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A sample of nitrogen gas has a volume of 478 cm3 and a pressure of 104.1 kPa. What volume would the gas occupy at 88.2 kPa if the temperature remains constant?

Respuesta :

Answer:

[tex]564 cm^3[/tex]

Explanation:

First we propose the ideal gas equation for each situation

[tex]P.V=n.R.T[/tex]

Situation 1

[tex]P_1.V_1= n. r.T[/tex]

[tex]P_1= 104.1 KPa \\V_1= 478 cm^3[/tex]

Situation 2

[tex]P_2.V_2= n. r.T\\P_2= 82.2 KPa \\V_2= ?[/tex]

R is a constant, the moles remain constant and also the temperature

Therefore we can say that

[tex]P_1.V_1= P_2.V_2[/tex]

We cleared the volume in situation number two

[tex]P_1.V_1= P_2.V_2\\V_2= \frac{P_1.V_1}{P_2}[/tex]

[tex]V_2= \frac{104.1 KPa. 478cm^3}{88.2 KPa}\\V_2= 564 cm^3[/tex]

Eduard22sly

The volume of the gas at 88.2 KPa is 564 cm³

Data obtained from the question

•Initial volume (V₁) = 478 cm³

•Initial pressure (P₁) = 104.1 KPa

•Temperature = Constant

•Final pressure (P₂) = 88.2 KPa

•Final volume (V₂) =?

Since the temperature is constant, the final volume of the gas can be obtained by using the Boyle's law equation as shown below:

P₁V₁ = P₂V₂

104.1 × 478 = 88.2 × V₂

49759.8 = 88.2 × V₂

Divide both side by 88.2

V₂ = 49759.8 / 88.2

V₂ = 564 cm³

Learn more about gas laws:

https://brainly.com/question/6844441

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