What is the relationship between the equilibrium constants Kp and Kc for a gaseo

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Question: What is the relationship between the equilibrium constants Kp and Kc for a gaseous reaction?

Options:

Correct Answer: Kp = Kc(RT)^(Δn)

Solution:

The relationship between Kp and Kc is given by Kp = Kc(RT)^(Δn), where Δn is the change in the number of moles of gas.

What is the relationship between the equilibrium constants Kp and Kc for a gaseous reaction?

What is the relationship between the equilibrium constants Kp and Kc for a gaseous reaction?

Step 1: Understand that Kp and Kc are both equilibrium constants for chemical reactions involving gases.
Step 2: Kp is used when dealing with partial pressures of gases, while Kc is used when dealing with concentrations of gases.
Step 3: Identify Δn, which is the change in the number of moles of gas during the reaction. It is calculated as (moles of gaseous products) - (moles of gaseous reactants).
Step 4: Use the formula Kp = Kc(RT)^(Δn) to relate Kp and Kc, where R is the ideal gas constant and T is the temperature in Kelvin.
Step 5: Remember that this relationship shows how Kp and Kc are connected through the change in moles of gas and the conditions of the reaction.

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