Draw an energy diagram for a one-step reaction with Keq<1 . Label the parts of the diagram corre

Draw an energy diagram for a one-step reaction with Keq<1 ....

Key Concepts

Relationship between ?G° and the Equilibrium Constant

The relationship between ?G° and the equilibrium constant (K_eq) is given by the equation ?G° = -RT ln(K_eq). When K_eq is less than one, ln(K_eq) is negative, making ?G° positive. This indicates that the reaction is not thermodynamically favored in the forward direction under standard conditions.

Activation Energy (?G‡)

?G‡ is the free energy difference between the reactants and the transition state. This value represents the kinetic barrier that must be overcome for the reaction to proceed, influencing the rate at which the reaction occurs. It is a key factor in understanding the reaction mechanism and dynamics.

Standard Free Energy Change (?G°)

?G° is the difference in free energy between the products and the reactants under standard conditions. It indicates whether a reaction is exergonic (negative ?G°) or endergonic (positive ?G°). For a reaction with K_eq < 1, ?G° is positive, meaning that the reaction is non-spontaneous under standard conditions.

Energy Profile Diagram

An energy profile diagram is a graphical representation of the change in free energy as a reaction progresses from reactants to products. It shows the energy of the reactants, the rise to a peak at the transition state, and the energy of the products, helping to visualize both the reaction driving force (?G°) and the kinetic barrier (?G‡).

Reactants and Products

In an energy diagram, reactants and products are depicted at distinct energy levels. The reactants are placed at the starting energy level and the products at the final level. For a reaction with an equilibrium constant less than one (K_eq < 1), the products are at a higher energy level than the reactants, indicating that the reaction is non-spontaneous under standard conditions.

Transition State

The transition state represents the highest energy point along the reaction coordinate in an energy diagram. It corresponds to the brief, unstable structure that the reaction system passes through on its way from reactants to products, and its energy relative to the reactants defines the activation energy of the reaction.

Transcript

00:01 In this problem, you're told that you have a one -step reaction where the equilibrium constant is less than one.

00:15 And from here, you want to draw a reaction coordinate diagram.

00:20 Now, before you do that, you first want to figure out is the overall exorganicity of the reaction greater than one or less than one? and you can go about this in two different ways.

00:36 The first is you want to consider the fact that k equilibrium is essentially the concentration of your products over the concentration of your reactants.

00:49 So if k equilibrium is greater than one, this tells you that your products are going to be in a higher concentration than your reactants.

01:00 If your k equilibrium is equal to one, your concentration of your products is going to be equal to the concentration of your reactants.

01:09 And finally, if your k equilibrium is less than one, this tells you that the concentration of your products is going to be less than the concentration of your reactants.

01:24 So because we are concerned with this last statement, we know that in this one -step reaction, our concentrations of our product is going to be lower than the concentration of our reactants.

01:52 Now, we can also consider the equation where k equilibrium is equal to this value here.

02:06 Right? and so what this tells us is that k equilibrium is correlating to our negative delta g.

02:25 So because of this correlation, if k equilibrium is less than one, then, and our delta g is going to be greater than zero.

02:45 And another way we can think about this is, again, going back to our reactants and our products.

02:56 Draw this in equilibrium...

Please give Ace some feedback