A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2 X 10^4 at room temp. However, after 15minutes the chemist finds that the reaction with the smaller equilibrium constant produces more desired product. Explain how this might be possible.
I don't get it???
UsuAlly when the constant has a larger value it produces more produces making the reaction lie to the right at equilibrium. Why is the smaller constAnt producing more product????
What you say is true at equilibrium but no one said these reactions were at equilibrium. The activation energy may be so high that the more favorable reaction thermodynamically is so slow that it proceeds at a snails pace, even if it proceeds at all. The other reaction may not have that problem.
The next time you see or try to buy a diamond remember that diamonds are not favored; graphite is the stable form of carbon. Why? because of the activation energy required to get to the more stable form. So I need not fear that I will wake up tomorrow and my diamond will be graphite. That conversion will take place eventually but long after I've left this earth.
Although it is true that a larger equilibrium constant typically indicates that more product is formed, it is important to consider the reaction kinetics and the time frame in which the reactions are being compared. The equilibrium constant is a measure of the ratio of reactants to products at equilibrium, but it does not provide information about the rate at which the reaction reaches equilibrium.
In this case, the chemist observes the reactions after 15 minutes, which may not be sufficient time for the reactions to reach equilibrium. It is possible that the reaction with the smaller equilibrium constant has a faster rate of reaction, meaning it reaches a higher concentration of product after 15 minutes compared to the reaction with the larger equilibrium constant.
Additionally, the equilibrium constant is temperature-dependent. The given equilibrium constants are specifically stated to be at room temperature. If the two reactions have different activation energies, it is possible that the reaction with the smaller equilibrium constant may have a lower activation energy, allowing it to proceed at a faster rate at room temperature.
In summary, while a larger equilibrium constant generally indicates a more favorable equilibrium position, the rate of reaction and the time frame in which the reactions are compared can affect the observed amount of product at a given point in time.
In this case, it may seem counterintuitive that the reaction with the smaller equilibrium constant is producing more desired product. However, it is important to remember that equilibrium constant alone does not determine the reaction rate or the rate at which product is formed.
Equilibrium constants, denoted by K, provide information about the relative amounts of reactants and products present at equilibrium. The magnitude of K indicates the position of the equilibrium: a larger value of K suggests that there are more products present at equilibrium, while a smaller value of K suggests that there are more reactants present.
In the context of this question, the larger equilibrium constant of 2.2 x 10^4 indicates that the reaction at equilibrium predominantly favors the formation of products. On the other hand, the smaller equilibrium constant of 23.3 suggests that the reaction at equilibrium predominantly favors the formation of reactants.
Now, let's consider the reaction rates. The rate of a chemical reaction determines how quickly the reactants are converted into products. It is possible for a reaction with a smaller equilibrium constant to have a faster rate, leading to the formation of more product within a given timeframe.
There are multiple factors that can influence reaction rates, such as temperature, concentration, and catalysts. In this case, it is likely that the reaction with the smaller equilibrium constant has favorable conditions, such as a higher temperature or higher reactant concentrations, that promote a faster reaction rate.
Therefore, even though the reaction with the smaller equilibrium constant may have a larger amount of reactants at equilibrium, the faster rate of the reaction allows it to produce more desired product within the same timeframe.
It is important to note that the equilibrium constant provides information about the relative amounts of reactants and products at equilibrium, while the reaction rate determines the speed at which reactants are converted into products.