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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...
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...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s)...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s)...
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s) Fe2+(aq) Pt2+(aq) + Fe(s) Fe2+0.0050 M Pt2+10.035 M The cell is E = V not spontaneous O spontaneous. Cu(s)2 Ag(aq) Cu2t(aq) + 2 Ag(s) [Cu2+0.015 M [Ag 0.015 M The cell is E = V O spontaneous. O not spontaneous Co2+(aq)Ti3(aq)Co3t(aq) +...
5. (20pts) Consider the reaction between oxalate ion and permanganate ion in acidic solution: MnO4 (aq)...
5. (20pts) Consider the reaction between oxalate ion and permanganate ion in acidic solution: MnO4 (aq) + C202-(aq) → Mn2+ (aq) + CO2(9) a. Balance the reaction in acidic solution b. Determine the standard cell potential of the representative voltaic cell c. Determine the standard free energy change of this reaction d. Determine the cell potential if the pH = 4 and all other solute concentrations were standard.
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using...
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using the following standard reduction potentials. Ag+(aq) + e- → Ag(s) E° = 0.80 V Ca2+(aq) + 2e + Ca(s) E° = -2.87 V 2.07 V -3.67 V 3.67 V -2.29 V -2.07 V
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V...
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V Cult(aq) + e + Cu(s) E° = 0.521 v Determine the half-cell reactions and the overall cell reaction, calculate the cell potential, and determine the equilibrium constant at 298.5 K for the cell: Pt (8)| H2(g)| H+(aq, ah+ = 0.25)||Cu²+( aq, acu2+ = 0.10) Cu(s) Is the cell reaction spontaneous as written?
And a copper electrode with 0.500 M Cu?' as the second half cell Cu2+ (aq) +...
And a copper electrode with 0.500 M Cu?' as the second half cell Cu2+ (aq) + 2 e Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0905 V. Write the balanced equation for the overall reaction in acidic solution. AgCl(s) + Cu2+ (aq) + 3 e → Ag(s) + Cu(s) + CI+ (aq) 04- 03. 02. + 2 O 4+ 1 2 3 4 5 6...
Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentr...
Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E ). Pt(s) + Fe2+ (aq) = P22+ (aq) + Fe(s) [Fe2+] = 0.0017 M [P12+] = 0.040 M The cell is O spontaneous. O not spontaneous Cu(s) + 2 Ag+ (aq) = Cu2+(aq) + 2 Ag(s) [Cu2+] =...
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...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s) Fe2+(aq) Pt2+(aq) + Fe(s) Fe2+0.0050 M Pt2+10.035 M The cell is E = V not spontaneous O spontaneous. Cu(s)2 Ag(aq) Cu2t(aq) + 2 Ag(s) [Cu2+0.015 M [Ag 0.015 M The cell is E = V O spontaneous. O not spontaneous Co2+(aq)Ti3(aq)Co3t(aq) +...
5. (20pts) Consider the reaction between oxalate ion and permanganate ion in acidic solution: MnO4 (aq) + C202-(aq) → Mn2+ (aq) + CO2(9) a. Balance the reaction in acidic solution b. Determine the standard cell potential of the representative voltaic cell c. Determine the standard free energy change of this reaction d. Determine the cell potential if the pH = 4 and all other solute concentrations were standard.
Calculate the value of Eºcell for the reaction 2Ag(s) + Ca2+(aq) + 2Ag+(aq) + Ca(s), using the following standard reduction potentials. Ag+(aq) + e- → Ag(s) E° = 0.80 V Ca2+(aq) + 2e + Ca(s) E° = -2.87 V 2.07 V -3.67 V 3.67 V -2.29 V -2.07 V
You are given the following half-cell reactions: Cu²+(aq) + e + Cult(aq) E° = 0.153 V Cult(aq) + e + Cu(s) E° = 0.521 v Determine the half-cell reactions and the overall cell reaction, calculate the cell potential, and determine the equilibrium constant at 298.5 K for the cell: Pt (8)| H2(g)| H+(aq, ah+ = 0.25)||Cu²+( aq, acu2+ = 0.10) Cu(s) Is the cell reaction spontaneous as written?
And a copper electrode with 0.500 M Cu?' as the second half cell Cu2+ (aq) + 2 e Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0905 V. Write the balanced equation for the overall reaction in acidic solution. AgCl(s) + Cu2+ (aq) + 3 e → Ag(s) + Cu(s) + CI+ (aq) 04- 03. 02. + 2 O 4+ 1 2 3 4 5 6...
Question 7 of 16 > Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E ). Pt(s) + Fe2+ (aq) = P22+ (aq) + Fe(s) [Fe2+] = 0.0017 M [P12+] = 0.040 M The cell is O spontaneous. O not spontaneous Cu(s) + 2 Ag+ (aq) = Cu2+(aq) + 2 Ag(s) [Cu2+] =...
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