An electrochemical cell based on the following reaction has astandard cell voltage (Eocell) of 0.48 V...
Find the best combination of half-cell pair from the following list, which will give the highest voltage. What is the voltage for that Galvanic cell? Given that Reduction Half-reaction Standard Potential (Eredo) Zn2+(aq) + 2e– → Zn(s) -0.763 (V) Fe2+(aq) + 2e– → Fe(s) -0.44 (V) Cu2+(aq) + 2e– → Cu(s) +0.34 (V) Sn2+(aq) + 2e– → Sn(s) -0.14 (V) Cu2+(aq) + e– → Cu+(aq) + 0.153 (V) Ag+(aq) + e– → Ag(s) + 0.80 (V) Cu+(aq) + e– →...
Given the following standard reduction potentials choose the cell which will work as a voltaic cell. All cells below are written according to the usual cell diagram convention. Cu2+(aq) + 2e → Cu(s) E° = 0.34 V 2H+(aq) + 2e → H2(g) E° = 0.00 V Sn2+ (aq) + 2e → Sn(s) E° = -0.14 V Ni2+(aq) + 2e → Ni(s) E° = -0.26 V Cd2+(aq) + 2e → → Cd(s) E° = -0.40 V Sn(s) | Sn2+(aq) || Ni2+(aq)...
QUESTION 4 Using the table below and the Nearnst Equation E-E° (0.0592/n)logQ Find the voltage of the cell: Cu2+(aq) + Ni(s) ? Cu(s) + Ni2+(aq) at 25° C if the concentrations of the soluble species are [Cu2+1-0.050 M and [Ni]- 1.40 M Reduction Reaction Sn2++ 2e-? Sn Cu2+ + 2e- ?Cu" Reduction Potential, Ecell 0.14 Volts 0.34 Volts 0.25 Volts +0.77 Volts Fe3+ + e-? Fe2+ 0.50 V 0.54 V 0.62 V 0.66 V
the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) fone 2 pts) a. Use the standard half-cell potentials listed below to calculate the standard cell potential (Eºcell) for 3 Sn(s) + 2 Fe* (aq) - 3 Sn2+ (aq) + 2 Fe(s) Sn 2(aq) + 2 e -Sn (s) E = -0.14 V Fe3+ (aq) + 3 e Fe(s) E° = -0.036 V A) -0.176 V B)-0.104 V C) +0.104 V D) +0.176 V b. Write...
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two metals below? Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V
What would be the standard cell potential for a spontaneous electrochemical cell constructed with the two metals below? Cu2+(aq) + 2e– → Cu(s) E° = 0.34 V Sn4+(aq) + 2e– → Sn2+(aq) E° = 0.13 V
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) Sn2+(aq, 1.8 M) II Ag+(aq, 0.55 M)1 Ag(s) Sn2+ (aq) + 2 e Ag+ (aq) + e- Sn(s) Ag(s) E = -0.14 V E = 0.80 V -0.84 V +0.86 V 0 -0.93 V +1.12 V O 0.92 V
Consider an electrochemical cell based on the following cell diagram: Pt1 Cut(aq), Cu2+ (aq) || C12(), CI (aq) | Pt Given that the standard cell emf is 1.20V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E*(Cu?+/Cut)? A) 1.01V B) 1.06 V C) 0.16 V D) 2.56 V E) -0.16 V
Table provided below for context Please answer all parts that you can. 1. Which electrochemical cell had the greatest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 2. Which electrochemical cell had the smallest voltage? Identify the anode and the cathode for this pair, the measured cell potential, and the calculated Eºcell- 3. If the oxidation and reduction half-reactions are separated in a battery, this means the oxidizing agent is...
40 points A galvanic cell is constructed using the following half reactions: Sn2++ 2 e-Sn(s) -0.14 V Cu2+ + 2 e Cu (s) +0.34 V Based on their reduction half-potentials, which metal will likely serve as the cathode and what would be the Eºcell for the cell? -0.20 V; Sn O +0.48 V; Cu +0.20 V; Cu -0.48 V; Sn O +0.20 V; Sn Previous Submit