Gibbs energy change, A;G", is related to cell potential, E, by theCalculate the standard Gibbs energy change at 25 °C for the following reaction:equationA:G = -nFEMg(s) + Fe?+(ag)→Mg²+(ag) + Fe(s)Express your answer to three significant figures and include the appropriate units.where n is the number of moles of electrons transferred andF = 96 500 C mol-1 is the Faraday's constant.• View Available Hint(s)kJmol- 1A,G" = 370.56SubmitPrevious AnswersPart BCalculate the standard cell potential at 25 °C for the reactionX(s) + 2Y*(ag)→X²+(ag) + 2Y(s)where A,H° = -729 kJ mol-1 and ArS" = -325 JK' mol1Express your answer to three significant figures and include the appropriate units.• View Available Hint(s)E =ValueUnits

For the given cell, change in enthalpy and entropy at 25oC is as follows: ∆rHo = -729 kJ mol-1∆rSo =…

Gibbs energy change, A:G®, is related to cell potential, E, by the equation Calculate the standard Gibbs energy change at 25 °C for the following reaction: A;G° = -nFE Mg(s) + Fe2+(aq)→Mg²+(aq) +Fe(s) Express your answer to three significant figures and include the appropriate units. where n is the number of moles of electrons transferred and F = 96 500 C mol- is the Faraday's constant. > View Available Hint(s) HẢ ? A,G" = 370.56 kJmol-1 Submit Previous Answers Part B Calculate the standard cell potential at 25 °C for the reaction X(s) +2Y*(aq)¬→X²*(aq) +2Y(s) where ArH° = -729 kJ mol- and A,S° = -325 JK' mo]1 Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) Eo = Value Units

Gibbs energy change, A:G®, is related to cell potential, E, by the equation Calculate the standard Gibbs energy change at 25 °C for the following reaction: A;G° = -nFE Mg(s) + Fe2+(aq)→Mg²+(aq) +Fe(s) Express your answer to three significant figures and include the appropriate units. where n is the number of moles of electrons transferred and F = 96 500 C mol- is the Faraday's constant. > View Available Hint(s) HẢ ? A,G" = 370.56 kJmol-1 Submit Previous Answers Part B Calculate the standard cell potential at 25 °C for the reaction X(s) +2Y(aq)¬→X²(aq) +2Y(s) where ArH° = -729 kJ mol- and A,S° = -325 JK' mo]1 Express your answer to three significant figures and include the appropriate units. > View Available Hint(s) Eo = Value Units

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

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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).
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+
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
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.
The standard cell potential of a Daniell cell, with cell reactionZn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), is 1.10 V at 25 °C.Calculate the corresponding standard reaction Gibbs energy.
Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
The standard potential of the AgCl/Ag,Cl− couple fits the expressionE⦵/V = 0.23659 − 4.8564 × 10−4(θ/°C) − 3.4205 × 10−6(θ/°C)2 + 5.869 × 10−9(θ/°C)3Calculate the standard Gibbs energy and enthalpy of formation of Cl−(aq) and its standard entropy at 298 K.
Adenosine triphosphate, ATP, is used to store energy within biological systems. It releases that energy by losing a terminal phosphate group, Pi, to form adenosine diphosphate, ADP, through the hydrolysis reaction ATP(aq) + H2O(I) → ADP(aq) + Pi(aq) + H+(aq) . The standard reaction Gibbs energy, ΔrGΘ, for the hydrolysis of ATP to ADP is+ 10 kJ mol-1 at 298 K.This assumes that the concentration of hydrogen ions is 1 mol dm-3 . (a) In biochemistry, it is common practice to assume an alternative , and more realistic, standard state for which pH = 7. What is the corresponding standard reaction Gibbs energy, denoted ΔrGΘ, for this biological standardstate? (b) What is the Gibbs energy of reaction in an environment at 37 °C and pH = 7 in which the ATP. ADP. and P; concentrations are all (i) 1.0 mmol dm-3, (ii) 1.0 μmol dm-3 ?
By how much does the cell potential change when Q is increased by a factor of 5 for a reaction in which ν = 3 at 298 K?
From the biological standard half-cell potentialsE⊕(O2,H+,H2O) = +0.82 V and E⊕(NADH+,H+,NADH) = -0.32 V, calculate the standard potential arising from the reaction in which NADH is oxidized to NAD+ and the corresponding biological standard reaction Gibbs energy.
What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous? what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean? If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system