Ideal Gas Law Question: Calculating Final Balloon Volume at High Altitude

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To calculate the final volume of a helium balloon at high altitude using the Ideal Gas Law, the initial conditions of 1.00 L, 23°C, and 1.00 atm must be converted to appropriate units. The pressure at altitude is given as 220 torr, which is approximately 0.29 atm. Using the combined gas law, the relationship between initial and final states can be applied without needing to determine the number of moles. The final volume can be calculated directly from the initial volume and the changes in temperature and pressure. The final volume of the balloon at the new altitude and temperature can be determined using these values.
blackjack18
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A sealed balloon is filled with 1.00 L of He gas at 23 deg C and 1.00 atm. The balloon rises to a point in the atmosphere where the pressure is 220 torr and the temperature is -31 deg C. What is the final volume of the balloon after it reaches an altitude where the pressure is 220 torr?

If I should use the Ideal Gas Law, Pv= nRT, how do I find the number of moles?
 
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blackjack18 said:
A sealed balloon is filled with 1.00 L of He gas at 23 deg C and 1.00 atm. The balloon rises to a point in the atmosphere where the pressure is 220 torr and the temperature is -31 deg C. What is the final volume of the balloon after it reaches an altitude where the pressure is 220 torr?

If I should use the Ideal Gas Law, Pv= nRT, how do I find the number of moles?

You are not asked for the number of moles. (Hint: You don't need it either.)

https://www.physicsforums.com/showpost.php?p=1914382&postcount=14
 
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