91Ó°ÊÓ

To comprehend chemical equilibrium, understanding the equilibrium constant is essential. When two reactants, such as fructose and glucose, are at equilibrium, the ratio of their concentrations becomes constant. This ratio is known as the equilibrium constant, denoted as \(K_c\). It represents how far a chemical reaction proceeds. In our example of fructose converting to glucose, we calculate \(K_c\) using \\[K_c = \frac{[\text{glucose}]}{[\text{fructose}]}\]. \At equilibrium, fructose concentration is \(0.113 \, \text{M}\) and glucose is \(0.131 \, \text{M}\). Substituting these into the formula, \(K_c\) becomes \(1.159\). This value helps chemists understand the balance of products to reactants, showing that more glucose forms from fructose. This constant provides insights into the direction and extent of the reaction under given conditions.

The concept of concentration change is crucial to quantify how much a reactant turns into a product. Initially, the solution has \(0.244 \, \text{M}\) fructose. Upon reaching equilibrium, only \(0.113 \, \text{M}\) fructose remains. The decrease, \(0.131 \, \text{M}\), reflects the amount converted to glucose. Understanding these changes clarifies a reaction’s progress:

• Initial concentration: measures the starting substance.
• Equilibrium concentration: reflects the substance amount when forward and reverse reactions balance.
• Change in concentration: indicates how much reactant transformed to product.

These values provide a clear picture of how chemical equilibrium shifts, enabling precise calculation of equilibrium constants.

Stoichiometry is a core aspect of chemistry that deals with the quantitative relationships between reactants and products in a chemical reaction. In our exercise, fructose converts to glucose in a 1:1 ratio. This means for every mole of fructose that reacts, one mole of glucose is formed. This simple stoichiometric relationship allows us to directly equate the change in fructose concentration to the formed glucose concentration. It enables us to accurately determine the concentrations of other substances involved in the reaction by understanding their stoichiometric coefficients. In essence, stoichiometry aids in predicting the amounts of products generated from a given amount of reactants.

Percentage conversion gives a numeric representation of how much reactant has been converted to product. For fructose turning into glucose, we calculate it to understand the extent of the conversion:The formula is \[\text{Percentage converted} = \left(\frac{\text{Change in concentration}}{\text{Initial concentration}}\right) \times 100\].Using the values from the exercise, we calculate \(\text{Percentage converted} = \left(\frac{0.131}{0.244}\right) \times 100 \approx 53.69\%\).This means over half of the fructose present initially turned into glucose. Knowing the percentage conversion helps assess the efficiency and completeness of a reaction. It is a handy metric for chemists to evaluate reaction conditions and optimize processes.