Question 2: For reaction 2 A(aq) <---> B(aq) + C(aq), the change in standard free enthalpy is 1.33 kJ at 25oC. The initial concentration of A is 0.572 M, the initial concentration of B is 0.347 M, and the initial concentration of C is 0.221 M. At equilibrium (still at 25oC), what will be the concentration of A(aq) (in mol/L)?

Question 2: For reaction 2 A(aq) <---> B(aq) + C(aq), the change in standard free enthalpy is 1.33 kJ at 25oC. The initial concentration of A is 0.572 M, the initial concentration of B is 0.347 M, and the initial concentration of C is 0.221 M. At equilibrium (still at 25oC), what will be the concentration of A(aq) (in mol/L)?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 73QAP: Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table...

See similar textbooks

Similar questions

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?
Estimate ΔrG° at 2000. K for each reaction in Question 60.
Consider the reaction below at 25°C: 2MnO4(aq)+16H+(aq)+10Br(aq)2Mn2+(aq)+5Br2(l)+8H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 2.00 with all other ionic species at 0.100 M? (c) Is the reaction spontaneous at a pH of 5.00 with all other ionic species at 0.100 M? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M?
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Consider the reaction low at 25°C: 3SO42(aq)+12H+(aq)+2Cr(s)3SO2(g)+2Cr3+(aq)+6H2O Use Table 17.1 to answer the following questions. Support your answers with calculations. (a) Is the reaction spontaneous at standard conditions? (b) Is the reaction spontaneous at a pH of 3.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (c) Is the reaction spontaneous at a pH of 8.00 with all other ionic species at 0.100 M and all gases at 1.00 atm? (d) At what pH is the reaction at equilibrium with all other ionic species at 0.100 M and all gases at 1.00 atm?
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?
For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 3.39 kJ at 25 oC and 5.43 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC. (I have already sent it once but the answer was 0.883 and its incorrect)
10. 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?
Metal corrosion by aqueous acid is a favorable process under many normal conditions and one of the many problems caused by acid rain. Use the following reaction and tabulated values to calculate ∆H and ∆S for the following reaction between metallic iron and free acid generated by species such as H2SO4. What is the overall favorability of the reaction (∆G) assuming STP? Fe (s) + 2H(aq)--> Fe(aq)+ H2(g) Species ∆Ηfo (kJ/mol) S (J/mol*K) Fe 0 27.28 H2 0 130.68 Fe2+ -89.1 -137.7 H+ 0 0
Calculate Kp at 298 K for this reaction2 NO2 (g) ⇌ N2O4 (g), Using ∆G values. What is the effect of decrease in pressure in the number of moles of NO2?What is the equilibrium constant at 500 K?What is the effect of adding Ar gas on the number of moles of NO2?At what temperature which the number of moles of NO2 and N2O4 are equal
The solubility product constant (Ksp) for the following reaction is 5.61x10-9. What is the Free Energy of this reaction in kJ at 298 K? BaCO3(s) ↔ Ba2+(aq) + CO32-(aq)
Given the following data:Fe2+ + 2e-→Fe Ered = -0.44 v, Ag+ + e- →Ag Ered = 0.80 v Answer the following questions with respect to the reaction;Fe2+(aq) + 2 Ag(s) → Fe(s) + 2 Ag+(aq) (a) what is E for the reaction?(b) is the reaction spontaneous at standard state conditions? (c) what is the value of E at equilibrium?(d) what is the value of equilibrium constant at 25○C ?(e) if [Fe2+]=0.100 M and [Ag+] = 0.0100 M , what is the magnitude of E at 25○C?