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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 31a
15장, 문제 31a

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

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1
Identify the given values and the required conversion: You are given the equilibrium constant in terms of pressure (Kp) and need to calculate the equilibrium constant in terms of concentration (Kc) for the reaction at a specific temperature (298K).
Write down the balanced chemical equation for the reaction: I2(g) ⇌ 2I(g).
Use the relationship between Kp and Kc, which is Kp = Kc(RT)^Δn, where R is the gas constant (0.0821 L atm K^-1 mol^-1), T is the temperature in Kelvin, and Δn is the change in moles of gas (moles of products - moles of reactants).
Calculate Δn for the reaction: Δn = 2 (moles of I) - 1 (moles of I2) = 1.
Substitute the values of Kp, R, T, and Δn into the formula to solve for Kc: Kc = Kp / (RT)^Δn.

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 (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. 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

Relationship Between Kc and Kp

Kc and Kp are related through the ideal gas law and the stoichiometry of the reaction. For reactions involving gases, the conversion between Kc and Kp depends on the difference in the number of moles of gaseous products and reactants. This relationship allows for the calculation of one constant if the other is known, provided the temperature remains constant.
추천 영상:
가이드 코스
02:18
Kp vs Kc Relationship

Stoichiometry of the Reaction

Stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction. In the given reaction, I2(g) ⇌ 2I(g), the stoichiometry indicates that one mole of iodine gas dissociates into two moles of iodine atoms. This stoichiometric ratio is crucial for calculating Kc from Kp, as it directly influences the value of Δn in the Kp-Kc relationship.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept
관련 실천
교과서 질문

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

b. 6 COF2(g) ⇌ 3 CO2(g) + 3 CF4(g)

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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)

4660
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교과서 질문

This reaction has an equilibrium constant of Kp = 2.2⨉106 at 298 K. 2 COF2(g) ⇌ CO2(g) + CF4(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium.

c. 2 CO2(g) + 2 CF4(g) ⇌ 4 COF2(g)

631
views
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)

6847
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교과서 질문

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

3548
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