Hydrofluoric acid,
(a) Using the
(b) Calculate the acid dissociation constant,
Want to see the full answer?
Check out a sample textbook solutionChapter 8 Solutions
Student Solutions Manual for Ball's Physical Chemistry, 2nd
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardConsider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25Carrow_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_forwarda) For the reaction given in Part A, how much heat is absorbed when 2.70 mol of AA reacts? (the image attached) b) For the reaction given in Part A, ΔS∘rxn is 39.0 J/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxn?arrow_forwardAssuming that neither standard enthalpy changes of formations (∆Hof) nor standard molar entropies (So) depend upon temperature, estimate using the Table of Thermodynamic Data : (a) the standard Gibbs free energy change for the reaction that forms rhombic sulfur at 600 K, and (b) the temperature (in oC) at which reaction will stop formation of products: 2H2S(g) + SO2(g) → 3S(rhombic, s) + 2H2O(g) Round off your answers to the nearest integer. Report the temperature in oC. and enter them with correct units: (a)∆Gorxn = (b) T =arrow_forward
- Consider the reactions in the table. (a) Write the equilibrium constant in terms of activities for the chemical reaction of fire extinguishers: 2NaHCO3 (s) ↔ Na2CO3 (s) + CO2 (g) + H2O (g) ΔrH = 135.54 KJ (b) At 300 K the equilibrium constant is 3.95x10-6 for the reaction in (a), what is ΔrGo? (c) State in words: what happens to the equilibrium when temperature is increased? Then, verify by finding K for the reaction in (a) at 420 K.arrow_forwardCalculate the equilibrium constant for the following reaction at 25o C, given that change in standard Gibbs free energy (f) of O3 (g) is 163.4 kJ/mol. 2O3(g) -> 3O2(g)arrow_forwardA 1.000 M solution of A was heated at 74.1 ° C for several hours. What is the concentration of B when Δ G = − 3.98 k J ?arrow_forward
- Consider the reaction: CaCO3(s) ↔ CaO(s) + CO2(g) The reaction enthalpy and entropy are: ΔHo rx = -117.1 kJ∙mol-1; ΔSo rx = -362 J∙K-1mol-1. Assume that these values are independent of temperature. Calculate the equilibrium constant for this reaction at 25.0⁰ Carrow_forwardThe evaporation of one mole of water at 298 K has a standard free energy change of 8.58 kJ.H2O(l) ⇌ H2O(g) ΔG°298 = 8.58 kJ(a) Is the evaporation of water under standard thermodynamic conditions spontaneous?(b) Determine the equilibrium constant, KP, for this physical process.(c) By calculating ΔG, determine if the evaporation of water at 298 K is spontaneous when the partial pressure of water, PH2 O, is 0.011 atm.(d) If the evaporation of water were always nonspontaneous at room temperature, wet laundry would never dry when placed outside. In order for laundry to dry, what must be the value of PH2 O in the air?arrow_forwardWith a ΔΔGo of -550.23 kJ, calculate the equilibrium constant for the reaction at 25.0 oC.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning