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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 95
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Chapter 15, Problem 95

Consider the reaction IO4- (aq) + 2 H2O (l) ⇌ H4IO6- (aq); Kc = 3.5 * 10^-2. If you start with 25.0 mL of a 0.905 M solution of NaIO4 and then dilute it with water to 500.0 mL, what is the concentration of H4IO6- at equilibrium?

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1
Calculate the initial concentration of IO4^- after dilution. Use the dilution formula: C1V1 = C2V2, where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.
Set up an ICE (Initial, Change, Equilibrium) table to determine the changes in concentration for the reaction IO4^- + 2 H2O ⇌ H4IO6^- at equilibrium. Start with the initial concentration of IO4^- and assume the initial concentration of H4IO6^- is zero.
Define the change in concentration of IO4^- as -x and the change in concentration of H4IO6^- as +x, since the stoichiometry of the reaction shows a 1:1 ratio between IO4^- and H4IO6^-.
Write the expression for the equilibrium constant Kc in terms of the concentrations at equilibrium: Kc = [H4IO6^-] / [IO4^-]. Substitute the equilibrium concentrations from the ICE table into this expression.
Solve the equation for x, which represents the equilibrium concentration of H4IO6^-. This will involve substituting the known value of Kc and solving for x algebraically.
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Open Question
An equilibrium mixture of H2, I2, and HI at 458 _x001F_C contains 0.112 mol H2, 0.112 mol I2, and 0.775 mol HI in a 5.00-L vessel. What are the equilibrium partial pressures when equilibrium is reestablished following the addition of 0.200 mol of HI?
Textbook Question

Consider the hypothetical reaction A(𝑔) + 2  B(𝑔) ⇌ 2 C(𝑔), for which 𝐾𝑐 = 0.25 at a certain temperature. A 1.00-L reaction vessel is loaded with 1.00 mol of compound C, which is allowed to reach equilibrium. Let the variable x represent the number of mol/L of compound A present at equilibrium. (e) From the plot in part (d), estimate the equilibrium concentrations of A, B, and C. (Hint: You can check the accuracy of your answer by substituting these concentrations into the equilibrium expression.)

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Textbook Question

At a temperature of 700 K, the forward and reverse rate constants for the reaction 2 HI(𝑔) ⇌ H2(𝑔) + I2(𝑔) are 𝑘𝑓=1.8×10−3 𝑀−1s−1 and 𝑘𝑟 = 0.063  𝑀−1s−1. (b) Is the forward reaction endothermic or exothermic if the rate constants for the same reaction have values of 𝑘𝑓 = 0.097 𝑀−1s−1 and 𝑘𝑟 = 2.6 𝑀−1s−1 at 800 K?

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Textbook Question

The following equilibria were measured at 823 K: CoO1s2 + H21g2 ΔCo1s2 + H2O1g2 Kc = 67 H21g2 + CO21g2 ΔCO1g2 + H2O1g2 Kc = 0.14 (a) Use these equilibria to calculate the equilibrium constant, Kc, for the reaction CoO1s2 + CO1g2ΔCo1s2 + CO21g2 at 823 K.

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Textbook Question

The following equilibria were measured at 823 K: CoO1s2 + H21g2 ΔCo1s2 + H2O1g2 Kc = 67 H21g2 + CO21g2 ΔCO1g2 + H2O1g2 Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO1s2 remains?

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Textbook Question

The phase diagram for SO2 is shown here. (d) At which of the three points marked in red does SO2(g) most closely approach ideal-gas behavior?

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