Reaction Coordinate Diagrams - AP Chemistry

The fully filled in reaction coordinate diagram is displayed below.

The arrow marked in the question represents the activation energy, which is the energy barrier that must be overcome in order for the reactants to form products.

This reaction is also exothermic because the energy of the products is lower than that of the reactants.

Start by drawing and labeling the reaction coordinate diagram.

Since we know that is negative, the products must be lower in energy than the reactants.

Now, the question wants you to find the activation energy if we were to reverse the reaction. In other words, we want to start at the products and end up with the reactants. From the diagram, you can see that the reverse activation energy is just the sum of the activation energy for the forward reaction and the .

In this question, we're presented with a free energy diagram for a chemical reaction occurring under standard conditions. We're asked to identify a true statement with regards to this diagram.

Right off the bat, we can see that the free energy of the products is greater than that of the reactants. Thus, this reaction has a positive change in free energy and so it is an endergonic reaction. Recall that one expression for the value of free energy change is as follows.

From this equation, we can see that the equilibrium constant is related to the standard change in free energy. Moreover, we can see that if the standard free energy change is positive, then the value of must be less than . Thus, we know that the reaction is favored towards the reactants.

Additionally, we cannot determine whether the entropy increases or decreases based on the diagram. The reason for this is that entropy is not the only factor that determines the change in free energy of a reaction. The change in enthalpy is also a factor that must be considered.

The fully filled in reaction coordinate diagram is displayed below.

The arrow marked in the question represents the activation energy, which is the energy barrier that must be overcome in order for the reactants to form products.

This reaction is also exothermic because the energy of the products is lower than that of the reactants.

Start by drawing and labeling the reaction coordinate diagram.

Since we know that is negative, the products must be lower in energy than the reactants.

Now, the question wants you to find the activation energy if we were to reverse the reaction. In other words, we want to start at the products and end up with the reactants. From the diagram, you can see that the reverse activation energy is just the sum of the activation energy for the forward reaction and the .

In this question, we're presented with a free energy diagram for a chemical reaction occurring under standard conditions. We're asked to identify a true statement with regards to this diagram.

Right off the bat, we can see that the free energy of the products is greater than that of the reactants. Thus, this reaction has a positive change in free energy and so it is an endergonic reaction. Recall that one expression for the value of free energy change is as follows.

From this equation, we can see that the equilibrium constant is related to the standard change in free energy. Moreover, we can see that if the standard free energy change is positive, then the value of must be less than . Thus, we know that the reaction is favored towards the reactants.

Additionally, we cannot determine whether the entropy increases or decreases based on the diagram. The reason for this is that entropy is not the only factor that determines the change in free energy of a reaction. The change in enthalpy is also a factor that must be considered.

The fully filled in reaction coordinate diagram is displayed below.

The arrow marked in the question represents the activation energy, which is the energy barrier that must be overcome in order for the reactants to form products.

This reaction is also exothermic because the energy of the products is lower than that of the reactants.

Start by drawing and labeling the reaction coordinate diagram.

Since we know that is negative, the products must be lower in energy than the reactants.

Now, the question wants you to find the activation energy if we were to reverse the reaction. In other words, we want to start at the products and end up with the reactants. From the diagram, you can see that the reverse activation energy is just the sum of the activation energy for the forward reaction and the .

In this question, we're presented with a free energy diagram for a chemical reaction occurring under standard conditions. We're asked to identify a true statement with regards to this diagram.

Right off the bat, we can see that the free energy of the products is greater than that of the reactants. Thus, this reaction has a positive change in free energy and so it is an endergonic reaction. Recall that one expression for the value of free energy change is as follows.

From this equation, we can see that the equilibrium constant is related to the standard change in free energy. Moreover, we can see that if the standard free energy change is positive, then the value of must be less than . Thus, we know that the reaction is favored towards the reactants.

Additionally, we cannot determine whether the entropy increases or decreases based on the diagram. The reason for this is that entropy is not the only factor that determines the change in free energy of a reaction. The change in enthalpy is also a factor that must be considered.

The fully filled in reaction coordinate diagram is displayed below.

The arrow marked in the question represents the activation energy, which is the energy barrier that must be overcome in order for the reactants to form products.

This reaction is also exothermic because the energy of the products is lower than that of the reactants.

Start by drawing and labeling the reaction coordinate diagram.

Since we know that is negative, the products must be lower in energy than the reactants.

Now, the question wants you to find the activation energy if we were to reverse the reaction. In other words, we want to start at the products and end up with the reactants. From the diagram, you can see that the reverse activation energy is just the sum of the activation energy for the forward reaction and the .

In this question, we're presented with a free energy diagram for a chemical reaction occurring under standard conditions. We're asked to identify a true statement with regards to this diagram.

Right off the bat, we can see that the free energy of the products is greater than that of the reactants. Thus, this reaction has a positive change in free energy and so it is an endergonic reaction. Recall that one expression for the value of free energy change is as follows.

From this equation, we can see that the equilibrium constant is related to the standard change in free energy. Moreover, we can see that if the standard free energy change is positive, then the value of must be less than . Thus, we know that the reaction is favored towards the reactants.

Additionally, we cannot determine whether the entropy increases or decreases based on the diagram. The reason for this is that entropy is not the only factor that determines the change in free energy of a reaction. The change in enthalpy is also a factor that must be considered.