Question

What volume would a 0.250 mole sample of `H_2` gas occupy, which has a pressure of 17.0 atm, and a temperature of 35°C?

Answer 1

Well, we solve the Ideal Gas equation..........and get approx. a `400*mL` volume.

Explanation:

`PV=nRT`, and so `V=(nRT)/P`

`=(0.250*molxx(0.0821*(L*atm)/(K*mol))xx308*K)/(17.0*atm)`

`=??*L`.

The actual pressure MIGHT be different from the value calculated here, because the pressure is somewhat elevated. At moderate pressures and high temperatures we know that ALL gases exhibit Ideal Gas behaviour.