6-Consider the first ionization of sulfurous acid: H2SO;(aq) → H* (aq) + HSO; (ag) Certain related thermodynamic data are provided below: H2SO3(aq) H*(aq) HSO; (aq) Hf kcal/mole -145.5 -151.9 S° cal/mole K 56 26 (a) Calculate the value of AG° at 25°C for the ionization reaction. (b) Calculate the value of K at 25°C for the ionization reaction. (c) Account for the signs of AS° and AH° for the ionization reaction in terms of the molecules and ions present.

6-Consider the first ionization of sulfurous acid: H2SO;(aq) → H* (aq) + HSO; (ag) Certain related thermodynamic data are provided below: H2SO3(aq) H*(aq) HSO; (aq) Hf kcal/mole -145.5 -151.9 S° cal/mole K 56 26 (a) Calculate the value of AG° at 25°C for the ionization reaction. (b) Calculate the value of K at 25°C for the ionization reaction. (c) Account for the signs of AS° and AH° for the ionization reaction in terms of the molecules and ions present.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The value of Ka for nitrous acid (HNO2) at 25 ∘C is 4.5×10-4 △G°=19.1kJ What is the value of △G at equilibirum?
What is ∆G0 for the reaction CN- + H2O = HCN + OH-? Ka for HCN = 4.0x10-10. R = 8.314 J/(mol*K)
The Ka of HCHO2 is 1.8 x 10-4. Calculate the ΔGº (in kJ/mol) for the acid dissociation reaction at 25ºC
Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2 (aq) --><-- C2H3O2- (aq) + H+ (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2] = 0.0990 M, [C2H3O2-] = 1.33 × 10-3 M and [H+] = 1.33 × 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is ________.
Given that the Ka for HOCl is 3.5  10-8, calculate the K value for the reaction of HOClwith OH- at 25oC.
Write the expression Kc for the following reactions. (a) Fe2+(aq) + Ce4+(aq) ⇋ Fe3+(aq) + Ce3+(aq) (b) CaCO3(s) ⇋ CaO(s) + CO3(g)
at 25oC, Ka for aspirin (C9H8O4) is 3.0 x 10-4. Calculate Δ Go (kJ/mol) for the reaction: C9H8O4(aq) + H2O(l) = H3O+(aq) + C9H7O4-(aq)
If the equilibrium constant for a reaction A + B <=> 2C is measured as Keq = 1.318. What would the value be for the same reaction if written as 2C <=> A + B. Keq' = ____. 3 sig. fig.
What is the quilibrium constant for a reaction at 25oC. The value of Delta G is -56.8 kJ/mol?
At 25oC, the ΔH o andΔH o for the following reaction is -24.7 kJ/mol and -49.9 J/mol-K, respectively. H2S (aq) + CN- (aq) ⇋ HS- (aq) + HCN (aq) If you mix 100 mL of 0.0450 M NaCN with 100 mL of 0.0450 M H2S, the reaction will proceed as indicated in the equation and will reach an equilibrium in the end. What will be the molar concentration of HCN at equilibrium?
Consider the following aqueous chemical equilibrium of benzoic acid, a weak acid: C6H5COOH(aq) + H2O(l) is in equilibrium with H3O+(aq) + C6H5COO-(aq) a. The addition of H3O+(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COO-(aq) in the system? b. Addition of OH-(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COOH(aq) in the system? c. Removal of C6H5COO-(aq) from the chemical equilibrium will have what effect on the amount of (moles) H3O+(aq) in the system? d. Increasing the pH of the solution will have what effect on the amount (moles) of C6H5COOH(aq) in the system?
If the equilibrium constant for the reaction A+ B ⇌ C is reported as 0.432, what would be the equilibrium constant for the reaction written as C ⇌ A+ B?