To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (assume constant)
V = volume
n = moles of air
R = ideal gas constant
T = temperature (assume constant)
Since air is added to the balloon, the moles of air remain the same (10 moles). Therefore, we can rewrite the equation as:
P1V1 = P2V2
Where:
P1 = initial pressure
V1 = initial volume
P2 = final pressure (assume constant)
V2 = final volume
Rearranging the equation to solve for P2, we get:
P2 = (P1V1) / V2
Let's assume the initial pressure is constant at P1 = 1 atm. Substituting the given values:
P2 = (1 atm * 0.2 m^3) / 0.3 m^3
P2 = 0.67 atm
Therefore, the final pressure inside the balloon is approximately 0.67 atm.
Air is added to a balloon containing 10 moles of air. It increases in size from .2 m3 to .3 m3
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