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Ch.15 - Chemical Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.15 - Chemical Equilibrium문제 32a
15장, 문제 32a

Calculate Kp for each reaction. a. N2O4(g) ⇌ 2 NO2(g) Kc = 5.9⨉10-3 (at 298 K)

검증된 단계별 안내
1
Identify the balanced chemical equation for the reaction: N2O4(g) ⇌ 2NO2(g).
Understand the relationship between Kc and Kp: Kp = Kc(RT)^{\(\Delta\) n}, where R is the gas constant (0.0821 L atm K^{-1} mol^{-1}), T is the temperature in Kelvin, and \(\Delta\) n is the change in moles of gas (moles of products - moles of reactants).
Calculate \(\Delta\) n for the reaction: \(\Delta\) n = 2 - 1 = 1.
Substitute the values into the equation: Kp = (5.9 \(\times\) 10^{-3}) \(\times\) (0.0821 \(\times\) 298)^1.
Simplify the expression to find Kp.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m

주요 개념

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

Equilibrium Constant (Kc and Kp)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Kp, on the other hand, is the equilibrium constant expressed in terms of partial pressures of gases. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
추천 영상:
가이드 코스
02:06
Kp vs. Kc Formula

Partial Pressure

Partial pressure is the pressure exerted by a single component of a gas mixture. In the context of Kp, it refers to the pressure of each gas in the reaction when it is at equilibrium. The total pressure of the gas mixture is the sum of the partial pressures of all the gases present, and understanding this concept is crucial for calculating Kp from Kc.
추천 영상:
가이드 코스
00:48
Partial Pressure Calculation

Change in Moles of Gas (Δn)

Δn is defined as the difference between the number of moles of gaseous products and the number of moles of gaseous reactants in a balanced chemical equation. This value is essential for converting Kc to Kp, as it indicates how the number of gas molecules changes during the reaction. A positive Δn suggests an increase in gas moles, while a negative Δn indicates a decrease, affecting the relationship between Kc and Kp.
추천 영상:
가이드 코스
03:42
Reversible Changes in Matter
관련 실천
교과서 질문

Consider the reactions and their respective equilibrium

constants:

NO(g) + 1/2 Br (g) ⇌ NOBr(g) Kp = 5.3

2 NO(g) ⇌ N2(g) + O2(g) Kp = 2.1⨉1030

Use these reactions and their equilibrium constants to predict

the equilibrium constant for the following reaction: N2(g) + O2(g) + Br2(g) ⇌ 2 NOBr(g)

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교과서 질문

Calculate Kc for each reaction.

b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kp = 7.7x1024 (at 298 K)

c. I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 (at 298 K)

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교과서 질문

Calculate Kc for each reaction. a. I2(g) ⇌ 2I(g) Kp = 6.26⨉10-22 (at 298K)

1992
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교과서 질문

Calculate Kp for each reaction.

b. N2(g) + 3 H2(g) ⇌ 2 NH3(g) Kc = 3.7⨉108 (at 298 K)

c. N2(g) + O2(g) ⇌ 2 NO(g) Kc = 4.10⨉10-31 (at 298 K)

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