Chapter 15.2, Problem 15.2.2SR

Interpretation Introduction

Interpretation:

The equilibrium constant $\left({\text{K}}_{\text{c}}\right)$ value for given reaction has to be calculated.

Concept Introduction:

Chemical equilibrium: The term applied to reversible chemical reactions.  It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction.  The equilibrium is achieved when the concentrations of reactants and products become constant.

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.

Balancing of equilibrium reaction: The many of chemical reaction involving for, reversible reaction is occurring backwards and forwards at the time by the same amount, it is balancing point of a chemical reaction, it seems to stop happening when the rates are equal equilibrium has occurred.

Reaction quotient: This type of chemical equilibrium reaction proceeds likely to produced, given either the pressure (or) the concentration of the reactants and the products.  The value can be compared to the equilibrium constant, to determine the direction of the reaction that is take place.  Then reaction quotient $\left(\text{Qc}\right)$ the indication of Q can be used to determine which direction will shift to reach of chemical equilibrium process.

To find: The chemical equilibrium reaction should be identified given the respective reactions.

Analyse the reactant product equilibrium reactions.