Kp only counts with gas molecules, while Kc only counts with aqueous solution + gases. So here both reactant and product are gaseous, so only one reaction with the same number of reactants and products has kp=kc, ie.
Key Difference – Kc vs. Kp
The key difference between Kc and Kp is that Kc is the equilibrium constant given by concentration while Kp is the equilibrium constant given by pressure . This equilibrium constant is given for reversible reactions.
Kp = Kc (RT)
Kc = equilibrium constant is the concentration. T = temperature. ∆ng = difference between the sum of the number of moles of the products and the sum of the number of moles of the reactants in the gas phase. ∴ Kp = KC for the synthesis of HI.
Explanation. Kc and Kp are both equilibrium constants. Kc is measured as the molar concentration of reactants and products, while Kp is measured as the partial pressure of reactants and products.
In which of the following equilibria are Kc and Kp not equal? D. The reaction in which the moles of gaseous products (np) is not equal to the moles of gaseous reactants (nR) has a different value from Kc and Kp.
Answer and explanation: The equilibrium constant cannot be 0. This is because the concentration of products at equilibrium is 0.
Kp and Kc are equilibrium constants of ideal gas mixtures that are considered under reversible reactions. Kp is an equilibrium constant written in terms of atmospheric pressure and Kc is the equilibrium constant used in terms of concentrations expressed in molarity.
The “law of chemical equilibrium” states this. the ratio of concentration product of. Product to product of the concentration of. Reactants, each term raised to the power. their stoichiometric coefficient in a balanced.
Assertion: Kp is always greater than Kc . Reason: The effect of pressure on the reaction rate is greater than the effect of concentration.
Le Chatelier’s principle states: “When an equilibrium is subjected to a change in concentration, pressure, or temperature, the equilibrium shifts in the direction tending to reverse the effect of the change< /b>“. Video explanation.