Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 17, Problem 17.89QE
For each reaction, an equilibrium constant at 298 K is given. Calculate ΔG° for each reaction.
(a) H+(aq) + OH-(aq)⇋H2O Kc = 1.0 × 10−14
(b) CaSO4(s)⇋Ca2+(aq) +
(c) HIO3(aq)⇋H+(aq) +
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
At 25oC, the equilibrium constant for the reaction 2 A(aq) ----> B(aq) + C(aq) is 1.91 . If the concentration of B(aq) is 0.399 M and the concentration of C(aq) is 0.502 M, what would be the minimal concentration of A(aq) (in mol/L) required to make the reaction spontaneous?
At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.79 . If the concentration of B(aq) were 0.311 M and the concentration of C(aq) were 0.477 M, what would be the minimum concentration of A(aq) required (in mol/L) to make this reaction spontaneous under these conditions?
Calculate the KP for the following reaction at 25°C:
H2(g) + I2(g) ⇌ 2HI(g) ΔGo = 2.60 kJ/mol
Chapter 17 Solutions
Chemistry: Principles and Practice
Ch. 17 - Prob. 17.1QECh. 17 - How is the sign of q, heat, defined? How does it...Ch. 17 - Identify the sign of the work when a fuel-oxygen...Ch. 17 - What is the sign of the work when a refrigerator...Ch. 17 - When a rocket is launched, the burning gases are...Ch. 17 - Prob. 17.6QECh. 17 - Prob. 17.7QECh. 17 - Prob. 17.8QECh. 17 - Prob. 17.9QECh. 17 - Explain why absolute enthalpies and energies...
Ch. 17 - Explain why absolute entropies can be measured.Ch. 17 - Under what conditions is the entropy of a...Ch. 17 - Prob. 17.13QECh. 17 - Prob. 17.14QECh. 17 - Prob. 17.15QECh. 17 - Prob. 17.16QECh. 17 - Prob. 17.17QECh. 17 - Prob. 17.18QECh. 17 - The free energy for a reaction decreases as...Ch. 17 - The equilibrium constant for a reaction decreases...Ch. 17 - When solid sodium acetate crystallizes from a...Ch. 17 - Prob. 17.22QECh. 17 - Prob. 17.23QECh. 17 - Prob. 17.24QECh. 17 - Prob. 17.25QECh. 17 - Prob. 17.26QECh. 17 - Prob. 17.27QECh. 17 - Calculate w for the following reactions that occur...Ch. 17 - How much work is done if a balloon expands from...Ch. 17 - Prob. 17.30QECh. 17 - Prob. 17.31QECh. 17 - A piston initially contains 688 mL of gas at 1.22...Ch. 17 - A 220-L cylinder contains an ideal gas at a...Ch. 17 - Prob. 17.34QECh. 17 - Prob. 17.35QECh. 17 - For a process, w = 34 J and q = 109 J. What is E...Ch. 17 - Prob. 17.37QECh. 17 - Prob. 17.38QECh. 17 - A reaction between a solid and a liquid produces...Ch. 17 - Prob. 17.40QECh. 17 - Prob. 17.41QECh. 17 - When an ideal gas is compressed at constant...Ch. 17 - Prob. 17.43QECh. 17 - Prob. 17.44QECh. 17 - Prob. 17.45QECh. 17 - Prob. 17.46QECh. 17 - Prob. 17.47QECh. 17 - Prob. 17.48QECh. 17 - What is the sign of the entropy change for each of...Ch. 17 - For each process, tell whether the entropy change...Ch. 17 - Prob. 17.51QECh. 17 - Prob. 17.52QECh. 17 - Prob. 17.53QECh. 17 - Prob. 17.54QECh. 17 - Use the data in Appendix G to calculate the...Ch. 17 - Prob. 17.56QECh. 17 - Prob. 17.57QECh. 17 - Prob. 17.58QECh. 17 - Calculate G for the following reactions and state...Ch. 17 - Prob. 17.60QECh. 17 - Prob. 17.63QECh. 17 - Prob. 17.64QECh. 17 - Prob. 17.65QECh. 17 - Prob. 17.66QECh. 17 - What is the sign of the standard Gibbs free-energy...Ch. 17 - What is the sign of the standard Gibbs free-energy...Ch. 17 - What is the sign of the standard Gibbs free-energy...Ch. 17 - What is the sign of the standard Gibbs free-energy...Ch. 17 - Predict the temperature at which the reaction in...Ch. 17 - Prob. 17.72QECh. 17 - Prob. 17.73QECh. 17 - Prob. 17.74QECh. 17 - Prob. 17.75QECh. 17 - Prob. 17.76QECh. 17 - Prob. 17.77QECh. 17 - Prob. 17.78QECh. 17 - Prob. 