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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 10a
15장, 문제 10a

The diagram shown here represents the equilibrium state for the reaction A2(𝑔) + 2B(𝑔) ⇌ 2AB(𝑔). (a) Assuming the volume is 2 L, calculate the equilibrium constant 𝐾𝑐 for the reaction.

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Step 1: Identify the equilibrium concentrations of the reactants and products from the diagram. The number of molecules of each species in the diagram represents the number of moles of that species. Divide the number of moles by the volume (2 L) to get the molar concentration.
Step 2: Write the expression for the equilibrium constant, Kc, for the reaction. For the reaction A2(g) + 2B(g) ⇌ 2AB(g), the equilibrium constant expression is Kc = [AB]^2 / ([A2][B]^2).
Step 3: Substitute the equilibrium concentrations from Step 1 into the equilibrium constant expression from Step 2. Remember that the concentrations should be in moles per liter (M).
Step 4: Perform the calculations as indicated in the equilibrium constant expression. Remember to square the concentration of AB and B as indicated in the equilibrium constant expression.
Step 5: The result of these calculations is the equilibrium constant, Kc, for the reaction. This value indicates the extent to which the reaction proceeds to the right (towards the products) at equilibrium.

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주요 개념

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Equilibrium Constant (Kc)

The equilibrium constant, Kc, is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the formula Kc = [products]^[coefficients] / [reactants]^[coefficients]. A Kc value greater than 1 indicates that products are favored at equilibrium, while a value less than 1 suggests that reactants are favored.
추천 영상:
가이드 코스
03:20
Equilibrium Constant Expressions

Concentration

Concentration refers to the amount of a substance (solute) present in a given volume of solution. It is typically expressed in moles per liter (Molarity, M). In equilibrium calculations, the concentrations of the reactants and products at equilibrium are essential for determining the value of Kc, as they directly influence the ratio used in the equilibrium expression.
추천 영상:
가이드 코스
07:35
Calculate Concentration of the Basic Form

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It involves using the coefficients from the balanced chemical equation to relate the amounts of substances consumed and produced. In the context of equilibrium, stoichiometry is crucial for determining the concentrations of reactants and products based on their initial amounts and the changes that occur as the system reaches equilibrium.
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가이드 코스
01:16
Stoichiometry Concept
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교과서 질문

The equilibrium constant for the dissociation of molecular iodine, I2(g) ⇌ 2 I(g), at 800 K is Kc = 3.1 × 10–5. (a) Which species predominates at equilibrium I2 or I?

교과서 질문

The reaction A2 + B2 ⇌ 2 AB has an equilibrium constant Kc = 1.5. The following diagrams represent reaction mixtures containing A2 molecules (red), B2 molecules (blue), and AB molecules. (a) Which reaction mixture is at equilibrium?

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교과서 질문

The equilibrium constant for the dissociation of molecular iodine, I2(g) ⇌ 2 I(g), at 800 K is Kc = 3.1×10−5. (b) Assuming both forward and reverse reactions are elementary reactions, which reaction has the larger rate constant, the forward or the reverse reaction?

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교과서 질문

When lead(IV) oxide is heated above 300°C, it decomposes according to the reaction, 2 PbO2(𝑠) ⇌ 2PbO(𝑠) + O2(𝑔). Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400°C and allowed to come to equilibrium, which of the following statements is or are true? (c) The amount of PbO2 remaining in each vessel will be the same. [Find more in Section 15.4]

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교과서 질문

Suppose that the gas-phase reactions A → B and B → A are both elementary reactions with rate constants of 4.7×10−3 s−1 and 5.8×10−1 s−1, respectively. (a) What is the value of the equilibrium constant for the equilibrium A(g) ⇌ B(g)? (b) Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?

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