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Monica [59]
3 years ago
11

1. A helium-filled balloon had a volume of 8.50 L on the ground at 20.0°C and a

Chemistry
1 answer:
maw [93]3 years ago
5 0

Answer:

133.74 L

Explanation:

First we <u>convert the given pressures and temperatures into atm and K</u>, respectively:

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

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

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

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

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