C-1. DETERMINE THE E° FOR A VOLTAIC CELL For each cell write the anode half reaction and the cathode half reaction. From the measured voltages, calculate the half-cell potentials for the lead and tin half-cells and the equilibrium constants for these two reactions. In these calculations, use E° = 0.34 V for the Cu2+/Cu couple.
Cell | trial 1 | trial 2 | trial 3 |
Cu-Pb | 0.505 V | 0.506 V | 0.508 V |
Cu-Sn | 0.688 V | 0.688 V | 0.691 V |
Pb-Sn | 0.190 V | 0.190 V | 0.190 V |
C-2. MEASURING CELL POTENTIAL AS A FUNCTION OF TIME Calculate ΔG for the cell at each of these temperatures. Plot ΔG as a function of temperature and obtain a best fit line. The slope will be –ΔS. From the values for free-energy, and entropy calculate the enthalpy at 298K.
Cu-Sn (temp in Kelvin) | Voltage |
383 | 0.731 V |
328 | 0.726 V |
313 | 0.717 V |
298 | 0.707 V |
274.4 | 0.680 V |
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C-1. DETERMINE THE E° FOR A VOLTAIC CELL For each cell write the anode half reaction...
Rearrange the following half-reaction to create an electrochemical cell. Write the labelled cathode half-reaction, anode half-reaction, and net ionic reaction. Also calculate the net cell potential. Cu(s )| Cu2+(aq) NO3-(aq) || Na+(aq) SO42-(aq) | Pb(s)
Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e– → Sn(s). What is the concentration of Sn2+ if Zn2+ is 2.5 × 10−3 M and the cell emf is 0.660 V? The standard reduction potentials are given below Zn+2(aq) + 2 e− → Zn(s) E∘red == −0.76 V Sn2+(aq) + 2 e– → Sn(s) E∘red −0.136 V
Write the half reactions and overall reaction for each cell with calculated overall potentials as shown in Table 5-1. (Note: for the iron solutions the Nernst equation must be used) Pb(s) | Pb(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) Cu(s) Zn(s) | Zn(NO3)2(0.1M) || Cu(NO3)2 (0.1M) Cu(s) Cds) | Ca(NO3)2 (0.1M) || Cu(NO3)2 (0.1M) | Cu(s) Cu() Cu(NO3)2(0.1M) Il Fe (0.1M/Fe? (0.1M graphite Pb(s) Pb(NO3)2(0.1M) Il Fe3(aq) (0.1M)/ Fe2(aq) (0.1MI graphite(s) Zns | Zn(NO3)2 (0.1M) || Pb(NO3)2 (0.1M) | Pb(s) Cdis Ca(NO3)2...
tandard reduction half-cell potentials at 25 ∘ C Half-reaction E ∘ ( V ) Half-reaction E ∘ ( V ) A u 3+ (aq)+3 e − →Au(s) 1.50 F e 2+ (aq)+2 e − →Fe(s) − 0.45 A g + (aq)+ e − →Ag(s) 0.80 C r 3+ (aq)+ e − →C r 2+ (aq) − 0.50 F e 3+ (aq)+3 e − →F e 2+ (aq) 0.77 C r 3+ (aq)+3 e − →Cr(s) − 0.73 C u +...
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73 0.52 -0.76 0.34 -1.18 Half-reaction Aut (aq) + 3e +Au(s) Ag+ (aq) + +Ag(s) Fe3+ (aq) +34 Fo+ (aq) Cut(aq) + Cu(s) Cu²+ (aq) + 2e +Cu(s) 2H+ (aq) - 2e +H2 (6) Fe3+ (aq) + 3e Fe(s) Pb2+ (aq) + 2e →Pb(s) Sn-(aq) + 2e +Sn(s) Ni2+ (aq) + 2e →Ni(s) Co2(aq) +2e + Co(s) ca? (aq) + 2e +Cd(s) 0.00 Half-reaction Fe(aq)...
A certain half-reaction has a standard reduction potential E = -0.45 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. 0-0 . " Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell...
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction + O2(9)+4 H (aq)+4e' 2H20) = 1.23 V red Ered Fe+. (аq) Fe3(aq)+e = +0.771 V Answer the following questions about thiss cell Write a balanced equation for the half-reaction that happens at the cathode Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous...
Please show all steps taken (prefer typed solution) Half-Reaction E ° (V) Ag+ (aq) + e− → Ag (s) 0.7996 Al3+ (aq) + 3e− → Al (s) −1.676 Au+ (aq) + e− → Au (s) 1.692 Au3+ (aq) + 3e− → Au (s) 1.498 Ba2+ (aq) + 2e− → Ba (s) −2.912 Br2 (l) + 2e− → 2Br− (aq) 1.066 Ca2+ (aq) + 2e− → Ca (s) −2.868 Cl2 (g) + 2e− → 2Cl− (aq) 1.35827 Co2+ (aq) + 2e−...
Use the following half-reactions to write 3 spontaneous reactions, calculate E°cell for each reaction, what is the n number (number of electrons transferred). Au+ (aq) + e− → Au (s) E° = 1.69 V N2O (g) + 2H+ (aq) + 2 e− → N2 (g) + H2O (l) E° = 1.77 V Cr3+ (aq) + 3 e− → Cr (s) E° = -0.74 V Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
A certain half-reaction has a standard reduction potential E Ted =-0.99 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 0.90 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell O- Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have?...