Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Chapter 22, Problem 22.56QP
Interpretation Introduction
Interpretation: The equilibrium constant and
Concept Introduction:
Equilibrium constant: The equilibrium constant of a
Gibb’s free energy: The Gibb’s free energy also termed as the available energy; is the
To Calculate: The equilibrium constant and
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Chapter 22 Solutions
Chemistry: Atoms First
Ch. 22.1 - Prob. 22.1WECh. 22.1 - Give oxidation numbers for the metals in (a)...Ch. 22.1 - Prob. 1PPBCh. 22.1 - Prob. 1PPCCh. 22.1 - Write the names of the following coordination...Ch. 22.1 - Give the correct name for (a) [Co(NH3)4Br2]Cl, (b)...Ch. 22.1 - Prob. 2PPBCh. 22.1 - Prob. 2PPCCh. 22.1 - Prob. 22.3WECh. 22.1 - Prob. 3PPA
Ch. 22.1 - Prob. 3PPBCh. 22.1 - Prob. 3PPCCh. 22.1 - Prob. 22.1.1SRCh. 22.1 - Prob. 22.1.2SRCh. 22.1 - Prob. 22.1.3SRCh. 22.1 - Write the correct formula for...Ch. 22.3 - Prob. 22.4WECh. 22.3 - Prob. 4PPACh. 22.3 - Prob. 4PPBCh. 22.3 - Prob. 4PPCCh. 22.3 - Prob. 22.3.1SRCh. 22.3 - Prob. 22.3.2SRCh. 22 - What distinguishes a transition metal from a main...Ch. 22 - Prob. 22.2QPCh. 22 - Prob. 22.3QPCh. 22 - Without referring to the text, write the...Ch. 22 - Write the electron configurations of the following...Ch. 22 - Prob. 22.6QPCh. 22 - Prob. 22.7QPCh. 22 - Prob. 22.8QPCh. 22 - Describe the interaction between a donor atom and...Ch. 22 - Prob. 22.10QPCh. 22 - Prob. 22.11QPCh. 22 - Prob. 22.12QPCh. 22 - Prob. 22.13QPCh. 22 - What are the systematic names for the following...Ch. 22 - Prob. 22.15QPCh. 22 - Write the formulas for each of the following ions...Ch. 22 - Prob. 22.17QPCh. 22 - Prob. 22.18QPCh. 22 - Prob. 22.19QPCh. 22 - Prob. 22.20QPCh. 22 - Prob. 22.21QPCh. 22 - Prob. 22.22QPCh. 22 - Prob. 22.23QPCh. 22 - Prob. 22.24QPCh. 22 - Prob. 22.25QPCh. 22 - Briefly describe crystal field theory.Ch. 22 - Prob. 22.27QPCh. 22 - What is the origin of color in a coordination...Ch. 22 - Prob. 22.29QPCh. 22 - Prob. 22.30QPCh. 22 - Prob. 22.31QPCh. 22 - Prob. 22.32QPCh. 22 - The absorption maximum for the complex ion...Ch. 22 - Prob. 22.34QPCh. 22 - Prob. 22.35QPCh. 22 - Prob. 22.36QPCh. 22 - Prob. 22.37QPCh. 22 - Prob. 22.38QPCh. 22 - Prob. 22.39QPCh. 22 - Prob. 22.40QPCh. 22 - The [Fe(CN)6]3 complex is more labile than the...Ch. 22 - Prob. 22.42QPCh. 22 - Prob. 22.43QPCh. 22 - Prob. 22.44QPCh. 22 - Prob. 22.45QPCh. 22 - Prob. 22.46QPCh. 22 - Prob. 22.47QPCh. 22 - Prob. 22.48QPCh. 22 - Prob. 22.49QPCh. 22 - Prob. 22.50QPCh. 22 - Prob. 22.51QPCh. 22 - Prob. 22.52QPCh. 22 - Prob. 22.53QPCh. 22 - Prob. 22.54QPCh. 22 - A student in 1895 prepared three coordination...Ch. 22 - Prob. 22.56QPCh. 22 - Prob. 22.57QPCh. 22 - Prob. 22.58QPCh. 22 - Prob. 22.59QPCh. 22 - Prob. 22.60QPCh. 22 - Prob. 22.61QPCh. 22 - Hydrated Mn2+ ions are practically colorless (see...Ch. 22 - Which of the following hydrated cations are...Ch. 22 - Prob. 22.64QPCh. 22 - Prob. 22.65QPCh. 22 - Prob. 22.66QPCh. 22 - Prob. 22.67QPCh. 22 - Prob. 22.68QPCh. 22 - Prob. 22.69QPCh. 22 - Prob. 22.70QPCh. 22 - Commercial silver-plating operations frequently...Ch. 22 - Prob. 22.72QPCh. 22 - Prob. 22.73QPCh. 22 - Prob. 22.74QPCh. 22 - Prob. 22.75QPCh. 22 - Prob. 22.76QPCh. 22 - Prob. 22.77QPCh. 22 - Prob. 22.78QPCh. 22 - Prob. 22.79QPCh. 22 - Prob. 22.80QP
