Textbook Question
(a) Based on the following energy profile, predict whether kf > kr or kf < kr. [Section 15.1]
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Ch.15 - Chemical Equilibrium
Chapter 15, Problem 3
Consider the equilibrium Na2O(s) + SO2(g) ⇌ Na2SO3(s). (a) Write the equilibrium-constant expression for this reaction in terms of partial pressures. (b) All the compounds in this reaction are soluble in water. Rewrite the equilibrium-constant expression in terms of molarities for the aqueous reaction.
Verified step by step guidance1
Step 1: Identify the phases of each compound in the reaction. Na2O is a solid, SO2 is a gas, and Na2SO3 is a solid.
Step 2: Write the equilibrium-constant expression for the reaction in terms of partial pressures. Since solids do not appear in the expression, only the gaseous component, SO2, is included. The expression is K_p = 1/P_{SO2}.
Step 3: Consider the aqueous reaction where all compounds are soluble in water. In this case, all species are in the aqueous phase, and we use molarities to express the equilibrium constant.
Step 4: Write the equilibrium-constant expression for the aqueous reaction in terms of molarities. The expression is K_c = [Na2SO3]/([Na2O][SO2]).
Step 5: Note that in the aqueous expression, the concentration of solids is typically considered constant and thus omitted, simplifying the expression to K_c = 1/[SO2].
Related Practice
Textbook Question
The following diagrams represent a hypothetical reaction A ¡ B, with A represented by red spheres and B represented by blue spheres. The sequence from left to right represents the system as time passes. Does the system reach equilibrium? If so, in which diagram(s) is the system in equilibrium? [Sections 15.1 and 15.2]
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Textbook Question
The following diagram represents a reaction shown going to completion. Each molecule in the diagram represents 0.1 mol, and the volume of the box is 1.0 L. (d) Assuming that all of the molecules are in the gas phase, calculate n, the change in the number of gas molecules that accompanies the reaction. [Section 15.2]
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Textbook Question
Ethene (C2H4) reacts with halogens (X2) by the following reaction:
C2H4(𝑔) + X2(𝑔) ⇌ C2H4X2(𝑔)
The following figures represent the concentrations at equilibrium at the same temperature when X2 is Cl2 (green), Br2 (brown), and I2 (purple). List the equilibria from smallest to largest equilibrium constant. [Section 15.3]
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Textbook Question
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? a. There will be less PbO2 remaining in vessel A,
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