The partial pressure of CO 2 and CO should be calculate given the heterogeneous equilibrium process (Kp) at 700 K . Concept Introduction: Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction. 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. Homogeneous equilibrium : A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution. 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. Equilibrium concentration: If Kc and the initial concentration for a reaction and calculate for both equilibrium concentration and example using (ICE) chart and equilibrium constant and derived changes in respective reactants and products.

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Chapter 15, Problem 15.37QP

Interpretation Introduction

Interpretation:

The partial pressure of CO2 and CO should be calculate given the heterogeneous equilibrium process (Kp) at 700K.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

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.

Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.

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.

Equilibrium concentration: If Kc and the initial concentration for a reaction and calculate for both equilibrium concentration and example using (ICE) chart and equilibrium constant and derived changes in respective reactants and products.

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