Answer: [tex]147 kPa[/tex]
Explanation:
According to Boyle's law, which mathematically describes the thermodynamic process in which the pressure of a gas has the tendency to increase as the volume of the container decreases, we have:
[tex]P_{1}V_{1}=P_{2}V_{2}[/tex] (1)
Where:
[tex]P_{1}=98kPa=98000 Pa[/tex] is the initial pressure of Helium (He)
[tex]V_{1}=500 mL=500(10)^{-3}L[/tex] is the initial volume of Helium (He)
[tex]V_{2}=750 mL=750(10)^{-3}L[/tex] is the final volume of Helium (He)
[tex]P_{2}[/tex] is the final pressure of Helium (He)
Now, we need to isolate [tex]P_{2}[/tex] from (1):
[tex]P_{2}=\frac{P_{1}V_{1}}{V_{2}}[/tex] (2)
[tex]P_{2}=\frac{(98000 Pa)(500(10)^{-3}L)}{750(10)^{-3}L}[/tex] (3)
Finally:
[tex]P_{2}=147000 Pa=147 kPa[/tex] This is the final pressure of Helium
