Textbook Question
The reaction 2 AsH31g2 ∆ As21g2 + 3 H21g2 has Kp =
7.2 * 107 at 1073 K. At the same temperature, what is Kp
for each of the following reactions?
(b) 4 AsH31g2 ∆ 2 As21g2 + 6 H21g2
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 15.64
Calculate the value of the equilibrium constant at 427 °C for the reaction
Na O1s2 + 1>2 O 1g2 ∆ Na O 1s2
given the following equilibrium constants at 427 °C.
Na2O1s2 ∆ 2 Na1l2 + 1>2 O21g2 Kc = 2 * 10-25 Na O 1s2 ∆ 2 Na1l2 + O 1g2 K = 5 * 10-29
Verified step by step guidance1
Identify the target reaction and the given reactions. The target reaction is Na2O(s) + 1/2 O2(g) ⇌ Na2O2(s). The given reactions are: (1) Na2O(s) ⇌ 2 Na(l) + 1/2 O2(g) with Kc = 2 * 10^-25, and (2) Na2O2(s) ⇌ 2 Na(l) + O2(g) with K = 5 * 10^-29.
Write the reverse of the second given reaction to align with the formation of Na2O2(s) from Na(l) and O2(g), which is 2 Na(l) + O2(g) ⇌ Na2O2(s). The equilibrium constant for this reverse reaction will be the reciprocal of the given K, which is 1/(5 * 10^-29).
Combine the first given reaction with the reversed second reaction to achieve the target reaction. This involves adding the first reaction to the reversed second reaction. The combined reaction should yield Na2O(s) + 1/2 O2(g) ⇌ Na2O2(s).
Apply the law of mass action to find the equilibrium constant for the target reaction, K_target. The equilibrium constant for a reaction obtained by adding two reactions is the product of the equilibrium constants of the individual reactions. Therefore, K_target = Kc for the first reaction * K for the reversed second reaction.
Calculate K_target using the values of Kc and K from the previous steps. This will give the equilibrium constant for the target reaction at 427 °C.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
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 temperature-dependent and provides insight into the extent of a reaction; a larger K indicates a greater concentration of products at equilibrium, while a smaller K suggests that reactants are favored.
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Equilibrium Constant K
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 is crucial for predicting how changes in concentration, pressure, or temperature will affect the position of equilibrium in a chemical reaction.
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07:32Le Chatelier's Principle
Reaction Stoichiometry
Reaction stoichiometry involves the quantitative relationships between the reactants and products in a chemical reaction, as described by the balanced chemical equation. Understanding stoichiometry is essential for calculating equilibrium constants, as it allows for the proper interpretation of the coefficients in the balanced equation, which directly influence the equilibrium expression.
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01:16Stoichiometry Concept
Related Practice
Textbook Question
The reaction 2 AsH31g2 ∆ As21g2 + 3 H21g2 has Kp =
7.2 * 107 at 1073 K. At the same temperature, what is Kp
for each of the following reactions?
(c) 9 H21g2 + 3 As21g2 ∆ 6 AsH31g2
Textbook Question
The reaction
2 PH31g2 + As21g2 ∆ 2 AsH31g2 + P21g2
has Kp = 2.9 * 10-5 at 873 K. At the same temperature,
what is Kp for each of the following reactions?
(a) 2 AsH31g2 + P21g2 ∆ 2 PH31g2 + As21g2
Textbook Question
Calculate the value of the equilibrium constant for the reaction 4 NH31g2 + 3 O21g2 ∆ 2 N21g2 + 6 H2O1g2
given the following equilibrium constants at a certain temperature.
2 H21g2 + O21g2 ∆ 2 H2O1g2 Kc = 3.2 * 1081
N21g2 + 3 H21g2 ∆ 2 NH31g2 Kc = 3.5 * 108
Textbook Question
Consider the interconversion of A molecules (red spheres) and B molecules (blue spheres) according to the reaction A ∆ B. Each of the series of pictures at the right represents a separate experiment in which time increases from left to right:(b) What is the value of the equilibrium constant Kc for the reaction A ∆ B?
Textbook Question
The reaction A2 + B ∆ A + AB has an equilibrium con-stant Kc = 2. The following pictures represent reaction mix- tures that contain A atoms (red), B atoms (blue), and A2 and AB molecules. (a) Which reaction mixture is at equilibrium?