At 1000 K, Kp = 2.1 * 106 and ΔH° = - 107.7 kJ for the reaction H21g2 + Br21g2 ∆ 2 HBr1g2.(b) For the equilibrium in part (a), each of the following changes will increase the equilibrium partial pressure of HBr. Choose the change that will cause the greatest increase in the pressure of HBr, and explain your choice.(ii) Adding 0.10 mol of Br2

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Identify the reaction: \( \text{H}_2(g) + \text{Br}_2(g) \rightleftharpoons 2 \text{HBr}(g) \).

Recognize that adding \( \text{Br}_2 \) will shift the equilibrium according to Le Chatelier's Principle.

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to minimize the disturbance.

Adding \( \text{Br}_2 \) increases the concentration of a reactant, causing the equilibrium to shift to the right to produce more \( \text{HBr} \).

The shift to the right results in an increase in the partial pressure of \( \text{HBr} \), as more \( \text{HBr} \) is formed.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of the given reaction, adding more Br2 will shift the equilibrium to the right, favoring the production of HBr to restore balance.

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium. For the reaction provided, Kp indicates a strong tendency to form HBr, and any increase in the concentration of reactants like Br2 will enhance the formation of products, thereby increasing the partial pressure of HBr.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in time, compared to the equilibrium constant Kp. If Q is less than Kp, the reaction will proceed to the right to produce more products. Adding Br2 increases the concentration of reactants, thus lowering Q and driving the reaction towards the formation of more HBr.

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