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

검증된 단계별 안내

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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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.

관련 실천

The F-F bond in F₂ is relatively weak because the lone pairs of electrons on one F atom repel the lone pairs on the other F atom; K_p = 7.83 at 1500 K for the reaction F₂(g) ⇌ 2 F(g). (a) If the equilibrium partial pressure of F₂ molecules at 1500 K is 0.200 atm, what is the equilibrium partial pressure of F atoms in atm?

교과서 질문

Refining petroleum involves cracking large hydrocarbon molecules into smaller, more volatile pieces. A simple example of hydrocarbon cracking is the gas-phase thermal decomposition of butane to give ethane and ethylene: (c) A sample of butane having a pressure of 50 atm is heated at 500 °C in a closed container at constant volume. When equilibrium is reached, what percentage of the butane has been converted to ethane and ethylene? What is the total pressure at equilibrium?

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교과서 질문

Halogen lamps are ordinary tungsten filament lamps in which the lamp bulb contains a small amount of a halogen (often bromine). At the high temperatures of the lamp, the halogens dissociate and exist as single atoms. (c) When the WBr41g2 diffuses back toward the filament, it decomposes, depositing tungsten back onto the fila- ment. Show quantitatively that the pressure of WBr4 from part (a) will cause the reaction in part (a) to go in reverse direction at 2800 K. [The pressure of Br1g2 is still 0.010 atm.] Thus, tungsten is continually recycled from the walls of the bulb back to the filament, allow-ing the bulb to last longer and burn brighter.

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교과서 질문

Heavy water, symbolized D2O 1D = 2H2 finds use as a neutron moderator in nuclear reactors. In a mixture with ordinary water, exchange of isotopes occurs according to the following equation: H2O + D2O ∆ 2 HDO Kc = 3.86 at 298 K When 1.00 mol of H2O is combined with 1.00 mol of D2O, what are the equilibrium amounts of H2O, D2O, and HDO (in moles) at 298 K? Assume the density of the mixture is constant at 1.05 g>cm3.

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