A reversible reaction has an equilibrium expression, Keq = 50. If the reaction quotient calcuated in by a student performing this reaction is Q = 75, which of the following statements is true?
a
Equilibrium will proceed in the reverse direction favoring products.
b
Equilibrium will proceed in the reverse direction favoring reactants.
c
Equilibrium will proceed in the forward direction favoring reactants.
d
Equilibrium will proceed in the forward direction favoring products.
I think its d but not sure
Keq = 50 = (products)/(reactants)
If Q = 75 then products are too large and reactants are too small; therefore, the reaction must proceed so as to make products smaller and reactants larger.
I don't agree with d BECAUSE products are too high as is. Products must get smaller. Reactants must get larger.
To determine the correct answer, we need to compare the reaction quotient (Q) to the equilibrium constant (Keq). The equilibrium constant (Keq) indicates the position of the equilibrium and tells us whether the reaction favors the reactants or products.
If Q < Keq, this means there are more reactants present than at equilibrium, and the reaction will shift in the forward direction to form more products until Q approaches Keq. This is known as "Le Chatelier's principle." Conversely, if Q > Keq, there are more products present than at equilibrium, and the reaction will shift in the reverse direction to form more reactants until Q approaches Keq.
In this case, Q = 75, while Keq = 50. Since Q > Keq, it indicates an excess of products compared to the equilibrium state. Therefore, the reaction will proceed in the reverse direction, favoring reactants and trying to decrease the concentration of products. Therefore, the correct answer is option b: "Equilibrium will proceed in the reverse direction favoring reactants."