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A quantity of helium gas occupies 5 liters at room temperature and standard atmospheric
pressure (760 mm Hg). If the temperature stays the same, what will be the volume o
the helium if the pressure is increased to 950 mm of mercury?

Sagot :

Asuwafohjamesidn

The new volume of occupied by helium gas when its pressure is increased from 760 mm Hg to 950 mm Hg at an initial volume of 5 L is equal to 4 L.

Boyle's Law

Boyle's law state that at constant temperature, the volume of a fixed mass of gas is directly proportional to its pressure.

To calculate the volume of the helium gas, we use the formula below.

Formula:

P₁V₁ = P₂V₂............. Equation 1

Where:

  • P₁ = Initial pressure
  • V₁ = Initial volume
  • P₂ = Final pressure
  • V₂ = Final volume.

Make V₂ The subject of the equation

  • V₂ = P₁V₁/P₂............... Equation 2

From the question,

Given:

  • P₁ = 760 mm Hg
  • V₁ = 5 L
  • P₂ = 950 mm Hg

Substitute these values into equation 2

  • V₂ = (760×5)/950
  • V₂ = 4 L.

Hence, The new volume of occupied by helium gas when its pressure is increased from 760 mm Hg to 950 mm Hg at an initial volume of 5 L is equal to 4 L.

Learn more about Boyle's law here: https://brainly.com/question/26040104

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