Using Gibbs Free Energy

Mr. Anderson explains Gibbs free energy, a key concept in chemistry that indicates whether a reaction is spontaneous. He discusses the roles of enthalpy, entropy, and temperature in determining reaction spontaneity. Using analogies and examples like thermite reactions and cold packs, he illustrates how these factors interact. The video also covers the Gibbs free energy equation, emphasizing its importance in predicting reaction behavior.

What does a negative Gibbs free energy indicate about a chemical reaction?

• The reaction requires energy input.

• The reaction is non-spontaneous.

• The reaction is at equilibrium.

• The reaction is spontaneous.

Which of the following is a good indicator of a spontaneous reaction?

• A positive delta H

• A negative delta H

• A decrease in entropy

• An increase in temperature

In the context of Gibbs free energy, what role does temperature play?

• It only affects endothermic reactions.

• It determines the sign of delta H.

• It affects the importance of entropy in the equation.

• It is irrelevant to spontaneity.

What happens to delta G when both enthalpy and entropy increase at high temperatures?

• Delta G becomes positive.

• Delta G becomes negative.

• Delta G equals zero.

• Delta G remains unchanged.

How does a cold pack demonstrate a spontaneous reaction despite a positive delta H?

• By decreasing entropy significantly.

• By increasing entropy significantly.

• By having a very low delta G.

• By maintaining constant temperature.

What is the significance of delta G being equal to zero?

• The reaction requires energy input.

• The reaction is at equilibrium.

• The reaction is non-spontaneous.

• The reaction is spontaneous.

Which scenario would likely result in a non-spontaneous reaction?

• Decrease in both enthalpy and entropy at low temperature

• Decrease in enthalpy and increase in entropy

• Increase in both enthalpy and entropy at high temperature

• Increase in enthalpy and decrease in entropy