[amoralyn12]

Hi, I've been working on this free response question, but I'm unsure if I'm doing it right. I'll post the first parts that I have done first, and continue editing when I have gone further into the question. Please tell me if I am doing things correctly, or if not, tell me what I am doing wrong and how to fix it. Thanks.

Here's the question: A mixture of 0.300 mol each of hydrogen gas, oxygen gas, and liquid water are present in a 20.00 liter container at 25 degrees Celsius. The equilibrium vapor pressure of water at 25 degrees Celsius is 23.76 torr.

(a) Calculate the total pressure inside the flask.

I used the ideal gas law to find the partial pressure of the gases, PV=nRT and modified it to become P=(nRT)/V
n= 0.600 mol of gases
R= 0.08206 L atm / mol K
T= 298 K
V= 20.00 L

(0.600)(0.08206)(298) / 20.00 = 0.73 atm

Then I added the vapor pressure of water,
P= (23.76 torr)(1 atm/760 torr)= 0.3 atm
0.73 atm+0.3 atm= 0.76 atm

(b) Using principles of kinetic molecular theory, explain which gas has the
  highest average kinetic energy
The kinetic molecular theory states that at any given temperature, the molecules of all gases have the same average kinetic energy.
  highest average velocity of molecules
For this reason, the gas with the smallest mass will have the highest average velocity of molecules (hydrogen gas).
  highest density
The oxygen gas will have the highest density because it has a larger atomic mass than hydrogen, meaning that at equal moles the oxygen will have more oxygen atoms.

I'm really not sure of this next part...

(c) The mixture is sparked, a reaction ensues consuming one of the reactants entirely, and the resulting mixture is allowed to come to equilibrium at 80 degrees Celsius.
  Write and balance a chemical equation to describe the reaction.
I'm have a lot of problems with chemical equations. How can I predict the products?
H_2(g)+O_2(g)+H₂O_(l)  2H₂O_(g)+H⁺
  Which is the limiting reactant? Explain.
I would guess that oxygen is the limiting reactant. However, it is only a guess and I have no explanation.
  Calculate the total pressure in the flask after the reaction is complete. The water vapor pressure at 80 degrees Celsius is 355 torr.
Working...

[Borek]

Water that is initially present doesn't take part in the reaction. Try just reaction between hydrogen and oxygen.

[kimyacı]

 İn fact,even at the begining this reaction begin, but very very slow.Because of its very much activation energy, Light or a metal catalyst is needed to occur reaction fast.