At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) If the equilibrium partial pressures of NOBr(𝑔) and Br2(𝑔) are both 0.100 atm at 373 K, what is the equilibrium partial pressure of NO(𝑔)?

Ch.15 - Chemical Equilibrium

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.15 - Chemical Equilibrium

문제 58

15장, 문제 58

At 373 K, 𝐾_𝑝= 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br₂(𝑔) If the equilibrium partial pressures of NOBr(𝑔) and Br₂(𝑔) are both 0.100 atm at 373 K, what is the equilibrium partial pressure of NO(𝑔)?

검증된 단계별 안내

Identify the equilibrium expression for the reaction: \( K_p = \frac{(P_{NO})^2 (P_{Br_2})}{(P_{NOBr})^2} \).

Substitute the known values into the equilibrium expression: \( K_p = 0.416 \), \( P_{NOBr} = 0.100 \) atm, and \( P_{Br_2} = 0.100 \) atm.

Rearrange the equation to solve for \( (P_{NO})^2 \): \( (P_{NO})^2 = K_p \times (P_{NOBr})^2 / P_{Br_2} \).

Substitute the known values into the rearranged equation: \( (P_{NO})^2 = 0.416 \times (0.100)^2 / 0.100 \).

Calculate \( P_{NO} \) by taking the square root of \( (P_{NO})^2 \).

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주요 개념

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

Equilibrium Constant (Kp)

The equilibrium constant, Kp, is a ratio that expresses the relationship between the partial pressures of the products and reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2 NOBr(g) ⇌ 2 NO(g) + Br2(g), Kp is calculated using the formula Kp = (P_NO^2 * P_Br2) / (P_NOBr^2), where P represents the partial pressures of the gases involved.

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of the equilibrium reaction, the partial pressures of NOBr, NO, and Br2 are crucial for calculating the equilibrium constant and determining the concentrations of each species at equilibrium. The total pressure of the gas mixture is the sum of the partial pressures of all components.

Stoichiometry of the Reaction

Stoichiometry refers to the quantitative relationship between the reactants and products in a chemical reaction. In this equilibrium, the stoichiometric coefficients indicate that for every 2 moles of NOBr that dissociate, 2 moles of NO and 1 mole of Br2 are produced. This relationship is essential for calculating the equilibrium partial pressure of NO based on the known partial pressures of NOBr and Br2.