General Chemistry II - Exam 2 Questions
and Answers | Latest Update | 2024/2025
| 100% Pass
How does the concentration of reactants and products influence the position of equilibrium in a
chemical reaction?
✔✔ The position of equilibrium shifts to favor the side (reactants or products) where the
concentration is decreased or where the concentration is increased, according to Le Chatelier’s
principle.
What is the reaction quotient (Q), and how is it used to predict the direction of shift for a reaction
not at equilibrium?
✔✔ The reaction quotient (Q) is calculated using the same formula as the equilibrium constant
(K) but with current concentrations. If Q < K, the reaction will shift toward the products; if Q >
K, it will shift toward the reactants.
How does a change in temperature affect the equilibrium constant (K) of an exothermic versus
an endothermic reaction?
✔✔ For an exothermic reaction, increasing the temperature decreases the equilibrium constant
(K), shifting the equilibrium towards the reactants. For an endothermic reaction, increasing the
1
, temperature increases the equilibrium constant (K), shifting the equilibrium towards the
products.
What is the concept of dynamic equilibrium in the context of chemical reactions, and how is it
maintained?
✔✔ Dynamic equilibrium is reached when the rates of the forward and reverse reactions are
equal, resulting in constant concentrations of reactants and products over time. It is maintained as
long as no external changes affect the system.
How do you determine the equilibrium constant (K) for a reaction given the equilibrium
concentrations of the reactants and products?
✔✔ The equilibrium constant (K) is determined by taking the ratio of the concentrations of the
products raised to their stoichiometric coefficients to the concentrations of the reactants raised to
their stoichiometric coefficients at equilibrium.
What is the difference between homogeneous and heterogeneous equilibria, and how are they
represented in equilibrium expressions?
✔✔ Homogeneous equilibria involve reactants and products in the same phase, while
heterogeneous equilibria involve reactants and products in different phases. In equilibrium
expressions, only concentrations of species in the same phase are included for homogeneous
2
and Answers | Latest Update | 2024/2025
| 100% Pass
How does the concentration of reactants and products influence the position of equilibrium in a
chemical reaction?
✔✔ The position of equilibrium shifts to favor the side (reactants or products) where the
concentration is decreased or where the concentration is increased, according to Le Chatelier’s
principle.
What is the reaction quotient (Q), and how is it used to predict the direction of shift for a reaction
not at equilibrium?
✔✔ The reaction quotient (Q) is calculated using the same formula as the equilibrium constant
(K) but with current concentrations. If Q < K, the reaction will shift toward the products; if Q >
K, it will shift toward the reactants.
How does a change in temperature affect the equilibrium constant (K) of an exothermic versus
an endothermic reaction?
✔✔ For an exothermic reaction, increasing the temperature decreases the equilibrium constant
(K), shifting the equilibrium towards the reactants. For an endothermic reaction, increasing the
1
, temperature increases the equilibrium constant (K), shifting the equilibrium towards the
products.
What is the concept of dynamic equilibrium in the context of chemical reactions, and how is it
maintained?
✔✔ Dynamic equilibrium is reached when the rates of the forward and reverse reactions are
equal, resulting in constant concentrations of reactants and products over time. It is maintained as
long as no external changes affect the system.
How do you determine the equilibrium constant (K) for a reaction given the equilibrium
concentrations of the reactants and products?
✔✔ The equilibrium constant (K) is determined by taking the ratio of the concentrations of the
products raised to their stoichiometric coefficients to the concentrations of the reactants raised to
their stoichiometric coefficients at equilibrium.
What is the difference between homogeneous and heterogeneous equilibria, and how are they
represented in equilibrium expressions?
✔✔ Homogeneous equilibria involve reactants and products in the same phase, while
heterogeneous equilibria involve reactants and products in different phases. In equilibrium
expressions, only concentrations of species in the same phase are included for homogeneous
2