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- MnO−4 reacts with Fe2+ in acid solution to produce Fe3+ and Mn2+. Write a balanced equation for this reaction. (include phases (g)(l)(s)arrow_forwardCalculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and twice that molar concentration of thiosulfate ions at equilibrium? The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. Your answer should have 2 sig figs.arrow_forwardConsider the following equation: [Ni(H2O)6]2+ + 6NH3 <----> [Ni(NH3)6]2+ +6H2O The effects of stress on this equilibrium can be monitored by changes in color. An equilibrium mixture is blue-green (indicating both products and reactants are present). a.) When the equilibrium mixture is heated, the color changes to bright green. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? Which is the exothermic direction of this reaction? Forward, reverse, or cannot tell? b.) When a few drops of concentrated NH3 are added to the equilibrium mixture, the solution turns deep blue. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? c.) Addition of concentrated HNO3 to the blue-green mixture will remove NH3 by reaction. What should happen to the color of the solution? Will it turn more blue, turn more green, or no change? Explain.arrow_forward
- Write the following equilibrium-constant expressions:(a) Kc for Cr(s) + 3 Ag+(aq) ⇌ Cr3+(aq) + 3 Ag(s),(b) Kp for 3 Fe(s) + 4 H2O(g) ⇌ Fe3O4(s) + 4 H2(g).arrow_forwardFor each of the following reactions, identify the acid and the base. Also indicate which acid-base definition is most applicable. Fe3+ + 6 SCN– →[Fe(SCN)6]3– HClO4 + (CH3)3N → (CH3)3NH+ + ClO4– [Co(H2O)6]2+ + 4 HCl → [CoCl4]2– + 4 H3O+ + 2 H2Oarrow_forwardIn the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+. Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+ + 3H2O ↔ [Al(H2O)3(OH)3]2+ + 3H3O+arrow_forward
- Use the thermodynamic data given below to compute the formation constant, Kf for [Zn(NH3)4]2+ in aqueous solution at 337.0 K. Species ΔfH0kJ/mol S0J/mol/K NH3(aq) -80.29 111.3 Zn2+(aq) -153.89 -112.1 [Zn(NH3)4]2+(aq) -533.5 301 Include 3 significant figuresarrow_forwardWrite the expression for the equilibrium constant Kc for the following equation. FeO(s) + CO(g) ↔ Fe(s) + CO2(g)arrow_forwardWrite the balanced equation that accounts for the source of OH- used in the following reactions: [Al(H2O)6]3+(aq) + 3 OH-(aq) = Al(OH)3(s) + 6 H2O(l) [FeCl4]-(aq) + 3 OH-(aq) = Fe(OH)3(s) + 4 Cl-(aq)arrow_forward
- The standard reduction potential for the reaction [Co(H2 O)6]3+(aq) + e− ⟶ [Co(H2 O)6]2+(aq) is about 1.8 V. The reduction potential for the reaction [Co(NH3)6]3+(aq) + e− ⟶ [Co(NH3)6]2+(aq) is +0.1 V. Calculate the cell potentials to show whether the complex ions, [Co(H2O)6]2+ and/or [Co(NH3)6]2+, can be oxidized to the corresponding cobalt(III) complex by oxygen.arrow_forwardWhat is the concentration of Ag+ at equilibrium in the following reaction when carried out at 238 K and [Fe2+] = [Fe3+] = 0.3 M at equilibrium?arrow_forwardGiven the following equilibria, Ni2+(aq) + 2 OH–(aq) Ni(OH)2(s) K1 = 1.8 × 1015 Ni2+(aq) + 4 CN–(aq) Ni(CN)42–(aq) K2 = 2.0 × 1031 determine the equilibrium constant, Kc, for the following reaction. Ni(OH)2(s) + 4 CN–(aq) Ni(CN)42–(aq) + 2 OH–(aq) Group of answer choicesarrow_forward
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