The Volume of air in a car tire is 800cm^3 and the pressure is 290kPa.
Determine the volume the air would occupy as soon as the tire bursts on a day when the atmospheric pressure is 102kPa.
(Assume that the temperature remains constant and assume an ideal gas)
The pressure goes from 290 to 102 kPa.
V=800cm^3*290/102
To determine the volume the air would occupy when the tire bursts, we can use Boyle's Law and the Ideal Gas Law.
Boyle's Law states that the pressure and volume of a gas are inversely proportional when the temperature remains constant. Mathematically, it can be written as:
P1 * V1 = P2 * V2
Where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.
In this case, we know the initial volume and pressure (V1 = 800 cm^3 and P1 = 290 kPa) and the final pressure (P2 = 102 kPa). Our goal is to find the final volume (V2).
Rearranging Boyle's Law equation to solve for V2, we have:
V2 = (P1 * V1) / P2
Now we can substitute the given values into the equation:
V2 = (290 kPa * 800 cm^3) / 102 kPa
V2 = 2256 cm^3
Therefore, the volume the air would occupy as soon as the tire bursts on a day when the atmospheric pressure is 102 kPa is 2256 cm^3.