a.) Determine E cell for the reaction b) Using the data given in the option, determine...
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) +...
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2 +] = 0.848 M and [Ni2+] = 0.0110 M. Use the standard reduction potentials in this table. Mg(s) + Ni2+(aq) = Mg2+ (aq) + Ni(s)
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Ag* concentration is 7.01x10" M and the Mg2+ concentration is 1.14 M? 2Ag+ (aq) + Mg(s) +2Ag(s) + Mg2+ (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
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2 Use the standard reduction potentials in this table 0801 M and [Fe+] 0.0120 M. Mg(s) + Fe2+(aq) Mg2+(aq) + Fe(s)
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg2+] = 0.893 M and [Ni2+] = 0.0140 M. Use the standard reduction potentials in this table. Mg(s) + Ni2+ (aq) = Mg2+ (aq) + Ni(s) E = V
Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the concentrations. Co(s)∣∣Co2+(aq, 0.0155 M)‖‖Ag+(aq, 2.50 M)∣∣Ag(s)Co(s)|Co2+(aq, 0.0155 M)‖Ag+(aq, 2.50 M)|Ag(s) net cell equation: Co+2Ag+⟶Co2++2AgCo+2Ag+⟶Co2++2Ag Calculate ?∘cellEcell∘, Δ?∘rxnΔGrxn∘, Δ?rxnΔGrxn, and ?cellEcell at 25.0 ∘C25.0 ∘C, using standard potentials as needed Calculate Ecell, AGixn , AGxn , and Ecell at 25.0 °C, using standard potentials as needed. AG x = -89.4 AGxn = -104 E cell = .54
What is the calculated value of the cell potential at 298 K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 5.79 x 10-4 M and the Mg2+ concentration is 1.03 M ? Hg2+ (aq) + Mg(s) → Hg(1) + Mg2+ (aq) Ecell = V The cell reaction as written above is for the concentrations given. Submit Answer Retry Entire Group 8 more group attempts remaining
Calculate the cell potential for the reaction as written at 25.00 °C , given that [Mg2+]=0.754 M[Mg2+]=0.754 M and [Ni2+]=0.0200 M[Ni2+]=0.0200 M. Use the standard reduction potentials. Mg(s)+Ni2+(aq) <-- double arrows --> Mg2+(aq)+Ni(s) What is E (in V)?
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Mg2 ] = 0.781 M and [Sn2 ] = 0.0150 M. Standard reduction potentials can be found here. Mg(s) + Sn2+(aq) Mg2+(aq) + Sn(s) E= __________V
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...