Oxidation half-reaction: Zn (s) + 2 OH- (aq) Z ZnO (s) + H20 (1) +2 €...
Mercury cells as “button” batteries are very common and consist of HgO, ZnO, and Zn(OH)2 in a KOH paste. Useful half-cell reactions: HgO(s) + H2O(l) + 2e = Hg(l) + 2OH-(aq) eo = 0.0977 V Zn(OH)42-(aq) + 2e = Zn(s) + 4OH-(aq) eo = -1.285 V Zn(OH)42-(aq) = ZnO(s) + H2O(l) + 2OH-(aq) A)Such batteries have a + sign marked on them. Which half-reaction is occurring at the electrode so marked? B)Draw a schematic of a mercury...
Identify the oxidation half reaction of Zn(s). Select one: O Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu(s) O Zn²+ (aq) + 2e + Zn(s) Zn(s) → Zn2+ (aq) + 2 e Zn(s) → Zn2+ (aq) +e
Consider the following reaction. 2Ag^+(aq) + Zn(s) --> 2Ag(s) +Zn(aq) a) write the individual oxidation and reduction half-reactions, specifying which is the anode and which is the cathode reaction. b) calculate the cell potential for a cell containing 0.10M Ag^+ and 0.25M Zn^2+ at 298K. (E ag= 0.80 V and E zn= -0.76 V)
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
5. (12 points) For the following oxidation reduction reaction: Zn(s)+NO3 (aq) > Zn2*(aq) + N2(g) + H20 a. What are the oxidation numbers of the reactants and products? Oxidation Number in products Element Oxidation Number in reactants Zn N b. Write the balanced oxidation half-reaction and the reduction half-reaction. (in acid medium) Balanced oxidation half-reaction: Balanced reduction half-reaction: Write the balanced full reaction c.
1. For the oxidation-reduction reaction Zn(s) + 2HNO3 (aq) → H2(g) + Zn(NO3)2 (aq) Hint: HNO3 a) provide equation for the oxidation half-reaction: b) provide equation for the reduction half-reaction: In the given equation above or in your answers to a) and b): c) label the substance which is oxidizing agent, d) label the substance which is reducing agent.
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help determine the chart. Please Show Work thank you so much An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
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:
The standard cell potential (Eocell) of the zinc-air battery is 1.65V. If at 25.0oC the partial pressure of oxygen in the air diffusing its cathode is 0.24 atm, what is the cell potential (Ecell)? Assume the cell reaction is: 2 Zn(s) + O2(g) yields 2 ZnO(s) The standard reduction potentials of the half-reactions in zinc-air batteries are: ZnO(s) +H2O(l) + 2e- yields Zn(s) + 2OH-(aq) Eored = -1.25V O2(g) + 2 H2O(l) + 4e- yields 4 OH-(aq) Eored= 0.401 Should...
MnO2(s) + HBr(aq) → MnBr2(aq) + Br2(l) (in acid) Reduction half reaction: Oxidation half reaction: Full balanced equation: