For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.61 kJ at 25°C. The initial concentration of A(aq) is 0.566 M, the initial concentration of B(aq) is 0.367 M, and the initial concentration of C(aq) is 0.246 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25°C)?

For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.61 kJ at 25°C. The initial concentration of A(aq) is 0.566 M, the initial concentration of B(aq) is 0.367 M, and the initial concentration of C(aq) is 0.246 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25°C)?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.94QE: Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at...

See similar textbooks

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?
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?
a. Calculate the Gibbs Free Energy for the reaction shown below at T=25 oC. b. What is the value of the equilibrium constant K? Zn + Cu+2 --> Zn+2 + Cu ξ0 = +1.1V
I want all questions answered Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ . Calculate ionic strength of solution?Calculate (in volts) Standard Electrode Potential of the cell E°:?Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°?Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag)? Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG?
Calculate the equilibrium constant Kc for a reaction occurring at a temperature of 15 oC, and with a ΔGo of -45.3 kJ/mol. (Use R=8.314 J/mol⋅K and 273.00 for oC/K conversion)
For a standard voltaic cell comprised of a Zn2+|Zn electrode and a Fe2+|Fe electrode, what is the cell potential, in volts?
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
Question 1:For the reaction A(aq) ---> B(aq) the change in standard free enthalpy is 2.65 kJ at 25 oC and 4.92 kJ at 45 oC. Calculate the value of the equilibrium constant for this reaction at 75 oC.
What is the equilibrium constant for a reaction whose AG 165 kJ/mol at 262 K?
What is the ΔrG for the following reaction (in kJ mol-1) at 298 K? 3 O2 (g) ⇌ 2 O3 (g) The conditions for this reaction are: PO2 = 1.75 bar PO3 = 1.99 bar You will also need to use Appendix II in your textbook (containing standard Gibbs energies of formation). A copy of Appendix II has also been posted on eClass. Please use the method of Gibbs energy of formation to calculate ΔrG° if needed. Enter the value of "Q" for this reaction.
At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Teq=△H/△S Use the information given.
For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe3+|Fe2+electrode, what is the cell potential, in volts?