Answer:
The resulting pressure is 3 times the initial pressure.
Explanation:
The equation of state for ideal gases is described below:
[tex]P\cdot V = n \cdot R_{u}\cdot T[/tex] (1)
Where:
[tex]P[/tex] - Pressure.
[tex]V[/tex] - Volume.
[tex]n[/tex] - Molar quantity, in moles.
[tex]R_{u}[/tex] - Ideal gas constant.
[tex]T[/tex] - Temperature.
Given that ideal gas is compressed isothermally, this is, temperature remains constant, pressure is increased and volume is decreased, then we can simplify (1) into the following relationship:
[tex]P_{1}\cdot V_{1} = P_{2}\cdot V_{2}[/tex] (2)
If we know that [tex]\frac{V_{2}}{V_{1}} = \frac{1}{3}[/tex], then the resulting pressure of the system is:
[tex]P_{2} = P_{1}\cdot \left(\frac{V_{1}}{V_{2}} \right)[/tex]
[tex]P_{2} = 3\cdot P_{1}[/tex]
The resulting pressure is 3 times the initial pressure.
