Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) + 2Ag+(aq) ----> Cu+2 (aq) + 2Ag(s) where [Ag+] = 0.00275 M and [Cu2+] = 8.75×10-4 M.
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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
1. Calculate Ecell at 298 K for a cell involving Sn and Cu and their ions: Sn(s) I Sn2+(aq,.25 m) II Cu2+(aq,.10 m) I Cu(s) a. .47 V b. .49 V c. .50 V Please explain and use equation. Thank you
Calculate Ecell at 298 K for a cell involving Sn and Cu and their ions: Sn(s) I Sn2+(aq, 0.25M) II Cu2=(aq, 0.10M) I Cu(s) A) 0.47 V B) 0.49 V C) 0.50 V
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 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 |...
1- Consider the following redox reaction: Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s) EoCell = 0.78 V If [Cu2+] = 0.3 M, what [Fe2+] is needed so that Ecell = 0.76 V 2- Calculate the Eocell for the following redox reaction: Cu(s) + 2Ag+(aq) --> Cu2+(aq) + 2Ag(s)
Calculate the cell potential for the reaction below when the concentrations of ions are: [Ag+ ] = 0.010 M and [Cu2+] = 0.750 M, at 25 °C. Cu(s) + 2Ag+ (aq) --> Cu2+(aq) + 2Ag(s) Given the standard reduction potentials: Cu2+(aq) + 2e– → Cu(s) Eϴ = 0.34 V Ag+ (aq) + e– → Ag(s) Eϴ = 0.80 V (A) 0.35 V (B) 0.44 V (C) 0.46 V (D) 0.48 V (E) 0.57 V
A voltaic cell set up utilizing the reaction Cu(s) + 2 Ag+ (aq) → Cu2+ (aq) + 2 Ag (s) has a cell potential of 0.45 V at 298 K. Describe how the potential of the cell will change as the cell is discharged. At what point does the cell potential reach a constant value? Explain your answer
please show work and how they got this answer 12. Consider the cell reaction Cu(s) + 2Agt → Cu2+ + 2Ag(s). If [Ag+] = 1.0M and Ecell = 0.62 V, then what is the concentration of Cu2+7 Eºcell = +0.46 (0.80 -0.34), Q = x/1.02, x = [Cu2+] = 3.9x10-6
Table view List view Ecell (calculated) Ecell (calculated) 1.115 1.124 Table 1. Voltaic cells data table Ecell (measured) Reaction Quotient Q 1. Zn | Zn2(1.0M) || Cu2+(1.0 M) | Cu 2. Zn | Zn2+(1.0 M) || Cu2+(0.1 M) Cu 1.067 3. ZnZn2+(0.1 M) || Cu2+(1.0 M) | Cu 4. Zn | Zn2+(1.0 M) || Pb2+(1.0 M) | Pb 5. ZnZn2(1.0M) || Pb2+(0.1 M) | Pb 0.600 6. Zn | Zn2+(0.1 M) || Pb2+(1.0 M) I Pb 0.644 7. ZnZn2+(1.0 M)...