A balloon at a pressure of 755 torr and a volume of 5.00 L was allowed to rise in the atmosphere to a point at which the pressure inside and outside the balloon was 697 torr. What was the volume of the balloon at that altitude, assuming the temperature was constant?
P1V1 = P2V2
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756
To solve this problem, we can use Boyle's Law, which states that the product of pressure and volume is constant at constant temperature.
Boyle's Law equation: P1 * V1 = P2 * V2
Where:
P1 = initial pressure (755 torr)
V1 = initial volume (5.00 L)
P2 = final pressure (697 torr)
V2 = final volume (unknown)
To find the final volume (V2), we can rearrange Boyle's Law equation:
V2 = (P1 * V1) / P2
Now we can substitute the known values into the equation:
V2 = (755 torr * 5.00 L) / 697 torr
Using a calculator, we can find:
V2 = 5.43 L (rounded to two decimal places)
Therefore, the volume of the balloon at that altitude is approximately 5.43 L.