Question

which statement about $k_{eq}$ is not true?
it is affected by changes to the equilibrium system.
it has a numerical value.
it can be used to determine the unknown concentration of a reactant.
it can be used to determine the unknown concentration of a product.
it has a unit of measure.
question 10 (1 point)
consider the system below.
$n_2o_4(g) \leftrightarrow 2n_2o(g)$
which is true of the value of $k_{eq}$ for the system?
its value remains constant regardless of the initial concentrations of products and reactants.
its value varies depending on the initial concentrations of products and reactants.
its value increases when initial concentrations of reactants are greater than concentration of products.
its value decreases when initial concentrations of reactants are greater than concentration of products.
its value cannot be predicted based on concentrations.
question 11 (1 point)
the variable, $q_{eq}$, represents which of these?
the equilibrium constant using partial pressure
the equilibrium constant using concentration
the reaction quotient using partial pressure
the reaction quotient using concentration
the equilibrium constant using partial pressure and concentration

Explanation:

First Question (About \( K_{eq} \) statement not true)

• \( K_{eq} \) (equilibrium constant) is a constant for a given reaction at a specific temperature. It is not affected by changes in concentrations of reactants or products (equilibrium system changes like concentration shifts don't alter \( K_{eq} \); only temperature does).
• \( K_{eq} \) has a numerical value, can be used to find unknown concentrations of reactants/products via the equilibrium expression, and its units depend on the reaction (so it can have a unit). Thus, the false statement is "It is affected by changes to the equilibrium system."

• \( K_{eq} \) for a reaction is constant at a fixed temperature, regardless of initial concentrations of reactants or products. Initial concentrations affect the direction the reaction proceeds to reach equilibrium, but not the value of \( K_{eq} \). So the true statement is "Its value remains constant regardless of the initial concentrations of products and reactants."

• \( Q_{eq} \) (reaction quotient) using concentration is calculated from the concentrations of reactants and products at any point (not just equilibrium) using the same formula as \( K_{eq} \) (concentration - based). \( K_{eq} \) is for equilibrium, \( Q_p \) is reaction quotient with partial pressures. So \( Q_{eq} \) (more accurately \( Q_c \)) is the reaction quotient using concentration.

Answer:

It is affected by changes to the equilibrium system.

Question 10 (About \( K_{eq} \) for \( \ce{N2O4(g) <=> 2N2O(g)} \))