Chapter 19.4, Problem 30R

To determine

To explain: the two ways that influence the given equilibrium to produce more ethanal.

Answer to Problem 30R

The reaction of formation of ethanal by the oxidation of ethanol is an exothermic reaction because it releases energy. According to the Le Chatelier’s principle, any change in the system at equilibrium due to change in temperature, volume, or concentration shifts the equilibrium in opposite direction or in direction to minimize that change and system achieves a new equilibrium state. By increasing the reactants concentration or ethanal, the equilibrium will shift to the right side and more ethanal will produce. Similarly, by decreasing the system’s temperature the equilibrium will shift to the right side.

Explanation of Solution

Introduction:

According to the Le Chatelier’s principle, any change in the system at equilibrium due to change in temperature, volume, or concentration shifts the equilibrium in opposite direction or in direction to minimize that change and system achieves a new equilibrium state.

Ethanal is formed by the oxidation of ethanol. This reaction is exothermic because it releases the energy. According to the Le Chatelier’s principle, if any change in the reaction takes place at equilibrium, equilibrium will shift in the direction to minimize that change. This results in establishing a new equilibrium.

The product can be enhanced by the following two ways:

1. By increasing the concentration of the reactants (ethanal in this case): the equilibrium will shift to the right side hence, that favors the product formation.
2. By decreasing the system’s temperature: this reaction is exothermic reaction, the decrease in temperature of the system will shift the equilibrium to the right side, according to the Le Chatelier’s principle and hence, that favors the product formation.

Conclusion:

Thus, the changes in equilibrium are explained by Le chatelier’s principle.