A sample of helium has a volume of 325mL and a pressure of 655mmHg. What wll be the pressure if the helium is compressed to 125mL (T constant)?
P1v1 =p2v2
1703 mmHg (this one is exact) or 1.70 X 10^3 mmHg (this one has three significant fugures)
To find the new pressure when the helium is compressed to 125 mL, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional if the temperature is constant. Boyle's Law can be expressed as:
P₁V₁ = P₂V₂
where P₁ and V₁ are the initial pressure and volume, and P₂ and V₂ are the final pressure and volume.
In this case, the initial pressure (P₁) is 655 mmHg, and the initial volume (V₁) is 325 mL. The final volume (V₂) is 125 mL, and we need to find the final pressure (P₂).
We can rearrange the equation to solve for P₂:
P₂ = (P₁ * V₁) / V₂
Substituting the given values:
P₂ = (655 mmHg * 325 mL) / 125 mL
P₂ ≈ 1702 mmHg
Therefore, the pressure of the helium when compressed to 125 mL would be approximately 1702 mmHg.