Inflating a balloon requires more pressure than the pressure of the atmosphere outside of the balloon, in order to compensate for the stretchiness of the balloon’s material. Would you need more or less gas to compensate? (Hint: Consider the ideal gas law equation. How does n need to change to increase P?)
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According to the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
In this case, we are inflating a balloon, which means we are increasing the volume while keeping the temperature relatively constant. To compensate for the stretchiness of the balloon's material, we need to increase the pressure inside the balloon.
If we increase the pressure (P) while keeping the volume (V) and temperature (T) constant, we can see from the ideal gas law equation that we will need to increase the number of moles (n) of gas.
Therefore, to compensate for the stretchiness of the balloon's material and achieve a higher pressure inside the balloon, we would need to add more gas (increase the number of moles, n).
To determine whether more or less gas is needed to compensate for the increased pressure in inflating a balloon, we need to consider the ideal gas law equation.
The ideal gas law equation is:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles of gas
R = Ideal gas constant
T = Temperature in Kelvin
In this scenario, the pressure inside the balloon is higher than the pressure of the atmosphere outside the balloon. To compensate for the increased pressure, we need to increase the number of moles of gas (n) while keeping the volume (V) constant. This can be achieved by using more gas.
Therefore, to compensate for the increased pressure, you would need more gas.