Partial Pressures
If
you have three gases inside of a container, the TOTAL pressure is the
sum of the pressures that each gas would exert if the others weren't
even there.
For
example...
0.1 mol of CH4 in a 1 L container at 298 K exerts 2.445 atm of pressure
0.4 mol of O2 in a 1 L container at 298 K exerts 9.78 atm of pressure
0.7 mol of H2 in a 1 L container at 298 K exerts 17.12 atm of pressure
So, if there was 0.1 mol of CH4, 0.4 mol of O2 and 0.7 mol of H2 in the same 1 L container, the total pressure would be:
0.1 mol of CH4 in a 1 L container at 298 K exerts 2.445 atm of pressure
0.4 mol of O2 in a 1 L container at 298 K exerts 9.78 atm of pressure
0.7 mol of H2 in a 1 L container at 298 K exerts 17.12 atm of pressure
So, if there was 0.1 mol of CH4, 0.4 mol of O2 and 0.7 mol of H2 in the same 1 L container, the total pressure would be:
