For the reaction [tex]N_2(g) + 3H_2(g) \rightarrow 2 NH_3(g)[/tex], a reaction mixture at a certain temperature contains [tex]N_2[/tex], [tex]H_2[/tex], and [tex]NH_3[/tex] in their standard states. If [tex]K_p = 41[/tex], which statement is true of the reaction mixture?

A. [tex]Q_p > K_p[/tex]; the reaction will proceed to the left.
B. [tex]Q_p = K_p[/tex]; the reaction is at equilibrium.
C. [tex]Q_p < K_p[/tex]; the reaction will proceed to the right.

The reaction quotient Qp in a chemical reaction is compared with the equilibrium constant Kp to determine the system's equilibrium state. If Qp > Kp, the reaction goes to the left, if Qp = Kp, it is at equilibrium, and if Qp < Kp, it goes to the right.

Explanation:

In the reaction N2(g) + 3H2(g) = 2 NH3(g) at a certain temperature, the reaction quotient Qp is used to determine the direction in which the reaction will proceed. If Kp = 41, the equilibrium constant of the reaction, we can compare it to Qp to determine where the reaction stands.

If Qp > Kp, the reaction will shift left to reach equilibrium, thus reducing the concentrations of the products.
If Qp = Kp, the reaction is at equilibrium.
If Qp < Kp, the reaction will shift right to reach equilibrium, thus increasing the concentrations of the products.

Without specific values for Qp, the exact direction of the reaction cannot be determined. However, the comparison of these parameters is a fundamental aspect of understanding chemical equilibrium.

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klassen114 klassen114 · Answer 2 · 2025-03-05T18:35:45-05:00

Final answer:

The value of Qp compared to Kp determines which direction a chemical reaction will proceed. If Qp > Kp, the reaction will proceed to the left. If Qp < Kp, it'll move to the right. If Qp = Kp, the reaction is at equilibrium.

Explanation:

In the reaction N2(g) + 3H2(g) = 2 NH3(g), the reaction quotient Qp and the equilibrium constant Kp are important for determining the direction in which the reaction will proceed. If Kp = 41, and Qp > Kp, this implies that there are more products (NH3) than reactants (N2 and H2) present at this moment. Hence, the reaction will proceed to the left, favoring the reactants to achieve equilibrium. On the other hand, if Qp < Kp, this means there is a higher concentration of reactants than products, and the reaction will proceed to the right, favoring the production of NH3 to achieve equilibrium. If Qp = Kp, the reaction is already at equilibrium and will not shift in either direction.

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