What pressure will be exerted by 2.01 mol hydrogen gas in a 6.5 l cylinder at 20 c?

Answer 1

You can answer this question using the ideal gas law: PV=nRT.

P = Pressure

V = volume

n = Number of moles

R = Real Gas Constant (with units equal to the PV and T you are using)

T = Temperature

In your problem, you want to solve for P, so the equation would read

P=(nRT)/V

This would look like

P = (2.01moles)(8.314 J/mol K)(273K+20K)/6.5L

After the units cancel, this leaves you with 753 J/L, which can be converted. For example:

1 J = 1 Pa m^3, which is equal to 1000 Pa L

So 753 J/L = 753,000 Pa L / L. Liters cancels so you are left with 7530 hPa (753000 Pa)

This is roughly 7 atm.