How Does Temperature and Pressure Affect Balloon Volume?

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The discussion focuses on how temperature and pressure changes affect the volume of a balloon filled with air. It uses the ideal gas law to derive the new volume when the balloon is taken outdoors, where the temperature drops and pressure is halved. Participants seek to determine the initial pressure at 296.5 K based on standard temperature and pressure (STP) conditions. The conversation also touches on the constancy of moles during the process and how this information can be applied to find initial and final moles. The thread emphasizes the importance of understanding these gas law relationships in practical scenarios.
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A balloon is filled up with air to a volume of 1.15 L at 296.5 K.* What does the volume change to if the balloon is taken outdoors where the temperature is 278.4 K and the pressure is half of what it was indoors?

V2 = (P1V1T2) / (T1P2)


How do I find the initial pressure at 296.5 K if I know that at STP the pressure is 760 mm Hg at 273.15 K?
 
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v3ra said:
A balloon is filled up with air to a volume of 1.15 L at 296.5 K.* What does the volume change to if the balloon is taken outdoors where the temperature is 278.4 K and the pressure is half of what it was indoors?

V2 = (P1V1T2) / (T1P2)


How do I find the initial pressure at 296.5 K if I know that at STP the pressure is 760 mm Hg at 273.15 K?

What remains constant in the process? Pressure, temperature, volume or moles?

If P is the initial pressure, what's the final pressure?
 
The moles would remain constant... how does this help me?
 
v3ra said:
The moles would remain constant... how does this help me?

Right! So what are the initial moles and final moles? Write the expressions. Do not evaluate.
 
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