Chapter 17, Problem 39A

Interpretation Introduction

Interpretation: An explanation has to be given on relative concentrations of products and reactants for equilibrium constant $\left(K\text{=4}{\text{.5×10}}^{-6}\right)$ that would be present at equilibrium and the way by which the reaction could be made more useful has to be predicted.

Concept introduction: For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is ratio of the concentration of the products to the concentration of the reactants. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

  $K=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

The equilibrium constant is represented as $K.$

Answer to Problem 39A

A small equilibrium constant directs that the concentration of product is much small compared to that of reactant. The equilibrium position is to the left and the reaction could be made useful, by shifting the equilibrium position to the right.

Explanation of Solution

The given equilibrium constant is $\text{4}{\text{.5×10}}^{\text{-6}}$ and the value of equilibrium constant is small.

For a balanced chemical reaction,

  $aA+bB\rightleftharpoons cC+dD$

The equilibrium expression is ratio of the concentration of the products to the concentration of the reactants. The concentration of each reactant/product is raised to a power corresponding to their coefficient in the balanced equation.

The law of chemical equilibrium is given by the equilibrium expression,

  $K=\frac{{\left[C\right]}^c{\left[D\right]}^d}{{\left[A\right]}^a{\left[B\right]}^b}$

The equilibrium constant is represented as $K.$

The magnitude of the equilibrium constant $\left(K\right),$ predicts the extent to which a reaction would proceed.

A small equilibrium constant shows that the equilibrium concentration of the reactants would be large. The reaction would proceed to the left side indicating an increase in the concentration of reactants.

A small equilibrium constant specifies that the concentration of product is much small compared to that of reactant. The equilibrium position is shifted to the left and is not good for the production of products. The reaction would be made useful by shifting the equilibrium position to the right.

Conclusion

In case of smaller equilibrium constant, the concentration of the reactants is higher, the equilibrium position shifts towards the left, and the reaction is a not good source of the products. By shifting the equilibrium position towards the right, the reaction would be made more useful.