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CU PIULUOS LO UCCU 30. Based on the given standard free energy change and electron stoichiometry...
Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding...
Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding standard cell potential. AG°= -4.5 kJ/mol, n = 1, F = 96485 J/mol O El-0.047 V O Edel = -4.5V El=+0.047V
+ Calculate the change in the standard free energy for the following reaction: Zn + Cu?+...
+ Calculate the change in the standard free energy for the following reaction: Zn + Cu?+ Zn²+ (aq) + Cu (3) Standard Reduction Potentials (5) (aq) + 2e → = -0.763 V (aq) + 2e → Cu (s) Ered = 0.337 V (aq) → → Zn (5) Ered Zn2+ Cu2+ A. - 212 kJ/mol B. 175 kJ/mol C. 81.0 kJ /mol OD. - 106 kJ / mol
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0...
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Calculate the change in the standard free energy for the following reaction: Znc+Cu?" (aq) (a +...
Calculate the change in the standard free energy for the following reaction: Znc+Cu?" (aq) (a + Cu Zn? Standard Reduction Potentials (al +2e-Zn(s) E-0.763 V (a) +2e - Cu Ered -0.337 V O A. 175 kJ/mol OB. 81.0 kJ/mol OC - 212 kl/mol OD. - 106 kJ/mol QUESTION 34 The density of a 0.84 M aqueous sugar (C12H22011) solution is 1.12 g/mL at 25°C What is the molal concentration (molality)? The molar mass of C12H22011 - 342.3 g/mol. O A...
The free energy change for the following reaction at 25 °C, when Cu?) - 1.15 M...
The free energy change for the following reaction at 25 °C, when Cu?) - 1.15 M and Co2+) = 3.46x10-M, is -133 kJ: Cu2+(1.15 M) + Co(s) — Cu(s) + Co2+(3.46x10-3 M) AG --133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Please circle final answer Calculate the change in free energy (AG) for the following standard cell...
Please circle final answer
Calculate the change in free energy (AG) for the following standard cell between Barium and Copper. Recall AG = -nFEcell, and F = 9.65 x 10 C/mol Ba Ba2 (aq) + 2e, E red -2.90 V 2e+Cu2+ (aq) Cus), Ered = +0.337 V +625 kJ/mol +495 kJ/mol -625 kJ/mol 495 kJ/mol
21A. Calculate the standard free energy change, AGºat 298 K for the reaction 2COXg) + 2NO(g)...
21A. Calculate the standard free energy change, AGºat 298 K for the reaction 2COXg) + 2NO(g) -2CO(g) + N:(g) The standard free energy of formation for CO is - 137 kJ, for NO it is 87.6 kJ/mol and for CO, it is -394 kJ/mol. B. Calculate the free energy change. AG. at 298 K. given that the partial pressure of CO is 5.0 atm, that of NO is 4.0 atm, that of CO, is 3.0 atm & that of N,...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
Need help with the second part please Calculate the standard change in Gibbs free energy, AGan,...
Need help with the second part please
Calculate the standard change in Gibbs free energy, AGan, for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH CI(s) NH(aq) + CI (aq) kJ/mol -7.67 AGa Determine the concentration of NHt (aq) if the change in Gibbs free energy, AG. for the -9.61 kJ/mol. м INH 676 Enter numeric value
A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant...
A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant F = 96,500 J/mol, calculate the standard Gibb's free energy change AG in kJ (to three significant figures) for the reaction.
Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding standard cell potential. AG°= -4.5 kJ/mol, n = 1, F = 96485 J/mol O El-0.047 V O Edel = -4.5V El=+0.047V
+ Calculate the change in the standard free energy for the following reaction: Zn + Cu?+ Zn²+ (aq) + Cu (3) Standard Reduction Potentials (5) (aq) + 2e → = -0.763 V (aq) + 2e → Cu (s) Ered = 0.337 V (aq) → → Zn (5) Ered Zn2+ Cu2+ A. - 212 kJ/mol B. 175 kJ/mol C. 81.0 kJ /mol OD. - 106 kJ / mol
Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH,CI() = NH(aq) + Cl(aq) AGxn = -7.7 kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGrxn , for the reaction is –9.53 kJ/mol. [NH] = 0.72 Consider a general reaction enzyme A(aq) = B(aq) The AG® of the reaction is -4.880 kJ mol-....
Calculate the change in the standard free energy for the following reaction: Znc+Cu?" (aq) (a + Cu Zn? Standard Reduction Potentials (al +2e-Zn(s) E-0.763 V (a) +2e - Cu Ered -0.337 V O A. 175 kJ/mol OB. 81.0 kJ/mol OC - 212 kl/mol OD. - 106 kJ/mol QUESTION 34 The density of a 0.84 M aqueous sugar (C12H22011) solution is 1.12 g/mL at 25°C What is the molal concentration (molality)? The molar mass of C12H22011 - 342.3 g/mol. O A...
The free energy change for the following reaction at 25 °C, when Cu?) - 1.15 M and Co2+) = 3.46x10-M, is -133 kJ: Cu2+(1.15 M) + Co(s) — Cu(s) + Co2+(3.46x10-3 M) AG --133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Please circle final answer
Calculate the change in free energy (AG) for the following standard cell between Barium and Copper. Recall AG = -nFEcell, and F = 9.65 x 10 C/mol Ba Ba2 (aq) + 2e, E red -2.90 V 2e+Cu2+ (aq) Cus), Ered = +0.337 V +625 kJ/mol +495 kJ/mol -625 kJ/mol 495 kJ/mol
21A. Calculate the standard free energy change, AGºat 298 K for the reaction 2COXg) + 2NO(g) -2CO(g) + N:(g) The standard free energy of formation for CO is - 137 kJ, for NO it is 87.6 kJ/mol and for CO, it is -394 kJ/mol. B. Calculate the free energy change. AG. at 298 K. given that the partial pressure of CO is 5.0 atm, that of NO is 4.0 atm, that of CO, is 3.0 atm & that of N,...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
Need help with the second part please
Calculate the standard change in Gibbs free energy, AGan, for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH CI(s) NH(aq) + CI (aq) kJ/mol -7.67 AGa Determine the concentration of NHt (aq) if the change in Gibbs free energy, AG. for the -9.61 kJ/mol. м INH 676 Enter numeric value
A two electron redox reaction has a redox potential E' = 0.58 V. Given Faraday's constant F = 96,500 J/mol, calculate the standard Gibb's free energy change AG in kJ (to three significant figures) for the reaction.
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