1. A helium-filled balloon had a volume of 8.50 L on the ground at 20.0°C and a pressure of 750.0 Torr. After the balloon was released, it rose to an altitude where the
temperature was 40.0°C and the pressure was .550 atm. What is the new volume of
the balloon in liters at the high altitude?

133.74 L

Explanation:

First we convert the given pressures and temperatures into atm and K, respectively:

750.0 Torr ⇒ 750/760 = 0.9868 atm20°C ⇒ 20+273.16 = 293.16 K40°C ⇒ 40+273.16 = 313.16 K

Then we use the PV=nRT formula to calculate the number of moles of helium in the balloon, using the data of when it was on the ground:

0.9868 atm * 8.50 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 293.16 Kn = 2.866 mol

Then, knowing the value of n, we use PV=nRT once again, this time to calculate V using the data of when the balloon was high up:

0.550 atm * V = 2.866 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 313.16 KV = 133.74 L

If it releases 5 tons a day and there are 7 days a take that answer and multiply by 5 percent (0.05) to find the amount released in one week. leave a comment if you need more .

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