A mixture of .47 moles of H2 and 3.59 moles of HCl is heated to 2800'C. Calculate the equilibrium partial?

pressure of H2,Cl2,and HCl if the total pressure if 2.00 atm . For the reaction H2(g) + Cl2(g) -----> 2HCl(g)

Kp is 193 at 2800'C

If anyone please help me solve this and if you can please guide me stop by step, i'm really lost.

Answer:
H2 + Cl2 <-----> 2 HCl
initial concentration
0.47. . . .3.59
at equilibrium
0.47-x . . 3.59-x . . . .2x
We have supposed V = 1.0 L
Since delta n = 0 ( 2 - 1 - 1 = 0 ) kp = kc
193 = (2x)^2 / (0.47 -x)(3.59-x)
Solve for x so you know moles HCl , H2 and Cl2 then the partial pressures
woah... that's confusing.

The answers post by the user, for information only, FunQA.com does not guarantee the right.



More Questions and Answers:
  • Bile salt and?
  • How do green flames work on lighters?
  • Find the vapor pressure of an aqueous (water as the solvent) solution in which the mole fraction of Hg...?
  • Name of Fuel? Seed?
  • What is the best way to melt zinc oxide?
  • What gas evolves from benzocaine with addition of sodium carbonate?
  • How much remains?
  • What chemical(s) do they use in diapers to mask odor?
  • What are the parts of the triple beam balance and its uses?