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A 2.0 L container of oxygen had a pressure of 3.2 atm. What volume would be necessary to decrease the pressure to 1.0 atm?

Use the formula: P1V1 = P2V2

Sagot :

Answer:

V= 6.4 L

Explanation:

P1V1= P2V2

(3.2)(2)=(1)V2

V2= 6.4 L

Nuhulawal20idn

If the pressure of the container of oxygen gas decreases to the given value, the volume increases to 6.4L.

What is Boyle's law?

Boyle's law simply states that "the volume of any given quantity of gas is inversely proportional to its pressure as long as temperature remains constant.

Boyle's law is expressed as;

P₁V₁ = P₂V₂

Where P₁ is Initial Pressure, V₁ is Initial volume, P₂ is Final Pressure and V₂ is Final volume.

Given the data in the question question;

  • Initial volume of the gas V₁ = 2.0L
  • Initial pressure of the gas P₁ = 3.2atm
  • Final pressure of the gas P₂ = 1.0atm
  • Final volume of the gas V₂ = ?

We substitute our given values into the expression above to determine the new volume.

P₁V₁ = P₂V₂

V₂ = P₁V₁ / P₂

V₂ = ( 3.2atm × 2.0L ) / 1.0atm

V₂ = 6.4Latm / 1.0atm

V₂ = 6.4L

Therefore, if the pressure of the container of oxygen gas decreases to the given value, the volume increases to 6.4L.

Learn more about Boyle's law here: brainly.com/question/1437490

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