What is the relationship between the equilibrium constants Kp and Kc for a gaseo
Practice Questions
Q1
What is the relationship between the equilibrium constants Kp and Kc for a gaseous reaction?
Kp = Kc
Kp = Kc(RT)^(Δn)
Kp = Kc/RT
Kp = Kc(RT)^(Δn) where Δn is the change in moles of gas
Questions & Step-by-Step Solutions
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.
