The relationship between equilibrium constants is defined by the fact that the expressions for equilibrium
constants depend on the concentration units used, typically expressed in moles per cubic decimeter ( mol
dm-3 ). For a reversible reaction represented as
aA + bB ⇌ cC + dD
the equilibrium constant (K) is calculated as
K = [C]c[D]d / [A]a[B]b, where the coefficients of the balanced
equation appear as
exponents in the
expression.
The value of the equilibrium constant is specific to a particular reaction and remains constant at a given
temperature, providing insights into the direction and extent of the reaction
How does the equilibrium constant relate to the concentrations of reactants and products?
The equilibrium constant is the ratio of the products of the concentrations of the products to the products of the concentrations of the reactants at equilibrium
What happens to the value of the equilibrium constant if the temperature changes?
The value of the equilibrium constant is specific to a particular reaction and remains constant at a given temperature; it changes if the temperature is altered
What does a large equilibrium constant indicate about a reaction?
A large equilibrium constant indicates that the reaction is almost complete, favoring the formation of products
What is the significance of the coefficients in the equilibrium constant expression?
The coefficients in the balanced equation appear as exponents in the equilibrium constant expression, reflecting the stoichiometry of the reaction
How do changes in concentration affect the position of equilibrium?
Changes in concentration can shift the position of equilibrium, but they do not alter the value of the equilibrium constant itself
What does a large equilibrium constant (K) indicate about a reaction?
a) The reaction is incomplete
b) The reaction favors the reactants
c) The reaction is almost complete
d) The reaction does not occur
Answer: c) The reaction is almost complete
Which of the following statements is true regarding the equilibrium constant?
a) It changes with concentration
b) It is specific to a particular reaction at a given temperature
c) It is always equal to 1
d) It is dependent on the pressure only
Answer: b) It is specific to a particular reaction at a given temperature
What is the relationship between Kc and Kp for reactions involving gases?
a) Kc is always greater than Kp
b) Kp is always greater than Kc for reactions with an increase in moles
c) Kc and Kp are always equal
d) Kp is independent of temperature
Answer: b) Kp is always greater than Kc for reactions with an increase in moles
What effect does increasing the concentration of reactants have on the equilibrium position?
a) It shifts the equilibrium to the left
b) It shifts the equilibrium to the right
c) It has no effect on the equilibrium position
d) It decreases the value of K
Answer: b) It shifts the equilibrium to the right
Which of the following is true about the equilibrium constant K?
a) It has units that are always the same
b) It can be calculated using the concentrations of reactants only
c) It is a ratio of the concentrations of products to reactants
d) It is affected by the presence of a catalyst
Answer: c) It is a ratio of the concentrations of products to reactants