### Chemical Equilibrium Question**Select the single best answer.****At 425°C, \( K_p = 4.18 \times 10^{-9} \) for the reaction:**\[ 2 \text{HBr}(g) \rightleftharpoons \text{H}_2(g) + \text{Br}_2(g) \]**In one experiment, 0.20 atm of HBr(g), 0.085 atm of H₂(g), and 0.085 atm of Br₂(g) are introduced into a container. Is the reaction at equilibrium? If not, in which direction will it proceed?**- Yes, the reaction is at equilibrium.- No, the reaction is not at equilibrium and will proceed to the right.- No, the reaction is not at equilibrium and will proceed to the left.**Instructions:**To determine whether the reaction is at equilibrium, you should compare the reaction quotient \( Q_p \) to the equilibrium constant \( K_p \). The reaction quotient \( Q_p \) is calculated using the partial pressures of the gases:\[ Q_p = \frac{P_{\text{H}_2} \cdot P_{\text{Br}_2}}{(P_{\text{HBr}})^2} \]Substitute the given partial pressures into the expression:\[ Q_p = \frac{(0.085 \, \text{atm}) \cdot (0.085 \, \text{atm})}{(0.20 \, \text{atm})^2} = \frac{0.007225}{0.04} = 0.180625 \]Compare \( Q_p \) to \( K_p \):- If \( Q_p < K_p \), the reaction will proceed to the right (toward the products).- If \( Q_p > K_p \), the reaction will proceed to the left (toward the reactants).- If \( Q_p = K_p \), the reaction is at equilibrium.In this problem:\[ Q_p = 0.180625 \]\[ K_p = 4.18 \times 10^{-9} \]Since \( Q_p \) is significantly greater than \( K_p \), the reaction will proceed to the left to reach equilibrium.Therefore, the correct answer is:- No, the reaction is not at equilibrium and will

In order to determine the direction in which reaction will proceed, we will calculate the reaction…

Select the single best answer. At 425°C, K, = 4.18 × 10 for the reaction 2 HBr(g) = H,(g) + Br,( g) In one experiment, 0.20 atm of HBr(g), 0.085 atm of H,(g), and 0.085 atm of Br,(g) are introd into a container. Is the reaction at equilibrium? If not, in which direction will it proceed? Yes, the reaction is at equilibrium. No, the reaction is not at equilibrium and will proceed to the right. No, the reaction is not at equilibrium and will proceed to the left.

Select the single best answer. At 425°C, K, = 4.18 × 10 for the reaction 2 HBr(g) = H,(g) + Br,( g) In one experiment, 0.20 atm of HBr(g), 0.085 atm of H,(g), and 0.085 atm of Br,(g) are introd into a container. Is the reaction at equilibrium? If not, in which direction will it proceed? Yes, the reaction is at equilibrium. No, the reaction is not at equilibrium and will proceed to the right. No, the reaction is not at equilibrium and will proceed to the left.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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