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.

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

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

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.

sry but any answer choices

it means there are 3 atoms of oxygen