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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 31b,c
15장, 문제 31b,c

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)

검증된 단계별 안내
1
Identify the relationship between Kc and Kp using the equation: Kc = Kp(RT)^-Δn, where R is the ideal gas constant (0.0821 L·atm/mol·K) and T is the temperature in Kelvin.
Determine Δn, the change in moles of gas, by subtracting the sum of the moles of gaseous reactants from the sum of the moles of gaseous products. For the given reaction, Δn = (1 + 3) - (1 + 1).
Substitute the given values into the equation: Kc = 7.7x10^24 * (0.0821 * 298)^-Δn.
Calculate the value of (RT)^-Δn using the values of R, T, and Δn.
Multiply Kp by the calculated value of (RT)^-Δn to find Kc.

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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. Understanding this relationship is crucial for converting between Kc and Kp.
추천 영상:
가이드 코스
02:06
Kp vs. Kc Formula

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in a reaction, not just at equilibrium. It is calculated using the same formula as K, but with the current concentrations or pressures. Comparing Q to K helps predict the direction in which a reaction will proceed to reach equilibrium, which is essential for understanding dynamic chemical systems.
추천 영상:
가이드 코스
00:49
Reaction Quotient Q

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by changes in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is vital for predicting how changes in conditions will affect the position of equilibrium and the values of Kc and Kp in a given reaction.
추천 영상:
가이드 코스
07:32
Le Chatelier's Principle
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

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)

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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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교과서 질문

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

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