = 4.94 bar

[tex]P_2[/tex] = final pressure = ?

[tex]V_1[/tex] = initial volume = 4.67 L

[tex]V_2[/tex] = final volume = 7.05 L

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

[tex]4.94bar\times 4.67L=P_2\times 7.05L[/tex]

[tex]P_2=3.27bar[/tex]

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

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