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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.15 - Chemical Equilibrium문제 42b
15장, 문제 42b

(b) At the start of a certain reaction, only reactants are present; no products have been formed. What is the value of Qc at this point in the reaction?

검증된 단계별 안내
1
Understand that Qc, the reaction quotient, is a measure of the relative amounts of products and reactants present during a reaction at a given point in time.
Recall that the expression for Qc is similar to the equilibrium constant (Kc), but it can be calculated at any point in the reaction, not just at equilibrium.
The formula for Qc is: \( Q_c = \frac{[C]^c[D]^d}{[A]^a[B]^b} \), where [C] and [D] are the concentrations of the products, and [A] and [B] are the concentrations of the reactants, with a, b, c, and d being their respective stoichiometric coefficients.
At the start of the reaction, only reactants are present, meaning the concentrations of the products are zero.
Since the concentrations of the products are zero, the numerator of the Qc expression is zero, making Qc equal to zero at the start of the reaction.

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주요 개념

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Reaction Quotient (Qc)

The reaction quotient, Qc, is a measure of the relative concentrations of products and reactants at any point in a chemical reaction. It is calculated using the same expression as the equilibrium constant (Kc), but for non-equilibrium conditions. Qc helps determine the direction in which a reaction will proceed to reach equilibrium.
추천 영상:
가이드 코스
00:49
Reaction Quotient Q

Initial Conditions of a Reaction

At the start of a reaction, only reactants are present, meaning the concentrations of products are zero. This initial state is crucial for calculating Qc, as it reflects the system's starting point before any reaction occurs. Understanding these initial conditions allows for predicting how the reaction will shift as it progresses toward equilibrium.
추천 영상:
가이드 코스
01:13
Benzene Reactions

Equilibrium and Reaction Direction

The value of Qc at any point in a reaction indicates whether the system is at equilibrium, or if it will shift toward products or reactants. If Qc is less than Kc, the reaction will proceed forward to produce more products; if Qc is greater than Kc, the reaction will shift backward to form more reactants. This concept is essential for understanding how reactions progress over time.
추천 영상:
가이드 코스
01:14
Equilibrium Constant K
관련 실천
교과서 질문

(a) If Qc < Kc, in which direction will a reaction proceed in order to reach equilibrium?

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교과서 질문

(a) If Qc > Kc, how must the reaction proceed to reach equilibrium?

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교과서 질문

At 100°C, the equilibrium constant for the reaction COCl2(𝑔) ⇌ CO(𝑔) + Cl2(𝑔) has the value 𝐾𝑐 = 2.19×10−10. Are the following mixtures of COCl2, CO, and Cl2 at 100°C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium.

(a) [COCl2] = 2.00×10−3 M, [CO] = 3.3×10−6 M, [Cl2] = 6.62×10−6 M

(b) [COCl2] = 4.50×10−2 M, [CO] = 1.1×10−7 M, [Cl2] = 2.25×10−6 M

(c) [COCl2] = 0.0100 M, [CO] = [Cl2] = 1.48×10−6 M

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교과서 질문

(b) What condition must be satisfied so that Qc = Kc?

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