Answered

Looking for answers? Westonci.ca is your go-to Q&A platform, offering quick, trustworthy responses from a community of experts. Get immediate and reliable answers to your questions from a community of experienced experts on our platform. Experience the ease of finding precise answers to your questions from a knowledgeable community of experts.

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

nuhulawal20

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

#SPJ5

Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. We appreciate your time. Please revisit us for more reliable answers to any questions you may have. Discover more at Westonci.ca. Return for the latest expert answers and updates on various topics.