Write the overall chemical reaction and calculate E for the following reduction and oxidation half- reactions. 2H (ag) + 2e Hz(g) = 0.000 V red Zn(s) Zn"(aq) + 2e E= +0.762 V a. Zn (aq) + H2(g) Zn(s) + 2H (aq) b. Zn (aq) + Hzlg) → Zn(s) + 2H (aq) c. Zn(s) + 2H (aq) → Zn (aq) + H(g) - d. Zn(s) + 2H (aq) → Zn (aq) + H(g) e. Zn(s) +2H (aq) → Zn (aq) + H2(g) E = +0.381 V E = -0.762 V E = +0.762 V. %3D E° = -0.762 V %3D -0.381 V

Q: Determine E° for the half-reaction Fe3 (aq) + e Fe2 (aq). Fe3+(aq) + H2(g) → 2H*(aq) + Fe2+(aq) E° =…

A: E° for the following net cell reaction = +0.77 V  Fe3+(aq) + H2(g) ---> 2H+(aq) + Fe2+(aq)  E°…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e –→ 2B1¯(aq) 1.080V Co2*(aq)…

A:

Q: Balance the following redox reaction if it occurs in a basic solution. What are the coefficients in…

A: Balancing of a redox reaction in acidic medium can be done as follows:

Q: For the reaction that occurs in the voltaic cell. Fe(s)  |   Fe2+ (aq)  | |  Cr3+ (aq),  Cr2+ (aq) |…

A: In electrochemistry, the Nernst equation is used as it relates the standard reduction potential…

Q: A voltaic cell is constructed with two Zn2+−ZnZn2+−Zn electrodes. The two cell compartments have…

A: The cell is made up of Zn electrodes only. Hence both oxidation and reduction is happening for Zn…

Q: A voltaic cell is constructed with two Zn 2+-Zn electrodes, where the half-reaction is Zn2+ + 2e-…

A: In concentration cell we used same electrodes here Zn2+ / Zn electrode but at different…

Q: For the following half-reactions: Cr3-(aq) – Cr(s) Zn2«(aq) → Zn(s) a. What will be the overall…

A:

Q: Balance the following reactions and write the reactions using cell notation. Ignore any inert…

A: (a). 3Ag+(aq)+NO(g) +2H2O ⟶3Ag(s)+NO3−(aq) + 4H+(aq) At Cathode:- 3Ag+------------> 3Ag(s)  -3e-…

Q: A current of 0.452 A is passed through an electrolytic cell containing molten CaCl2 for 1.50 hours.…

A:

Q: Determine E° for the half-reaction Fe3-(aq) + e → Fe2-(aq). Fe3 (aq) + H2(g) → 2H (aq) + Fe2•(aq) E°…

A:

Q: . Which phase changes result in ΔS < 0? 2. Which selection of coefficients properly balances the…

A: As per our guidelines , we can solve only first three questions. Please resubmit other questions as…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: From given Initially we are calculating E°cell and plugging that in ∆G° formula we get the solution…

Q: ELECTROCHEMISTRY Write the redox reactions and calculate the standard e.m.f.: Ce3+(aq) | Ce4+(aq)…

A:

Q: 7.14(b) Write the cell reaction and electrode half-reactions and calculate the standard emf of each…

A: A question based on electrochemistry, which is to be accomplished.

Q: (i) Pt(s) + 2 NH3(aq) + 2 CI ( (aq) cis-[PtCl₂(NH3)2](aq) + 2 e¯ E° = 0.274 V The likely cathodic…

A:

Q: A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in…

A:

Q: balance the following redox reaction if it occurs in basic solution what are the coefficients in…

A:

Q: . You are given the following reduction half reactions in basic solution: 2 NO2-(aq) + 3 H2O(l) + 4…

A: 2 NO2-(aq) + 3 H2O(l) + 4 e- →N2O(g) + 6 OH-(aq)    E° = 0.1500 V          HgO(s) + H2O(l) + 2 e- →…

Q: 2+ - A galvanic cell consisting of a Cu- Cu half cell versus a H - H2 half cell was used to…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: You are given the following reduction reactions and E Fe3+(aq) + e- → Fe2+(aq)        E= +0.771 V…

A: To find emf

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g)           E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm  P V = n R T  P  = ( n/ V ) R T = c R T  c = P / R T  T ( temperature ) = 25…

Q: In a Galvanic cell: Fe2+ + 2e- --> Fe Eº = -0.44V Fe3+ + 3e- --> Fe Eº = -0.04V Fe3+ + e- --> Fe2+…

A:

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

A:

Q: 1. The following redox reaction was constructed at 25.0°C. Pb²+ (aq) + Mg(s) → Pb(s) + Mg² (aq) a.…

A: The given reaction is :  Pb2+ (aq) + Mg (s) ----------&gt; Pb (s) + Mg2+ (aq)  d. As the reaction…

Q: For cell schematic notation    Zn(s) | ZnCl2 (1.0 M )| | CuSO4 ( 2.0 M ) | Cu(s)…

