Question

A large balloon contains 1.00 mol of helium in a volume of 22.4 L at 0.00oC. What pressure will the helium exert on its container? Give your answer in atm and in mmHg.

Answer 1

The pressure exerted by helium on the walls of the container is approximately 760.6 mmHg

Step-by-step explanation:

The parameters given in the question are;

Amount of moles of helium in balloon = 1.00 mole

Volume of balloon = 22.4 L = ‪0.0224 m³

Temperature of balloon = 0.00°C = 273.15 K

Therefore, we have the pressure given by the universal gas equation as follows;

P·V = n·R·T

So that

`P = (nRT)/(V) = (1 * 8.3145 * 273.15)/(0.0224 ) = 101388.646 \ Pa`

Converting the resultant pressure in pascals, Pa to millimetre mercury, mmHg we have;

1 mmHg = ‪133.3 Pa

∴ 1 Pa = 1/133.33 mmHg and

101388.646 Pa = 101388.646× 1/133.3 mmHg = ‪760.604996 mmHg

Therefore the pressure exerted by helium on the container ≈ 760.6 mmHg.