A sample of oxygen that occupies 1.00 x 10^6 mL at 575 mm Hg is subjected to a pressure of 1.20 atm. What will the final volume of the sample be if the temperature is held constant?
9 years ago
9 years ago
605263.15ML
8 years ago
630,482.46ml
11 months ago
To solve this problem, we can use Boyle's Law, which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume, as long as the temperature remains constant.
Boyle's Law formula: P₁V₁ = P₂V₂
Given:
Initial pressure (P₁) = 575 mm Hg
Initial volume (V₁) = 1.00 x 10^6 mL
Final pressure (P₂) = 1.20 atm
We need to find the final volume (V₂).
First, we need to convert the initial pressure from mm Hg to atm:
1 atm = 760 mm Hg
Initial pressure (P₁) = 575 mm Hg ÷ 760 mm Hg/atm = 0.75658 atm (approximately)
Now, we can plug the values into the Boyle's Law equation and solve for the final volume (V₂):
(P₁)(V₁) = (P₂)(V₂)
(0.75658 atm)(1.00 x 10^6 mL) = (1.20 atm)(V₂)
Simplifying the equation:
756,580 mL•atm = 1.20 atm • V₂
Dividing both sides of the equation by 1.20 atm:
V₂ = 756,580 mL•atm / 1.20 atm
V₂ ≈ 630,483 mL
Therefore, the final volume of the sample will be approximately 630,483 mL if the temperature is held constant.