The molar constant (Kc), partial pressure (Kp) values should be calculated and understand the equilibrium process of the given equilibrium constant (Kp) at 25 0 C. Concept Introduction: Equilibrium constant: The respective values of K depend on whether the solution being calculated for is using concentration (or) partial pressure. The gas equilibrium constant related to the equilibrium (K) and both are derived from the ideal gas. Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures. Kp and Kc: This equilibrium constants of gaseous mixtures, these difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system. Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

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Chapter 15, Problem 15.60QP

Interpretation Introduction

Interpretation:

The molar constant (Kc), partial pressure (Kp) values should be calculated and understand the equilibrium process of the given equilibrium constant (Kp) at 25⁰C.

Concept Introduction:

Equilibrium constant: The respective values of K depend on whether the solution being calculated for is using concentration (or) partial pressure. The gas equilibrium constant related to the equilibrium (K) and both are derived from the ideal gas.

Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.

Kp and Kc: This equilibrium constants of gaseous mixtures, these difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system.

Heterogeneous equilibrium: This equilibrium reaction does not depend on the amounts of pure solid and liquid present, in other words heterogeneous equilibrium, substances are in different phases.

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