Textbook Question
If Kc = 7.5×10−9 at 1000 K for the reaction N2(g) + O2(g) → 2 NO(g), give the value of Kc at 1000 K for the reaction
(a) 2 NO(g) → N2(g) + O2(g)
114
views
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 15.62c
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
Verified step by step guidance1
Identify the relationship between the given reaction and the target reaction. The target reaction can be derived by reversing the given reaction and then multiplying it by 3.
Write the expression for the equilibrium constant (Kp) for the given reaction: Kp = [As2]^2 * [H2]^3 / [AsH3]^2.
For the reversed reaction, the equilibrium constant expression will be the reciprocal of the original reaction's Kp. Thus, Kp' = 1 / Kp.
Since the target reaction is 3 times the reversed reaction, raise the Kp' to the power of 3 to find the new Kp for the target reaction: Kp'' = (Kp')^3.
Substitute the value of Kp from the given reaction into the expression derived in step 4 to find the Kp for the target reaction.
Verified Solution
Video duration:
4m
This video solution was recommended by our tutors as helpful for the problem above.Was this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Equilibrium Constant (Kp)
The equilibrium constant, Kp, is a numerical value that expresses the ratio of the partial pressures of the products to the reactants at equilibrium for a given reaction at a specific temperature. It is derived from the balanced chemical equation and indicates the extent to which a reaction favors products or reactants. A larger Kp value suggests a greater concentration of products at equilibrium.
Recommended video:
Guided course
03:20
Equilibrium Constant Expressions
Reaction Stoichiometry
Reaction stoichiometry refers to the quantitative relationship between the reactants and products in a chemical reaction, as represented by the coefficients in a balanced equation. This concept is crucial for determining how changes in the amounts of reactants or products affect the equilibrium position and the calculation of equilibrium constants for related reactions.
Recommended video:
Guided course
01:16Stoichiometry Concept
Reverse Reaction and Kp Relationship
The equilibrium constant for a reverse reaction is the reciprocal of the equilibrium constant for the forward reaction. If a reaction is reversed, the Kp value must be inverted to reflect the new direction of the reaction. This relationship is essential for calculating Kp for different but related reactions, as seen in the provided question.
Recommended video:
Guided course
02:18Kp vs Kc Relationship
Related Practice
Textbook Question
If Kc = 7.5×10−9 at 1000 K for the reaction N2(g) + O2(g) → 2 NO(g), give the value of Kc at 1000 K for the reaction
(b) NO(g) → 1/2 N2(g) + 1/2 O2(g)
89
views
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
102
views
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
95
views
Textbook Question
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
127
views
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
127
views