Kp for heterogeneous Equilibria (with (l))

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In summary, the conversation discusses the relationship between Kp and Kc for a chemical reaction, specifically whether Kp exists for reactions with reactants or products in aqueous or liquid form. The use of the Law of Mass Action and the equation Kp=Kc(RT)Δng is mentioned. The question is posed whether the activities of reactants and products can be written as functions of pressure (fugacity) and whether Kc for the reaction of HCl exists. The speaker expresses a lack of knowledge in chemistry and a desire to learn more.
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Homework Statement


3Cu(s) + 2NO3-(aq) + 8H+(aq) ⇔3Cu2+(aq) + 2NO(g) + 4H2O(l)
Kp and Kc relationship? does Kp exist?
or HCl(g)⇔H+(aq)+Cl-(aq)

Homework Equations


Law of mass action, Kp=Kc(RT)Δng

The Attempt at a Solution


In lots of places contradictory results are there, some say that in Kp , (not clearly signifying presence of liquid state) that just take gaseous moles, and in some, Kp doesn't exist..we know that solvent and solid state can be ignored in all K .. Does Kp exist for a reaction including a reactant/product in aqueous or liquid form? (im not asking about thermodynamical constant which is quite crystal clear in definition by acivity)
 
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ELiT.Maxwell said:
Does Kp exist for a reaction including a reactant/product in aqueous or liquid form? (im not asking about thermodynamical constant which is quite crystal clear in definition by acivity)
Can you write activities of reactants and products as functions of P (fugacity)?
 
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if we assume ideal behaviour and remove concept of activity (by taking the measurement of species in bar and M) ..
a simple answer in yes or no would suffice... and 2nd part of question was whether Kc of Hcl reaction exists too
[sorry for my lack of knowledge in chemistry in general, that's why I am going back to strengthen my roots]
 

1. What is Kp for heterogeneous equilibria?

Kp (equilibrium constant for partial pressures) is a thermodynamic quantity that measures the ratio of products to reactants at equilibrium for a heterogeneous chemical reaction. It is expressed in terms of partial pressures and is a measure of the extent to which a reaction proceeds towards products.

2. How is Kp calculated for heterogeneous equilibria?

Kp is calculated by taking the partial pressures of the products raised to their respective stoichiometric coefficients and dividing it by the partial pressures of the reactants raised to their respective stoichiometric coefficients. The resulting expression is then simplified using the ideal gas law to obtain a numerical value for Kp.

3. What is the significance of Kp for heterogeneous equilibria?

Kp is important because it provides information about the position of equilibrium for a heterogeneous reaction. A large Kp value indicates that there are more products present at equilibrium, while a small Kp value indicates that there are more reactants present at equilibrium.

4. How does temperature affect Kp for heterogeneous equilibria?

According to Le Chatelier's principle, an increase in temperature will shift the equilibrium towards the endothermic direction, resulting in an increase in Kp. On the other hand, a decrease in temperature will shift the equilibrium towards the exothermic direction, leading to a decrease in Kp.

5. Can Kp be used to predict the direction of a heterogeneous reaction?

Yes, Kp can be used to predict the direction of a heterogeneous reaction. If the calculated Kp value is greater than the given Kp value, the reaction will proceed towards products. If the calculated Kp value is less than the given Kp value, the reaction will proceed towards reactants. If the calculated Kp value is equal to the given Kp value, the reaction is at equilibrium.

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