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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: 9780134015187당신이 사용하는 게 아니라요?교과서 변경
모든 교과서McMurry 8th EditionCh.7 Chemical Reactions: Energy, Rate and Equilibrium문제 55a
7장, 문제 55a

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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1
Identify the chemical equilibrium reaction involved. The reaction is typically: N₂O₄ ⇌ 2NO₂. This means dinitrogen tetroxide (N₂O₄) dissociates into nitrogen dioxide (NO₂).
Write the equilibrium constant expression for the reaction: Kc = ([NO₂]²) / [N₂O₄]. Here, [NO₂] and [N₂O₄] represent the equilibrium concentrations of NO₂ and N₂O₄, respectively.
Rearrange the equilibrium constant expression to solve for [N₂O₄]: [N₂O₄] = ([NO₂]²) / Kc. This step isolates the concentration of N₂O₄ at equilibrium.
Substitute the given value of [NO₂] = 0.0250 mol/L into the rearranged equation. You will also need the value of Kc, which should have been determined in Problem 7.53. Ensure the units of Kc are consistent with the concentration units (mol/L).
Perform the calculation by squaring the [NO₂] value, dividing it by the Kc value, and solving for [N₂O₄]. This will give you the equilibrium concentration of N₂O₄ in mol/L.

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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]. Understanding Kc is essential for predicting the concentrations of species in a chemical reaction at equilibrium.
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02:50
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 understanding how changes in concentration, pressure, or temperature affect the position of equilibrium in a chemical reaction.
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09:34
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 is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It involves using mole ratios derived from the coefficients of the balanced equation to relate the amounts of different substances. Mastery of stoichiometry is crucial for determining the concentrations of reactants and products at equilibrium.
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01:16
Stoichiometry
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교과서 질문

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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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

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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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Why do catalysts not alter the amounts of reactants and products present at equilibrium?

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교과서 질문

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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교과서 질문

Write the equilibrium constant expressions for the following reactions.

d. C(s) + H2O(g) ⇌ CO(g) + H2(g)

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