Kp = pA*pB = 4.
I would let pA = p which means pB = p and solve for p.
Kp = Kc(RT)delta n
Could you please explain what you wrote above? Like can you replace all the constants with the numbers given so I get what you are saying...Thanks! Also how will I find the equilibrium pressure and Kc?
And how do I solve for p? I'm confused :(
Kp = 4 = partial pressure of A x partial pressure of B
4 = p^2
partial pressure A = 2 atm at eqilibrium.
partial pressure of B = 2 atm at equilibrium.
Kp = Kc(RT)delta n
You know Kp and you know R and T. You can calculate delta n (it's mols reactants - moles products = 2-0=2)
Note that Kp = pA*pB and does NOT (repeat NOT) include AB since it is a solid.
So is this right:
Also what is the answer to this part of the question:
What is the equilibrium pressure of A(g) and B(g) above AB(s) at 300 K?
Kc is right but you worked it wrong.
It's 4 = Kc*(0.08206*300)^2
What do you not understand about partial pressure? Do you know what that means? I have posted the equilibrium partial pressures for both A and B in all of my responses but you continue to ask what is the answer.
Ohh I'm sorry I didn't see that! Sorry for the mishap :( I really appreciate your help!
Hey, I just wanted to help and point out that delta n = moles of gaseous products - moles of gaseous reactants according to my chem lecture.
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