3. (24 points) Consider the following reaction: Au(s) + NO3(aq) + 4H+ (aq) → NO(g) +...
E° = -0.04 V For the reaction: Au(s) + 4H+ (aq) + NO3(aq) + 4Cl(aq) → AuCl4- (aq) + NO(g) + 2H20 If the standard potential for the reduction of NO3(aq) to NO(g) is +0.96 V, determine the value of Eº for the following half-reaction AuCl4 (aq) + 3e → Au(s) + 4C1 (aq)
Half-potentials. Homework – Unanswered Due in 8 hours For the reaction: Au(s) + 4H" (aq) + NO3(aq) + 4C"(aq) -- Aucla (aq) + NO(g) + 2H20 the standard potential E=-0.04 V. If the standard potential for the reduction of NO3 aq) to NO(g) is +0.96 V, determine the value of Efor the following half-reaction. AuCl(aq) + 3e - Au(s) + 4C1 (aq) (answer in V) Numeric Answer:
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at 25 ∘C , given that [Fe3+]=0.00150 M and [Au3+]=0.795 M . Refer to the table of standard reduction potentials. E= V
10. Consider the following electrochemical cell at 25°C : Sn(s)ISn2 (aq, 0.0155 M)|IAg* (aq, 2.50 M)IAg(s) a. Calculate the cell potential b. Calculate the Gibbs free energy change c. Is this a galvanic or electrolytic cell?
Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s) Q3\ For the previous cell, determine the concentration of the cobalt ion when a cell voltage of 1.76 V is obtained using a 0.761 M gold (III) nitrate solution. Q4\ Calculate the free energy for the nonstandard cell in the previous problem. Show all work. Be mindful of signs, sig figs, and units Q5\ Consider a galvanic cell consisting of the following two redox couples: Sn2+ (aq, 0.010 M)...
The following occursin a galvanic cell that utilizes the following reaction (unbalanced):(AuCl4)-(aq)+Cu(s)=Au(s)+Cl-(aq)+Cu^2+(aq)Given the following information determine the standard cell potentail:Au^3+= 1.4980 VCu^2+= -.3389 VA: .8292B: 4.1551C: 1.1591D: 1.8369E: 3.8162
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+Pb(NO3),(aq) → Ni(NO3)2(aq)+Pb(s) E1 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?
A galvanic cell at a temperature of 25.0°C is powered by the following redox reaction: 2VO+2(aq)+4H+(aq)+Fe(s)->2VO+2(aq)+2H2O(l)+Fe+2(aq) Suppose the cell is prepared with 3.82 M VO+2 and 1.96 M H+ in one half-cell and 4.70 M VO+2 and 6.88 M Fe+2 in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
5) Will this reaction occur spontaneously as written? (3 points) why 3Pb(s) + NO3 (aq) + 8H(aq) 3Pb2+(aq) + 2NO(g) + 4H2O(1)
Suppose the galvanic cell sketched below is powered by the following reaction: 4 Fe(s)+2 Fe(NO3)2(aq) — 3 Fe(NO3),(aq)+3 Fe(s) S1 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?