Final answer:
The relationship between Kp and Kc for gas-phase reactions is Kp = Kc(RT)Δn, where R is the gas constant, T is the temperature in Kelvin, and Δn is the change in moles of gases between the products and reactants.
Step-by-step explanation:
The relationship between Kp (equilibrium constant in terms of partial pressures) and Kc (equilibrium constant in terms of concentrations) is derived from the ideal gas law, which is PV = nRT. For gas-phase reactions, this relationship can be expressed as:
Kp = Kc(RT)Δn
where:
- R is the gas constant.
- T is the temperature in Kelvin.
- Δn is the change in moles of gas between products and reactants.
This equation shows that Kp is related to Kc by a factor that includes the gas constant, the temperature, and the difference in the amount of moles of gaseous products and reactants. To use this formula correctly, one must ensure that all the gases involved comply with the assumptions of the ideal gas law.