A:

Q: When an aqueous NaCl solution is electrolyzed, how many faradays need to be transferred at the anode…

A: FROM the reaction , we can see that for 1 mol of Cl2 , 2 faradays are required . where 1 faraday is…

Q: 5) During the operation of lead storage battery, the reaction at the two electrodes is as follows:…

A:

Q: Fe | Fe²+ (0.100M) || Cd²+(0.001) | Cd I. Write the half-reactions and cell reaction 2. Calculate…

A:

Q: The reaction between Ag+ ion and Solid Zinc given by the following equation. 2Ag+ + Zn(s) = Zn2+ +…

A: The given cell reaction is 2Ag+ + Zn(s) = Zn2+ + 2Ag(s) Anode is made by Zn Cathode is made by Ag

Q: In an electrolytic cell for aqueous KI solution: - what is the effect of [KI] - what is the effect…

A: Electrolysis is the process in which the compound is broken down into its constituent ions with the…

Q: Write the overall chemical reaction and calculate E° for the following reduction and oxidation…

A: The half reactions taking place are, Reduction : 2 H+ (aq) + 2 e- -----&gt; H2 (g)…

Q: 13) In a single replacement reaction (for example, Mg(s) + 2Ag (NO3)(aq) → 2 Ag(s) + Mg(NO3)2(aq) ),…

A: Those  metal present below in SRP table will precipitate by upper metal

Q: a. Use your knowledge of redox and equilibrium to derive an expression for Keq in terms of E°cell…

A: An expression for Keq in terms of E°cell for a general redox reaction has to be derived ΔG°rxn and…

Q: Consider the cell Pt(s)|H2(g,p°)|HCl(aq)|AgCl(s)|Ag(s), for which the cell reaction is…

A: In electrochemistry, the Nernst equation is an equation that relates the reduction potential of an…

Q: Balance the following in basic solution. (Omit states-of-matter from your answer. Use the lowest…

A: The given reaction is first noted as follows,

Q: 8. The following redox reaction occurs at 25.0°C: 5F22*(aq) + MnO4 (aq) + 8H*(aq) → Mn2 (aq) +…

A: Electrochemistry is the branch of chemistry which studies the change of chemical energy into…

Q: For the following reactions, (i) write the half-reactions, (ii) write a balanced equation for the…

A: Redox reaction- the reaction in which oxidation and reduction takes place simultaneously called as…

Q: Half Reaction A: 2H+ + 2e- ---> H2 (at standard conditions, pH 0 ) Half Reaction B: S + 2H+ + 2e-…

A:

Q: ELECTROCHEMISTRY Write the redox reactions and calculate the standard e.m.f.: a) Ni(s) | Ni2+(aq)…

A:

Q: Pb2+ + 2e– → Pb ε° = –0.13 V Cu2+ + 2e– → Cu ε° = +0.34 V If the Pb2+ and Cu2+ are each 1.0 M,…

A: This problem is based on Nerst Equation For which, first we need to calculate the E°cell E°cell =…

Q: 6. Zn + NOs- Zn²+ + NHa" (in acidic solution) 7. MnOs + H2S Mn²* + S (in acidic solution) 8. Cu +…

A:

Q: An electrochemical cell utilizes the following redox reaction NH4 + (ag) + 8Ce4*(ag) + 3H2O(I) →…

A:

Q: Determine E° for the half-reaction Fe*(aq) + e¯ → Fe²*(aq). V Fe3+(aq) + H2(g) → 2H*(aq) + Fe2+(aq)…

A: Given,  Fe3+ (aq) + H2 (g) ---&gt; 2H+ (aq) + Fe2+(aq) E°cell = + 0.77 V

Q: 8. For the oxidation-reduction reaction: S406(aq) + Cr+(aq) Cr (aq) + S202 (aq), -> the appropriate…

A: recall the given half cell reactions Reduction half cell reaction     S4O62-+2e-→2S2O32-  ......(i)…

Q: Calculate the Free Gibb’s Energy, kJ/mol, for the following redox reaction at 25.0°C. 2Ce4+(aq) +…

A: Given  The following redox reaction is - 2Ce4+ (aq) + 2Cl- (aq) →Cl2 (g) + 2Ce3+(aq) anode - 2Cl-…

Q: Cu(s)||Cu2+(aq, 0.0155 M)‖‖Ag+(aq, 3.50 M)||Ag(s)Cu(s)⁢|Cu2+⁢(aq, 0.0155 M)‖Ag+⁢(aq, 3.50 M)|Ag(s)…

A: Ok we will calculate last 2 parts.

Q: he oxidation–reduction reaction: S4O62- + Cr2+ → Cr3+ + S2O32- Half-reactions:

A: The given chemical reaction  S4O62- + Cr+2 → Cr+3+ S2O32- In an electrochemical cell, oxidation…

Q: Write the balanced half reactions of the following reactions: a. NiO2 + 2 H2O + Fe -> Ni(OH)2 +…

A:

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.