A gas occupying a volume of 806 mL at a pressure of 0.970 atm is allowed to expand at constant temperature until its pressure reaches 0.541 atm. What is its final volume?
P1V1=P2V2
solve for V2
To find the final volume, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature. The equation for Boyle's Law is:
P1 * V1 = P2 * V2
Where:
- P1 and P2 are the initial and final pressures, respectively
- V1 and V2 are the initial and final volumes, respectively
We are given:
P1 = 0.970 atm
V1 = 806 mL = 0.806 L
P2 = 0.541 atm
Plugging these values into the equation, we can solve for V2:
0.970 atm * 0.806 L = 0.541 atm * V2
Cross-multiplying:
0.78182 L.atm = 0.541 atm * V2
Dividing both sides by 0.541 atm:
V2 = 0.78182 L.atm / 0.541 atm
Simplifying:
V2 ≈ 1.442 L
Therefore, the final volume of the gas is approximately 1.442 L.