Calculating Volume of Helium Balloon at Different Temperatures

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To calculate the volume of a helium balloon at different temperatures, start by applying the ideal gas law using the initial conditions of 9.9 g of liquid helium at 4.20 K and 1.00 atm pressure. Determine the density of helium at 4.2 K to find its volume, which serves as the baseline for further calculations. Use the relationship V1/T1 = V2/T2 to find the volumes at the specified temperatures of 23.0 K and 299 K. This approach allows for the calculation of volume changes with temperature while maintaining constant pressure. Understanding these principles is essential for solving the problem accurately.
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Question from my homework. I'm not exactly sure what I am doing wrong, and it is bugging me. I hope this post is in the right forum.

Imagine that 9.9 g of liquid helium, initially at 4.20 K, evaporate into an empty balloon that is kept at 1.00-atm pressure. What is the volume of the balloon at the following?
(a) 23.0 K (b) 299 K

After missing the question, help was given, but I can't make sense of it:

Apply the ideal-gas law to find the volume of the gas at 4.2 K, and a fixed amount of gas to find its volume at the given temperatures.
 
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you must have the density at 4.2 the you can calculate the volume at 4.2 . then you can calculate the volume at the other temperatures from the equation
V1/T1=V2/T2=V3/T3=...=Vn/Tn
 
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