Spontaneous Processes

Mr. Anderson explains spontaneous and nonspontaneous processes in chemistry, focusing on enthalpy and entropy changes. He uses examples and simulations to illustrate how equilibrium constants can determine reaction favorability. The video concludes with a brief introduction to Gibbs free energy.

What is a key characteristic of a spontaneous process?

• It occurs without any change in enthalpy.

• It requires external energy to proceed.

• It occurs without external energy input.

• It always results in a decrease in entropy.

Which of the following indicates a spontaneous process?

• Increase in both enthalpy and entropy

• Decrease in both enthalpy and entropy

• Decrease in enthalpy and increase in entropy

• Increase in enthalpy and decrease in entropy

What does an equilibrium constant greater than 1 signify?

• The reaction favors the reactants.

• The reaction is nonspontaneous.

• The reaction favors the products.

• The reaction is at equilibrium.

Why is the conversion of graphite to diamond considered nonspontaneous?

• It occurs without any energy input.

• It requires a large amount of energy and pressure.

• It results in a decrease in entropy.

• It happens instantly under normal conditions.

In a spontaneous process, what happens to enthalpy and entropy?

• Both enthalpy and entropy decrease

• Both enthalpy and entropy increase

• Enthalpy decreases, entropy increases

• Enthalpy increases, entropy decreases

What does a K value of less than 1 indicate about a reaction?

• The reaction is at equilibrium.

• The reaction favors the products.

• The reaction is spontaneous.

• The reaction is nonspontaneous.

What is the significance of a negative change in enthalpy?

• It means the reaction requires energy input.

• It indicates an endothermic reaction.

• It suggests a nonspontaneous process.

• It implies the reaction is exothermic.