Calculate [Cu2+] when E cell is 0.22 V. AP CHEMISTRY. Add your answer and earn points. spontaneous reaction generates an electric current. Chlorine is gaining electrons and being oxidized. According to the first law of thermodynamics, the energy given off in a chemical reaction can be converted into heat, work, or a mixture of heat and work. Get your answers by asking now. zn(s) + cu2+ (aq) —> zn2+ (aq) + cu(s) which half reaction correctly describes the oxidation that is taking place? A student balances the following redox reaction using half-reactions. *Consider that: (a) The reaction … E° = 1.51 V). Hg2CI2(aq) +2 Cu (s) Standard reduction Potentials are given below. Chlorine is losing electrons and being oxidized. Ion-electron equations are found on page 11 of the Data Booklet. Chlorine is gaining electrons and being oxidized. Balancing the electrons gives the overall reaction as: SO 4 2-(aq) + 4H+(aq) + Sn2+(aq) !SO 2(g) + 2H 2O(l) + Sn 4+(aq) The cell potential is E° = ((+0.20) + (−0.15)) V = +0.05 V. As E° > 0, the reaction should occur but the value is very small so an equilibrium mixture will form. During a redox reaction, the term reduction refers to. Au3+ + 3 e- → Au (s) ξo= 1.420 V Br2 (l) + 2 e-→ 2 Br- (aq) ξo= 1.087 V Calculate the equilibrium constant (K) for this cell. (3. 1 0. 3.7k views. Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.3×10-4 M). … Oxidation: Zn Zn 2+ + 2 e-Reduction: 2 H + + 2 e-H 2: By separating the two half-reactions, the energy given off by this reaction can be used to do work. Add the half-reactions together. What is the final, balanced equation that is formed by combining these two half reactions? E o reduction of Zn2+ = - 0.762 V Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq) || Cl2(g), Cl−(aq) | Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, Chemical Formulas and Reactions. Chlorine is losing electrons and being reduced. Before a discussion of the cell reaction, ... and the left-hand half-reaction, written as an oxidation, is added to it. Zn(s) + 2H+(aq) mc013-1.jpg Zn2+(aq) + H2(g) has an overall reduction potential of 0.76 V. Therefore. [30 Points] Consider the incomplete reaction (partial ionic equation) given below: A) Cu^2+ + Zn --> Zn^2+ + Cu I) Give the two half equations for this reaction; oxidation + reduction II) Identify the chemical substance (species) that has undergone oxidation Write the balanced oxidation half reaction that occurs. Solved: Consider the reaction below: Fe (s) + Cu2+ (aq) \rightarrow Cu (s) + Fe2+ (aq) Which species is reduced at the cathode? The measured voltage is +0.060 V. Taking [ Cu 2 … What is the overall reduction potential for the reaction Ag+(aq) + Cu(s) -------- Ag(s) + Cu2+ (aq) mc024-35.jpg. Consider this redox reaction: Al + Ag + → Al 3+ + Ag. A battery that cannot be recharged is a fuel cell. The information below describes a redox reaction. Recombine the two half-reactions by adding all the reactants together on one side and all of the products together on the other side. Cl2(g) + 2e- --> 2Cl-(aq) Consider the half reactions below for a chemical reaction. Calculate the value of ΔG° and K for this cell. E. How many of these battery designs involve zinc: Leclanche cell, alkaline, mercury, lithium-ion? In a disproportionation reaction, the disproportionate substance, What is the overall reduction potential for the reaction Al3+(aq) + Mg(s) ------ Al(s) + Mg2+(aq) mc025-35.jpg. Chlorine is losing electrons and being oxidized. E°cell = 0.61 V 2Cr(s) + 3Pb2+(aq) Picture 3Pb(s) + 2Cr3+(aq) (a)4.1 × 10^20 (b)8.2 × 10^30 (c)3.3 × 10^51 (d)7.4 × 10^61 (e)> 9.9 × 10^99. Consider the half reaction below. Consider the reaction that occurs when copper is added to nitric acid. The following cell is set up: Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) Write down the equation for the reaction which takes place in each half cell. 4 b. spontaneous combustion - how does it work? Calculate the cell potential at 25°C when the concentration of Ag+ in the compartment on the right is the following.c. In a redox reaction, an electron is lost by the reducing agent. Cu(s) E° = +0.34 V Sn2+(aq) + 2 e- ? Consider this redox reaction: Al + Ag + → Al 3+ + Ag. Zn(s) + Cu2+ (aq) -- Zn2+ (aq) + Cu(s) Zn(s) + Cu2+ (aq) Cu* (ag)+ 2e" Zn2+ (aq) + Cu(s) Cu(aq) + Zn(s) Zn2+ (aq) + 2e" - Cu2(aq) + 2e 1 See answer gabriellasanchez383 is waiting for your help. Oxidation involves the LOSS of electrons (OIL): Fe Fe2+ + 2e Mg Mg2+ + 2e The ion-electron equation for oxidation must be written in reverse. zn(s) —> zn2+ (aq) +e-zn(s) -> zn2+ (aq) + 2e-o cu2+(aq) +2e- cu(s) o cu2+ (aq) + cu(s) Answers: 2 Get. Still have questions? This is a redox reaction in which octane (C8H18) is oxidized. a) C... Dec 14 2011 05:36 PM. The Nernst equation can be applied to half-reactions. The function of the salt bridge is to maintain electrical neutrality in each half cell. E° = 0.34 V). At first glance, this equation seems balanced: there is one Ag atom on both sides and one Al atom on both sides. (The half-reaction is Cu2+ + 2e- --> Cu. Which answer best describes what is happening in the following reaction? Which type of reaction occurs in the following equation? Chlorine is gaining electrons and being reduced. Consider the half reactions below for a chemical reaction. Which is an important step in the alternate method for balancing equations in redox reactions? Gold (Au) goes from an oxidation number of +3 to 0 in the reaction below. Which step should be completed first when using this method? The Nernst equation can be applied to half-reactions. Balanced half-reactions are well tabulated in handbooks and on the web in a 'Tables of standard electrode potentials'. The cell is at equilibrium. CuS(s) +6 NO3−(aq)+8H+(aq)=== Cu2+(aq) + 6NO2(g) + SO2(g)+4H2O charge conservation both ends of the … The oxidation reaction, the anode reaction discussion of the above metals or metal ions will oxidize Fe s. Is nonspontaneous with a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell at atm. Of finding oxidation states of atoms of Volts NO_3^- ) # ions flood in to the |... Is usually -2, by convention, contain the half-cell Cu/Cu2+ ( 1.3×10-4 M ) [ Cu2+ ] E! Hydrogen gas at 1 atm is bubbled through 1 M HCl solution -88.8 None are -374.4. 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