Pressure help: I cannot solve this problem - Help.com

does this link help at all

http://www.freepatentsonline.com/3787…

or did i just make it worse?

http://www.physicsforums.com/showthre… wrote:
what i know: when you double volume, pressure is halved and le chatliers principle says the equation will shift to the side with more moles of gas

Nor can I.

1) Write down the equilibrium equation. In this case,
N2(g) + 3H2(g) -> 2NH3(g)
Which means 1 mol nitrogen gas (N2) with 3 moles hydrogen gas (H2) makes 2 moles ammonia gas.

2) State the values you’ve been given so far, ie:
Temperature: 500 C
Pressure: 300 atm
Ratio N2:H2 = 1:3
Partial pressure NH3: 10%
And that means the partial pressure of ammonia in that system is 10% x 300 atm = 30 atm, therefore partial pressures of N2 and H2 = 300 - 30 = 270 atm.

3) N2 and H2 exist in a ratio of 1:3. Soooo, divide the 270 atm between the 2 gases in that ratio?

I think that’s it, I haven’t done this for awhile xD But I remember some law states that:
Total pressure = Partial pressure gas 1 + PP gas 2 + PP gas 3 etc…

67.5???

F.anjel wrote:
1) Write down the equilibrium equation. In this case,
N2(g) + 3H2(g) -> 2NH3(g)
Which means 1 mol nitrogen gas (N2) with 3 moles hydrogen gas (H2) makes 2 moles ammonia gas.

2) State the values you’ve been given so far, ie:
Temperature: 500 C
Pressure: 300 atm
Ratio N2:H2 = 1:3
Partial pressure NH3: 10%
And that means the partial pressure of ammonia in that system is 10% x 300 atm = 30 atm, therefore partial pressures of N2 and H2 = 300 - 30 = 270 atm.

3) N2 and H2 exist in a ratio of 1:3. Soooo, divide the 270 atm between the 2 gases in that ratio?

I think that’s it, I haven’t done this for awhile xD But I remember some law states that:
Total pressure = Partial pressure gas 1 + PP gas 2 + PP gas 3 etc…

but your way is probably right… i dunno what the answer would be that way though…

I’m not sure if I AM actually right, but it’s making sense to me so far, since there’s no changes in temperature or pressure that I can see…