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Ch.7 Chemical Reactions: Energy, Rate and Equilibrium
McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.7 Chemical Reactions: Energy, Rate and EquilibriumProblema 56a
Capitolo 7, Problema 56a

Use your answer from Problem 7.54 to calculate the following:
a. [O2] at equilibrium when [CO2] = 0.18 mol/L and [CO] = 0.0200 mol/L

Guida verificata passo dopo passo
1
Identify the chemical equilibrium reaction involved. For example, if the reaction is CO(g) + 1/2 O2(g) ⇌ CO2(g), write the balanced equation and note the stoichiometric relationships between the reactants and products.
Write the equilibrium constant expression (Kc) for the reaction. For the example reaction, Kc = ([CO2]) / ([CO] * [O2]^(1/2)).
Substitute the given equilibrium concentrations into the Kc expression. In this case, [CO2] = 0.18 mol/L and [CO] = 0.0200 mol/L. Let [O2] = x, which is the unknown concentration to solve for.
Rearrange the Kc expression to isolate [O2]. For the example reaction, this would involve solving for x in the equation Kc = (0.18) / (0.0200 * x^(1/2)).
Use the value of Kc from Problem 7.54 (provided in the earlier problem) to solve for x, which represents the equilibrium concentration of O2. Ensure proper algebraic manipulation and square both sides if necessary to eliminate the square root.

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Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given chemical reaction. It is specific to a particular reaction at a certain temperature. Understanding K is essential for predicting the concentrations of reactants and products when the system reaches equilibrium.
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The Equilibrium Constant Concept 1

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. This principle helps in predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.
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The following is an endothermic reaction where Kc = 6.73 x 103.For each of the choices below predict in which direction the reaction will proceed

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows for the determination of the relationships between the amounts of substances consumed and produced, which is crucial for calculating equilibrium concentrations when given specific initial conditions.
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Stoichiometry
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Domanda del libro di testo

Oxygen can be converted into ozone by the action of lightning or electric sparks:

3 O2(g) ⇌ 2 O3(g)

For this reaction, ∆H = +69kcal/mol (+285 kj/mol) and K = 2.68 × 10-29 at 25 °C.

b. Are the reactants or the products favored at equilibrium?

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Write the equilibrium constant expressions for the following reactions:

a. 2 CO(g) + O2(g) ⇌ 2 CO2(g)

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Hydrogen chloride can be made from the reaction of chlorine and hydrogen:

Cl2(g) + H2(g) → 2 HCl(g)

For this reaction, K = 26 × 1033 and ∆H = -44 kcal/mol(-184 kJ/mol) at 25 °C.

a. Is the reaction endothermic or exothermic?

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Domanda del libro di testo

Oxygen can be converted into ozone by the action of lightning or electric sparks:

3 O2(g) ⇌ 2 O3(g)

For this reaction, ∆H = +69kcal/mol (+285 kj/mol) and K = 2.68 × 10-29 at 25 °C.

a. Is the reaction exothermic or endothermic?

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Write the equilibrium constant expressions for the following reactions.

d. C(s) + H2O(g) ⇌ CO(g) + H2(g)

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Use your answer from Problem 7.53 to calculate the following:

a. [N2O4] at equilibrium when [NO2] = 0.0250 mol/L

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