Chapter 15.3, Problem 15.3.3SR

Interpretation Introduction

Interpretation:

The equilibrium constant $\left({\text{K}}_{\text{c}}\right)$ values for given reactions are given.  From this the equilibrium constant of given aqueous phase equilibrium reaction at ${\text{25}}^{\text{0}}\text{C}$ has to be calculated.

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.

$K_{p}and{K}_c:$ This equilibrium constants of gaseous mixtures, these difference between the two constants is that ${\text{K}}_{\text{c}}$ is defined by molar concentrations, whereas ${\text{K}}_{\text{p}}$  is defined by the partial pressures of the gasses inside a closed system.

Equilibrium pressure: 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.

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.