17.79QECh. 17 - Prob. 17.80QECh. 17 - Prob. 17.81QECh. 17 - Determine whether the condensation of nitromethane...Ch. 17 - At 298 K, G = 70.52 kJ for the reaction 2NO(g) +...Ch. 17 - Prob. 17.84QECh. 17 - Prob. 17.85QECh. 17 - Prob. 17.86QECh. 17 - Prob. 17.87QECh. 17 - Prob. 17.88QECh. 17 - For each reaction, an equilibrium constant at 298...Ch. 17 - For each reaction, an equilibrium constant at 298...Ch. 17 - Prob. 17.91QECh. 17 - Use the data in Appendix G to calculate the value...Ch. 17 - Suppose you have an endothermic reaction with H =...Ch. 17 - Suppose you have an endothermic reaction with H =...Ch. 17 - Suppose you have an exothermic reaction with H =...Ch. 17 - Suppose you have an exothermic reaction with H =...Ch. 17 - Calculate G and G at 303 C for the following...Ch. 17 - Calculate G and G at 37 C for the following...Ch. 17 - Prob. 17.101QECh. 17 - Prob. 17.102QECh. 17 - A 220-ft3 sample of gas at standard temperature...Ch. 17 - What is the sign of the standard Gibbs free-energy...Ch. 17 - Elemental boron, in the form of thin fibers, can...Ch. 17 - Calculate the standard Gibbs free-energy change...Ch. 17 - The thermite reaction is 2Al(s) + Fe2O3(s) ...Ch. 17 - Chemists and engineers who design nuclear power...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Calculate the equilibrium constant at 25 C for each of the following reactions from the value G given. (a) I2(s)+Cl2(l)2ICl(g)G=10.88kJ (b) H2(g)+I2(s)2HI(g)G=3.4kJ (c) CS2(g)+3Cl2(g)CCl4(g)+S2Cl2(g)G=39kJ (d) 2SO2(g)+O2(g)2SO3(g)G=141.82kJ (e) CS2(g)CS2(l)G=1.88kJarrow_forwardCalculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest whole-number coefficients.arrow_forwardCalculate E°, G°, and K at 25°C for the reaction 3Mn2+(aq)+2MnO4(aq)+2H2O5MnO2(s)+4H+(aq)arrow_forward
- Calculate E°, G°, and K at 25°C for the reaction 3MnO4(aq)+4H+(aq)+Cl2(g)2Mn2+(aq)+2ClO3(aq)+2H2Oarrow_forwardCalculate G for the following reactions and state whether each reaction is spontaneous under standard conditions at 298 K. (a) 2Na(s) + H2SO4() Na2SO4(s) + H2(g) (b) Cu(s) + H2SO4() CuSO4(s) + H2(g)arrow_forwardFor a redox reaction, when Ecell∘ > 0, then _____________ A) the reactants are less abundant than the products in the equilibrium mixture. B) the reaction is spontaneous under both standard and nonstandard conditions. C) K < 1 D) Δ?∘ΔG∘ > 0arrow_forward
- 5, Calculate ΔG° for the following reaction from the equilibrium constant at the temperature given. 2SO2 (g) + O2 (g) -> 2SO3 (g) T=300OC KP =48.2 Group of answer choices a, -18.5 kJ b, 5.34 kJ c, -5.34 kJ d, 18.5 kJarrow_forwardWith a ΔΔGo of -550.23 kJ, calculate the equilibrium constant for the reaction at 25.0 oC.arrow_forwardConsider the following reaction at 298K.Cr3+ (aq) + Cu+ (aq) Cr2+ (aq) + Cu2+ (aq) Which of the following statements are correct?Choose all that apply. n = 1 mol electrons The reaction is reactant-favored. Eocell > 0 ΔGo > 0 K > 1arrow_forward
- At 25oC, for the reaction 2 A(aq) ----> B(aq) + C(aq), the equilibrium constant is 1.89. If the concentration of B(aq) was 0.361 M and the concentration of C(aq) was 0.496 M, what would be the minimum concentration of A(aq) necessary in order (in mol/L) to make this reaction spontaneous under these conditions?arrow_forwardDetermine the equilibrium constant, Kp at 25˚C for the reaction below using the table(picture). 2NO2(g) + 7H2(g) ⇄ 2NH3(g) + 4H2O(g)arrow_forward10. For the reaction A(aq) + B(aq) <---> C(aq) + D(aq), the equilibrium constant is 20.3 at 25oC and 36.8 at 50oC. What is the value of the standard Gibbs free energy change (in kJ) of this reaction at 75oC?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY