A weather balloon is filled with helium that occupies a volume of 5.27 10^4 L at 0.995 atm and 32.0°C. After it is released, it rises to a location where the pressure is 0.720 atm and the temperature is - 12.7°C. What is the volume of the balloon at that new location?

Question

Chemistry

Caiden Orozco

25 October, 02:26

A weather balloon is filled with helium that occupies a volume of 5.27 10^4 L at 0.995 atm and 32.0°C. After it is released, it rises to a location where the pressure is 0.720 atm and the temperature is - 12.7°C. What is the volume of the balloon at that new location?

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Alison Levy · Answer 1

Ideal gas law:

pv = nrt

nr is mole times the ideal gas constant, these are both held constant (do not change value)

pv/t = nr

Then you can set the conditions before = after

pv/t = PV/T

before: (convert to Kelvin)

(0.995) (5.27x10^4) / 305

After: (convert to Kelvin)

(0.720) V / 206.3

solve for V, volume after.

(0.995) (5.27x10^4) / 305 = (0.720) V / 206.3

4.926 x 10^4 L = V