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Art [367]
2 years ago
8

A gas sample has a volume of 30.0 mL at a pressure of 1.53 atm. If the volume increases to 50.1 mL and the temperature remains c

onstant, the new pressure in atms will be
Chemistry
1 answer:
Tems11 [23]2 years ago
6 0

At constant temperature, if the volume of the sample of gas increases to the given value, the pressure decreases to 0.92atm.

<h3>Boyle's law</h3>

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 = 30.0mL = 0.03L
  • Initial pressure of the gas P₁ = 1.53atm
  • Final volume of the gas V₂ = 50.1mL = 0.0501L
  • Final pressure of the gas P₂ = ?

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

P₁V₁ = P₂V₂

P₂ = P₁V₁ / V₂

P₂ = ( 1.53atm × 0.03L ) / 0.0501L

P₂ = 0.0459Latm / 0.0501L

P₂ = 0.92atm

Therefore, at constant temperature, if the volume of the sample of gas increases to the given value, the pressure decreases to 0.92atm.

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

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