Respuesta :
a. 327.5 mm Hg, b. 26.2 mm Hg, c. 4,366.7 mm Hg
Explanation:
We can use the Boyle's law to find the new pressure.
P₁V₁ = P₂V₂
Now P₁ = 655 mm Hg
V₁ = 10 L
V₂ = 20 L
[tex]P_{2}=\frac{P_{1} V_{1}}{V_{2}}[/tex]
Plugin the values in the equation, we will get the new pressures as,
a. [tex]P_{2}=\frac{10 L \times 655 \mathrm{mm} \mathrm{Hg}}{20 \mathrm{L}}=327.5 \mathrm{mm} \mathrm{Hg}[/tex]
b. [tex]P_{2}=\frac{10 L \times 655}{250 L}=26.2 \mathrm{mm} \mathrm{Hg}[/tex]
c.[tex]P_{2}=\frac{10 L \times 655}{1.5 L}=4,366.7 \mathrm{mm} \mathrm{Hg}[/tex]
The pressure at 20L volume has been 327.5 mm Hg, at 250 L volume has been 26.2 mm Hg, and at 1500 ml has been 4,366.6 mm Hg.
The ideal gas equation helps in the determination of the pressure of the gas at constant temperature and volume.
The ideal gas equation can be given by:
PV=nRT
When V and n are constant. The relationship between the initial and final can be given by:
P1V1 = P2V2
P1 and V1 are the initial pressure and temperature, and P2 and V2 are the final pressure and temperature.
Given, P1 = 655 mm Hg, V1 = 10 L
(a) V2 = 20 L
655 [tex]\times[/tex] 10 = P2 [tex]\times[/tex] 20
P2 = 327.5 mm Hg.
(b) V2 = 250 L
655 [tex]\times[/tex] 10 = P2 [tex]\times[/tex] 250
P2 = 26.2 mm Hg
(c) V2 = 1500 ml
V2 = 1.5 L
655 [tex]\times[/tex] 10 = P2 [tex]\times[/tex] 1.5
P2 = 4,366.6 mm Hg
For more information about the pressure of the gas, refer to the link:
https://brainly.com/question/14696697
