3) Consider the cell Pt|H2(g)| HCl(aq)|AgCI(s) |Ag, for which the cell reaction is 2 AgCI(s) + H2(g) → 2 Ag(s) + 2 HCl(aq). At 25 °C and a molality of HCl of 0.020 mol kg-1, Ecell = +0.4658 V. (i) Write the Nernst equation for the cell reaction. (ii) Calculate A,G for the cell reaction. (iii) Assuming that the Debye-Hückel limiting law holds at this concentration, calculate E°(CI", AgCI, Ag).

3) Consider the cell Pt|H2(g)| HCl(aq)|AgCI(s) |Ag, for which the cell reaction is 2 AgCI(s) + H2(g) → 2 Ag(s) + 2 HCl(aq). At 25 °C and a molality of HCl of 0.020 mol kg-1, Ecell = +0.4658 V. (i) Write the Nernst equation for the cell reaction. (ii) Calculate A,G for the cell reaction. (iii) Assuming that the Debye-Hückel limiting law holds at this concentration, calculate E°(CI", AgCI, Ag).

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

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Consider the cell Pt|H,(g) HCI(aq)|AgCl(s)JAg, for which the cell reaction is 2 AgCl(s) + H,(g) and a molality of HCI of 0.020 mol kg', Ecell = +0.4658 V. (i) Write the Nernst equation for the cell reaction. (ii) Calculate A,G for the cell reaction. (iii) → 2 Ag(s) + 2 HCI(aq). At 25 °C Assuming that the Debye-Hückel limiting law holds at this concentration, calculate E'(CI, AgCl, Ag).
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
Consider the cell Pt(s)|H2(g,p°)|HCl(aq)|AgCl(s)|Ag(s), for which the cell reaction is 2 AgCl(s) + H2(g) ------->. 2 Ag (s) + 2 HCl. (aq). At 25 °C and a molality of HCl of 0.010 mol/kg, Ecell = +0.4658 V. a. Write the Nernst equation for the cell reaction. b. Calculate ΔGr for the cell reaction.
One ecologically important equilibrium is that between carbonate and hydrogencarbonate (bicarbonate) ions in natural water. (a) The standard Gibbs energies of formation of CO32−(aq) and HCO3−(aq) are −527.81 kJ mol−1 and −586.77 kJ mol−1, respectively. What is the standard potential of the HCO3−/CO32−,H2 couple? (b) Calculate the standard potential of a cell in which the cell reaction is Na2CO3(aq) + H2O(l) → NaHCO3(aq) + NaOH(aq). (c) Write the Nernst equation for the cell, and (d) predict and calculate the change in cell potential when the pH is changed to 7.0 at 298 K.
Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg−1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s) + Zn(s) → 2 Hg(l) + 2 Cl−(aq) + Zn2+(aq). The cell potential is +1.2272 V, E⦵(Zn2+,Zn) = −0.7628 V, and E⦵(Hg2Cl2,Hg) = +0.2676 V. (a) Write the Nernst equation for the cell. Determine (b) the standard cell potential, (c) ΔrG, ΔrG⦵, and K for the cell reaction, (d) the mean ionic activity and activity coefficient of ZnCl2 from the measured cell potential, and (e) the mean ionic activity coefficient of ZnCl2 from the Debye–Hückel limiting law. (f) Given that (∂Ecell/∂T)p = −4.52 × 10−4 V K−1, Calculate ΔrS and ΔrH.
Consider the cell, Zn(s)|ZnCl2(0.0050 mol kgHg2Cl2(s)|Hg(I), for which the cell reaction is Hg2Cl2(s) + Zn(s) → 2Hg(1) + 2C1(aq) + Zn2+(aq). The cell potential is +1.2272 v, Ee(Zn²*,Zn) -0.7628 V, and Ee(Hg2Cl2,Hg) = +0.2676 V. (a) Write the Nernst equation for the cell. Determine (b) the standard cell potential, (c) A,G, A,GE, and K for the cell reaction
13.38 For the cell at 25°C and 1 bar Pt|Ag|AGCI(s)|HCI(aq)|Hg,Cl,(s)|Hg|Pt' (a) write the cell reaction; (b) use Table 13.1 to find the emf if the HCl molality is 0.100 mol/kg; (c) find the emf if the HCl mo- lality is 1.00 mol/kg. (d) For this cell, (8E/aT)p = 0.338 mV/K at 25°C and 1 bar. Find AG°, AH°, and ASº for the cell reaction at 25°C.
(a) Calculate the standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s) and the standard Gibbs energy and enthalpy of the cell reaction at 25 °C. (b) Estimate the value of ΔrGΘ at 35 °C.
Calculate the biological standard Gibbs energies of reactions of the following reactions and half-reactions:(a) 2 NADH(aq) + O2(g) + 2 H+(aq) → 2 NAD+(aq) + 2 H2O(I) E⊕=+1.14 V(b) Malate(aq) + NAD+(aq) → oxaloacetate(aq) + NADH(aq) + H+(aq) E⊕=-0.154 V(c) O2(g) + 4H+(aq) + 4 e- → 2 H2O(I) E⊕ = +0.81 V
Calculate the standard Gibbs energies at 25 °C of the following reactions from the standard potential data.(a) Ca(s) + 2 H2O(I) → Ca(OH)2(aq) + H2(g)(b) 2 Ca(s) + 4 H2O(I) → 2 Ca(OH)2(aq) + 2H2(g)(c) Fe(s) + 2 H2O(I) → Fe(OH)2(aq) + H2(g)(d) Na2S2O8(aq) + 2 Nal(aq) → 12(s) + 2 Na2SO4(aq)(e) Na2S2O8(aq) + 2 Kl(aq) → l2(s) + Na2SO4(aq) + K2SO4(aq)(f) Pb(s) + Na2CO3(aq) → PbCO3(aq) + 2 Na(s)
Consider the cell:Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Agfor 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 a) Calculate ionic strength of solution?b) Calculate mean activity coefficient Ɣ∓? c) Calculate (in volts) Standard Electrode Potential of the cell E°:. d) Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°:. e) Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag):. f) Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG:
The standard reaction Gibbs energy for the reactionH2(g) + (1)/(2)O2(g) → H2O(I) is -237.13 kJ mol-1 at 25 °c. Determine the equilibrium constant in terms of concentration, Kc, at this temperature.