Consider the cellPt | H2(g,P°) | HCI(aq) | AgCl(s) | Agfor which the cell reaction is 2 AgCl(s) + H2(g) → 2Ag(s) + 2 HCI(aq).Assuming that the Debye-Hückel limiting law holdsat this concentration, calculate Ecell (CI, AgCI, Ag) at25°C and a molarity of HCl of 0.010 mol/L.

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Answered: Pt | H2(g,P°) | HCI(aq) | AgCl(s) | Ag…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 62QAP: Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the...

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Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Consider 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 25C
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).
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.
The electromotive force of the cell Pb(s) PbSO4(s) Na2SO4.10H₂O(aq)|Hg2SO4(s) Hg() is 0.9647 V at 25 °C. The temperature coefficient is 1.74 x 10-4 V K-¹. What is the AH for the reaction in kJ mol-¹? Express your answer in four significant figures.
Chemistry 1. (a) Balance the following simple redox reaction. Fe (s) + O₂(g) + 2H₂O (1) Fe³+ + 4 OH (b) If the standard change in the Gibbs energy of the molar reaction in part (a) is -507.13 kJ. Calculate the cell potential of the reaction.
Consider the cell Zn(s)|ZnCl2(0.005 mol kg-1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s)+Zn(s)->2Hg(l)+2Cl-(aq)+Zn2+(aq). The cell potential is 1.2272 V, E0(Zn2+,Zn)=-0.7628V, and E0(Hg2Cl2,Hg)=+0.2676V. Calculate the ∆ r G 0 , ∆ r G and K e q . Question 7 options: A. -202.23 kJ.mol-1; 222.85 kJ.mol-1; 6.21x1032 B. -198.84 kJ.mol-1; 236.81 kJ.mol-1; 7.11x1034 C. -182.23 kJ.mol-1; 256.22 kJ.mol-1; 5.66x1033 D. -190.34 kJ.mol-1; 232.42 kJ.mol-1; 6.62x1031
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.
The standard potential of the cell Bi(s)|Bi2S3(s)|Bi2S3(aq)|Bi(s) is +0.96 V at 25 °C. Calculate the equilibrium constant for the dissolution of Bi2S3(s).
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)

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Pt | H2(g,P°) | HCI(aq) | AgCl(s) | Ag for which the cell reaction is 2 AgCI(s) + H2(g) → 2 Ag(s) + 2 HCI(aq). Assuming that the Debye-Hückel limiting law holds at this concentration, calculate Ecell (CI¯, AgCI, Ag) at 25°C and a molarity of HCI of 0.010 mol/L.