23) The equilibrium constant for the gas phase reaction

2NH3 (g) <-> N2 (g) + 3H2 (g)
is Keq = 230 at 300 °C. At equilibrium, __________.
A) reactants predominate
B) products predominate
C) only products are present
D) roughly equal amounts of products and reactants are present
E) only reactants are present
please explain the answer you choose.

If the Keq is >1, then products must be greater than reactants. If Keq <1, then reactants must be greater than products.

To determine the answer, we need to consider the value of the equilibrium constant (Keq). The equilibrium constant is a ratio of the concentrations of the products to the concentrations of the reactants at equilibrium.

In this case, the equilibrium constant (Keq) is given as 230. However, the value of Keq alone does not provide information about the relative concentrations of products and reactants at equilibrium.

To get a better understanding, we can look at the stoichiometry of the reaction:

2NH3 (g) <-> N2 (g) + 3H2 (g)

From the balanced equation, we can see that there are more molecules of product (N2 and H2) compared to the reactant (NH3). This suggests that if the reaction were to proceed to completion, more products would be formed.

However, in this case, we are dealing with an equilibrium reaction. At equilibrium, both forward and reverse reactions are occurring simultaneously. The concentrations of reactants and products reach a point where there is no further net change in their concentrations.

Based on the given information that Keq = 230, we can conclude that the reaction favors the products. A Keq value greater than 1 indicates that the concentration of products is greater than the concentration of reactants at equilibrium. Therefore, the answer is B) products predominate.

To determine the answer to this question, we need to consider the value of the equilibrium constant (Keq) and how it relates to the concentrations of the reactants and products at equilibrium.

The equilibrium constant (Keq) is calculated as the ratio of the concentrations of the products to the concentrations of the reactants, with each concentration raised to the power of its stoichiometric coefficient in the balanced equation.

In this case, the balanced equation is: 2NH3 (g) <-> N2 (g) + 3H2 (g)

Given that Keq = 230, this means that the products will be favored at equilibrium. The magnitude of Keq indicates the extent of the reaction. A Keq value greater than 1 signifies that the products are favored, while a Keq value less than 1 suggests that the reactants are favored.

Since Keq = 230 (>1), we can conclude that at equilibrium, products will predominate (choice B). This means that there will be a higher concentration of N2 and H2 gases compared to NH3 gas.

Additionally, it is important to note that the stoichiometry of the balanced equation can also provide a clue. In this case, since there are 2 moles of NH3 reacting to produce 1 mole of N2 and 3 moles of H2, there are more moles of products than reactants. Hence, it supports the notion that products will predominate at equilibrium.

Therefore, the correct answer is B) products predominate.

Products predominate