A sample of carbon dioxide occupies a volume of 1.50L at 165kPa pressure. What pressure would the gas exert if the volume was increased to 2.5L?
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A sample of carbon dioxide occupies a volume of 1.50L at 165kPa pressure. What pressure would the gas exert if the volume was increased to 2.5L?
To find the pressure of the gas when the volume is increased, we can use Boyle's Law. Boyle's Law states that the pressure and volume of a gas are inversely proportional when the temperature is constant.
The equation for Boyle's Law is:
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, the initial volume (V1) is 1.50 L, the initial pressure (P1) is 165 kPa, and the final volume (V2) is 2.5 L. We need to find the final pressure (P2).
Substituting the values into the equation:
165 kPa * 1.50 L = P2 * 2.5 L
Rearranging the equation to solve for P2:
P2 = (165 kPa * 1.50 L) / 2.5 L
P2 = 99 kPa
Therefore, the gas would exert a pressure of 99 kPa if the volume was increased to 2.5 L.
Remember to always double-check the units and make sure they are consistent throughout the calculation.