The SAT Subject Test in Chemistry assesses students' understanding of chemical concepts and their ability to apply them in problem-solving.
In many reactions, products can turn back into reactants. When the rates of forward and reverse reactions are equal, the system is in equilibrium.
The ratio of product concentrations to reactant concentrations (each raised to the power of their coefficients) is constant at a given temperature:
\( K_{eq} = \frac{[products]}{[reactants]} \)
According to Le Chatelier's Principle, if you change the concentration, temperature, or pressure, the system will adjust to counteract the change.
The production of ammonia in the Haber process relies on manipulating equilibrium to maximize yield.
\[K_{eq} = \frac{[products]}{[reactants]}\]
Adding more reactant to a system at equilibrium shifts the reaction toward more products.
Decreasing temperature in an exothermic reaction shifts equilibrium toward products.
At equilibrium, forward and reverse reactions occur at equal rates, and the system resists changes.