Suppose that a sample of gas occupies 140 mL
of volume at 25�C and a pressure of 252 torr.
What would be the volume if the pressure
were changed to 552 torr at 25�C?
(P1V1/T1) = (P2V2/T2)
To determine the final volume of the gas when the pressure is changed, we can use Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional at constant temperature.
Boyle's Law can be represented by the equation:
P1 * V1 = P2 * V2
where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
In this case, we have:
P1 = 252 torr
V1 = 140 mL
P2 = 552 torr
V2 = unknown (to be determined)
Substituting the given values into the equation, we have:
252 torr * 140 mL = 552 torr * V2
Now, we can solve for V2 by rearranging the equation:
V2 = (252 torr * 140 mL) / 552 torr
Calculating the expression on the right side of the equation gives us:
V2 = 63.23 mL
Therefore, the volume of the gas would be approximately 63.23 mL if the pressure were changed to 552 torr at 25�C.