at 2 atm of pressure the volume of a ballon is 4.7 L. Assuming that the temperature remains constant, what will the volume of the ballon be at 1 atm of pressure?.
P1V1 = P2V2
To find the volume of the balloon at 1 atm of pressure, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when the temperature remains constant.
Boyle's Law equation is as follows:
P1 * V1 = P2 * V2
Where:
P1 is the initial pressure
V1 is the initial volume
P2 is the final pressure (1 atm in this case)
V2 is the final volume (what we need to find)
Given:
P1 = 2 atm
V1 = 4.7 L
P2 = 1 atm
We can rearrange the equation to solve for V2:
V2 = (P1 * V1) / P2
Substituting the given values:
V2 = (2 atm * 4.7 L) / 1 atm
V2 = 9.4 L
Therefore, the volume of the balloon at 1 atm of pressure will be 9.4 L.