Free Energy and the Equilibrium Constant

Mr. Anderson explains the relationship between free energy (delta G) and the equilibrium constant (K) in chemical reactions. He discusses how delta G and K are interconnected and how they can predict the direction of a reaction. The video also covers the importance of these concepts in biological systems, particularly in cellular respiration and ATP production. Examples of reactions with different delta G and K values are provided to illustrate these concepts.

What does a delta G value of zero indicate about a chemical reaction?

• The reaction is at equilibrium.

• The reaction is non-spontaneous.

• The reaction is exothermic.

• The reaction is endothermic.

If the equilibrium constant K is greater than 1, what can be inferred about delta G?

• Delta G is positive.

• Delta G is undefined.

• Delta G is zero.

• Delta G is negative.

In a reaction where delta G is positive, what is the nature of the reaction?

• Non-spontaneous and exothermic

• Spontaneous and endothermic

• Non-spontaneous and endothermic

• Spontaneous and exothermic

How does a small K value affect the position of equilibrium in a reaction?

• Equilibrium is undefined.

• Equilibrium shifts towards the products.

• Equilibrium remains unchanged.

• Equilibrium shifts towards the reactants.

What is the significance of delta G in biological systems?

• It predicts the color change in reactions.

• It measures the heat released in reactions.

• It indicates the total energy change in reactions.

• It determines the speed of reactions.

In cellular respiration, what does a negative delta G value suggest?

• The reaction favors the reactants.

• The reaction is non-spontaneous.

• The reaction is spontaneous.

• The reaction is at equilibrium.

What role does ATP play in cellular processes?

• It stores genetic information.

• It acts as a catalyst.

• It serves as cellular energy currency.

• It transports oxygen.