According to Boyle's Law , the pressure of an ideal gas varies inversely with its volume. However, when I blow a balloon, both the pressure and volume increase and lead it to a contradiction. Why would this happen?
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P ∝ V 1 only when the right hand side of the Ideal Gas Equation is constant.
In other words,
Since P V = n R T , then,
For P ∝ V 1 , we want,
n R T = K
Thus,
Assuming the Temp. doesn't change,
n = no. of moles = K
But, while blowing air into the balloon, we increase the quantity of air inside it, and therefore, n is not constant, i.e the mass of the gas is not fixed.
This would lead us to think that Boyle's Law is violated.