I'm doing chemical equilibrium, and there's a question in my lecture notes. Can someone check my answers and tell me if i'm right or wrong? Thanks!
The Kc expression for this reversible reaction:
3Fe(s) + 4H2O (g) --><-- Fe3O4(s) + 4H2 (g)
is [H2]^4 / [H2O]^4
Am I correct? My lecture notes apparently said that the reaction has a Kp expression but it didn't say anything about Kc expression. I just thought it can also have a Kc expression, not sure if i'm right.
And this one too! I thought it should also have a Kc expression but my notes only mentioned the Kp expression:
( that weird arrow is the forward backward arrow for a reversible reaction)
H2(g) + Br2(l) --><-- 2HBr2(g)
Kc = [HBr]^2 / [Br][H2]
Please tell me if im right! I reasoned that there should be a Kc expression since for Kc expressions you should exclude water (when used as a solvent) and solids, so i thought that's applicable for these equations...
please help thanks!
What is included in the Kp expression - partial pressures of the components.
The partial pressure of a solid does not change, so does not appear in Kp. This is the same with Kc as solids do not appear in Kc.
Liquids do not appear in Kp either.
Um. that does not answer my question of whether liquids, aqueous, and gases appear in Kc expressions or not.
OK
Gases appear in Kc expressions as concentrations.
In aqueous and other solvent systems the solute appears as a concentration in Kc expressions.
Pure materials such as solids and solvents (including water) do not appear in the equilibrium expression.
A substance such as water will of course appear if they are one of the products or reactants. For example in
H2(g)+O2(g)<=> H2O(g)
note the gas phase.
Yes, you are correct! The Kc expression for the reversible reaction you provided is [H2]^4 / [H2O]^4.
For a reversible reaction like this one, it is possible to have both a Kc expression and a Kp expression. The Kc expression is used to represent the equilibrium constant in terms of molar concentrations, while the Kp expression represents the equilibrium constant in terms of partial pressures.
In your case, since you are given the reaction in terms of molar concentrations, you correctly used the Kc expression. The Kc expression is determined by taking the concentrations of the products ([H2]^4) and dividing it by the concentrations of the reactants ([H2O]^4). Therefore, [H2]^4 / [H2O]^4 is the correct Kc expression for this reaction.