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26. Determine the cell potential under the stated conditions for the electrochemical reaction described. State wheth...
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...
Based on the reduction potentials provided below, calculate the the cell potential at 25°C under the...
Based on the reduction potentials provided below, calculate the the cell potential at 25°C under the stated conditions: Hg() + 92-aq, 0.10M) + 2Ag+(aq, 0.25M)+ 2Ag(s) + HgS(s). Upload your work HgS(s) + 2e- + Hg() + S2-aq) E' = -0.70V Ag+ (aq) +- Ag(s) E = 0.7996V
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) +...
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag concentration is 2.68x10-4 M and the Art concentration is 1.06 M ? 3Ag" (aq) + Al(s) +3Ag(s) + Ap+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: Submit Answer Retry Entire Group 4 more group attempts remaining What is the calculated value of the cell potential at 298K for an electrochemical cell...
0 What is the Ecell for the cell represented by the combination of the following 4)...
0 What is the Ecell for the cell represented by the combination of the following 4) half-reactions? 2Hg2+(aq) + 2e-→Hg22+(aq) Cr3t(ag)+3eCr(s) E-0.92 V B) 1.28 V 9) 0.18 V A) 2.12 V D) 1.66 V E)-0.18 V 5) Examine the following half-reactions and select the weakest oxidizing agent among the 5)_ species listed. E。= 0.854 V E1.185 V K+(aq) + e-→ K(s) F20(aq) + 2H+(aq) + 4e-→ 2p-(aq) + H20() E。= 2.153 V A) F2o(ag) B) AuBr4Taq) C) Mn2+(ag) D)...
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Agt concentration is 1.13 M and the Mn2+ concentration is 3.22x10-M? 2Ag+ (aq) + Mn(s) — 2Ag() + Mn2(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Agt concentration is 8.96x10-4 M and the Zn2+ concentration is 1.05 M ? 2Ag+(aq) + Zn(s)—>2Ag(s) + Zn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: __ What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 1.94x10-4 atm,...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2+ (0.15 M) Fe2+ (0.0039 M) Fe(s) E =-0.440 V E+Cu = 0.339 V Fe2+/Fe Is the electrochemical cell spontaneous or not spontaneous -0.779 Ecell = as written at 25 C? not spontaneous spontaneous о Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 'C Pt(s) Sn2 (0.0024 M), Sn4+ (0.12 M) |...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Cu(s) Cu2+(0.14 M) | Fe2+(0.0044 M) Fe(s) Ecu?+Icu = 0.339 V Efez lfe = -0.440 V Ecell = v Is the electrochemical cell spontaneous or not spontaneous as written at 25 °C? O not spontaneous O spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2+(0.0048 M), Snº+(0.11 M) || Fe3+(0.12...
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...
Based on the reduction potentials provided below, calculate the the cell potential at 25°C under the stated conditions: Hg() + 92-aq, 0.10M) + 2Ag+(aq, 0.25M)+ 2Ag(s) + HgS(s). Upload your work HgS(s) + 2e- + Hg() + S2-aq) E' = -0.70V Ag+ (aq) +- Ag(s) E = 0.7996V
Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag(s) where [Ag+] = 0.00350 M and [Cu2+] = 7.00x10-4 M. The standard reduction potentials are shown below: Ag+(aq) +e → Ag(s) E° = 0.7996 V Cu2+ (aq) + 2e -→ Cu(s) E° = 0.3419 V 2nd attempt Ecell = V
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag concentration is 2.68x10-4 M and the Art concentration is 1.06 M ? 3Ag" (aq) + Al(s) +3Ag(s) + Ap+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: Submit Answer Retry Entire Group 4 more group attempts remaining What is the calculated value of the cell potential at 298K for an electrochemical cell...
0 What is the Ecell for the cell represented by the combination of the following 4) half-reactions? 2Hg2+(aq) + 2e-→Hg22+(aq) Cr3t(ag)+3eCr(s) E-0.92 V B) 1.28 V 9) 0.18 V A) 2.12 V D) 1.66 V E)-0.18 V 5) Examine the following half-reactions and select the weakest oxidizing agent among the 5)_ species listed. E。= 0.854 V E1.185 V K+(aq) + e-→ K(s) F20(aq) + 2H+(aq) + 4e-→ 2p-(aq) + H20() E。= 2.153 V A) F2o(ag) B) AuBr4Taq) C) Mn2+(ag) D)...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Agt concentration is 1.13 M and the Mn2+ concentration is 3.22x10-M? 2Ag+ (aq) + Mn(s) — 2Ag() + Mn2(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Agt concentration is 8.96x10-4 M and the Zn2+ concentration is 1.05 M ? 2Ag+(aq) + Zn(s)—>2Ag(s) + Zn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given: __ What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 1.94x10-4 atm,...
38. The following redox half reactions are combined in a voltaic cell. Which reaction occurs at the cathode and what is the Eceu? Fe2+(aq) + 2e → Fe(s) E°=-0.44 V Cu²+(aq) + 2e → Cu(s) E°= 0.34 V a) b) c) d) Cu2+(aq) + 2e → Cu(s), Ecell = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecel = 0.78 V Fe2+(aq) + 2e → Fe(s), Ecell =-0.10 V Cu²+(aq) + 2e → Cu(s), Ecel = 0.10 V Cu²+ (aq) +...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C Cu(s) Cu2+ (0.15 M) Fe2+ (0.0039 M) Fe(s) E =-0.440 V E+Cu = 0.339 V Fe2+/Fe Is the electrochemical cell spontaneous or not spontaneous -0.779 Ecell = as written at 25 C? not spontaneous spontaneous о Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 'C Pt(s) Sn2 (0.0024 M), Sn4+ (0.12 M) |...
Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Cu(s) Cu2+(0.14 M) | Fe2+(0.0044 M) Fe(s) Ecu?+Icu = 0.339 V Efez lfe = -0.440 V Ecell = v Is the electrochemical cell spontaneous or not spontaneous as written at 25 °C? O not spontaneous O spontaneous Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at 25 °C. Pt(s) Sn2+(0.0048 M), Snº+(0.11 M) || Fe3+(0.12...
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