Calculate the cell potential (Ecell) and Gibbs Free Energy (Delta G) for the reaction (2Ag+ (aq)...
Calculate the cell potential (Ecell) and Gibbs Free Energy (Delta G) for the reaction (2Ag+ (aq) + Fe (s) -> Fe2+ (aq) + 2Ag (s) ) under these conditions: a 250mL beaker of 1.0mol Fe metal electrode and 0.10 moles of Fe 2+; and a second 250mL beaker of 2.0 moles Ag metal electrode ad 0.50 moles of Ag+. E naught of the cell= 1.21 V.
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Calculate the cell potential (Ecell) and Gibbs Free Energy
(Delta G) for the reaction (2Ag+ (aq)...
A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + N12+(aq) a) calculate the...
A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + N12+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode?
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a)...
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode? a) 1.03 V; b) nickel a) 1.03 V; b) silver oooo a) 0.57 V; b) nickel a) 0.57V; b) silver
14. Determine the standard cell potential and the cell potential under the stated conditions for the...
14. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at 298.15 K. a) Hg(l) + S2-(ag, 0.10 M) + 2Ag+(ag, 0.25 M) → 2Ag(s) + HgS(s) \ (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half-cell consisting of a nickel electrode in 0.25 M...
7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) Fe2+(aq) (1.1...
7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) Fe2+(aq) (1.1 M) || Cu2+ (aq) (0.50 M) Cu(s) Ecell = Eºcell - 0.0592/n logQ
The free energy change for the following reaction at 25 °C, when [Fe2+1 - 6.16*10' M...
The free energy change for the following reaction at 25 °C, when [Fe2+1 - 6.16*10' M and (Ag - 1.19 M, is 252 kJ: Fe2+(6.16*109 M) + 2Ag(s) >Fe(s) + 2Ag*(1.19 M) AG = 252 kJ What is the cell potential for the reaction as written under these conditions? Would this reaction be spontaneous in the forward or the reverse direction? We were unable to transcribe this imageThe free energy change for the following reaction at 25 °C, when [Pb2+]...
Calculate the standard cell potential for the following reaction: Co ()| Co2+ (aq) || 2Ag+ (aq)...
Calculate the standard cell potential for the following reaction: Co ()| Co2+ (aq) || 2Ag+ (aq) | 2Ag (). Standard Reduction Potentials Co2+ (aq) Ered = -0.277 V Ag+ (aq) + 6 → Ered = 0.799 V + 2e → Co (8) → Ag (3) A. 1.32 V B. 1.88 V C. 0.522 V D. 1.08 V
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to...
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K....
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K. AG MPEO 7. Ag (aq) + Mg(s) S Ag(s)+ Mg2 (aq) (a)
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State wheth...
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + N12+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode?
Question 4 A galvanic cell uses the reaction: 2Ag+(aq) + Ni(s) --> 2Ag(s) + Ni2+(aq) a) calculate the Standard Cell Potential (Ecell) of this galvanic cell and b) which metal is the cathode? a) 1.03 V; b) nickel a) 1.03 V; b) silver oooo a) 0.57 V; b) nickel a) 0.57V; b) silver
14. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaneous under each set of conditions at 298.15 K. a) Hg(l) + S2-(ag, 0.10 M) + 2Ag+(ag, 0.25 M) → 2Ag(s) + HgS(s) \ (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half-cell consisting of a nickel electrode in 0.25 M...
7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) Fe2+(aq) (1.1 M) || Cu2+ (aq) (0.50 M) Cu(s) Ecell = Eºcell - 0.0592/n logQ
The free energy change for the following reaction at 25 °C, when [Fe2+1 - 6.16*10' M and (Ag - 1.19 M, is 252 kJ: Fe2+(6.16*109 M) + 2Ag(s) >Fe(s) + 2Ag*(1.19 M) AG = 252 kJ What is the cell potential for the reaction as written under these conditions? Would this reaction be spontaneous in the forward or the reverse direction? We were unable to transcribe this imageThe free energy change for the following reaction at 25 °C, when [Pb2+]...
Calculate the standard cell potential for the following reaction: Co ()| Co2+ (aq) || 2Ag+ (aq) | 2Ag (). Standard Reduction Potentials Co2+ (aq) Ered = -0.277 V Ag+ (aq) + 6 → Ered = 0.799 V + 2e → Co (8) → Ag (3) A. 1.32 V B. 1.88 V C. 0.522 V D. 1.08 V
Standard free energy change (Delta degree G) and cell potential (E degree) can be said to measure the same thing and are convertible by the equation: Delta G degree = nF E degree _cell where n is the total number of moles of electrons being transferred, and F is Faraday constant 9.6- 1853415 times 10^C/mol. The free energy (Delta G degree) of a spontaneous reaction is always negative. For each of the electrochemical cells below, calculate the free energy of...
Calculate the Gibbs energy change from the standard cell potential following redox reactions at 350 K. AG MPEO 7. Ag (aq) + Mg(s) S Ag(s)+ Mg2 (aq) (a)
26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State whether each is spontaneous or nonspontaneous under the set of conditions at 298.15 K. Hg(l) + s (aq, 0.10 M) + 2Ag (aq, 0.25 M) - 2Ag(s) + HgS(s) E°= -0.70 V E°= 0.7996 V HgS(s) +2e → Hg(1) +S?(aq) Agt (aq) + e +Ag(s) A.Ecell = 1.43 V, spontaneous B. Ecel = 1.50 V, spontaneous C. Ecell = 0.0996 V, spontaneous on TT 1...
Free-energy change, AGº, is related to cell potential, Eº, by the equation AG° = -nFE° where n is the number of moles of electrons transferred and F = 96,500 C/(mol e ) is the Faraday constant. When Eº is measured in volts, AGⓇ must be in joules since 1 J =1C.V. Part A Calculate the standard free-energy change at 25°C for the following reaction: Mg(s) + Fe2+ (aq)Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include...
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