4. Hydrogen gas at 1 atm is bubbled through 1 M HCl solution. Is this reaction an… 3.7k views. Al(s) E° = -1.66 V Mg2+(aq) + 2 e- ? c. The cell reaction is spontaneous with a standard cell potential of 2.15 V. d. The cell reaction is spontaneous with a standard cell potential of 2.61 V. e. The cell reaction is nonspontaneous with a standard cell potential of -2.61 V. Mg(s)E° = -2.37 V Which of the above metals or metal ions will oxidize Fe(s)? Chemistry Chemistry: Principles and Reactions Consider a cell in which the reaction is 2 Ag ( s ) + Cu 2 + ( a q ) → 2 Ag + ( a q ) + Cu ( s ) (a) Calculate E ° for this cell. Which of the following substances is the most powerful oxidizing agent? Solved: Consider the reaction below: Fe (s) + Cu2+ (aq) \rightarrow Cu (s) + Fe2+ (aq) Which species is reduced at the cathode? Sn(s) E° = -0.14 V Fe2+(aq) + 2 e- ? Chlorine is losing electrons and being reduced. For the best answers, search on this site https://shorturl.im/WqfIZ. Redox Reaction Example: Half reaction (1) Cu (s) → Cu+2 (aq) + 2e- The half reaction here tells you that solid copper (Cu (s)) is being oxidized, losing an e-, to form the copper ion with a plus two charge (Cu+2). Add the reactions and simplify.) Consider the redox reaction below: Cu*2 + 2Ag (s) --> Cu (s) + 2Ag* Half-Reaction Cu+2 +2e --> Cu(s) Ag* + e --> Ag(s) Ecell (V) 0.34 0.80 Calculate the standard free energy (kJ) for this reaction. 1 See answer demondgary02 is waiting for your help. Figure 1. Balance the following oxidation-reduction reactions, which occur in basic solution, using the half-reaction method. What must be true of a disproportionate substance? What is the purpose of finding oxidation states in the half-reaction method for balancing equations? Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.3×10-4 M). Determine net ionic equations for both half-reactions 2. The cell reaction is nonspontaneous with a standard cell potential of -2.15 V. b. Social Studies, 22.06.2019 06:00, isaiahromero15. What is the concentration of Sn2+ if Zn2+ is 2.5 X 10-3 M and the cell emf is 0.660 V? b. E° is the standard reduction potential.The superscript “°” on the E denotes standard conditions (1 bar or 1 atm for gases, 1 M for solutes). Although it is unbalanced, it can be balanced by using the half-reaction method. (3. What is the oxidation number for N in the compound NH3? Oxidation involves the LOSS of electrons (OIL): Fe Fe2+ + 2e Mg Mg2+ + 2e The ion-electron equation for oxidation must be written in reverse. Mg2+(aq) + 2 e- ? primary battery. I tried working out the answer for both questions using this equation: Ecell= .34 - (.0592/2) log (1 / 1.3×10-4). spontaneous reaction generates an electric current. 5 years ago. Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s) Cu2+→Cu+2e−… REDOX Reactions A REDOX reaction involves two half reactions - oxidation and reduction. Half-reaction Cu2+(aq) + 2e- → Cu(s) +0.337 V Ni2+(aq) + 2e- → Ni(s) -0.28 V determine the potential (in V) of an electrochemical cell in which the concentration of nickel(II) ion is 0.155 M and the concentration of copper(II) ion is 0.352 M. (T = 298 K) a. Solution for 7. 7.4 × 10^61. a) C... Dec 14 2011 05:36 PM. Solved: Consider the reaction below: Fe (s) + Cu2+ (aq) \rightarrow Cu (s) + Fe2+ (aq) Which species is reduced at the cathode? a. Consider the reaction below. Problem: Consider the concentration cell shown below. This is a redox reaction in which octane (C8H18) is oxidized. Consider the half reactions below for a chemical reaction. What is the overall reduction potential for the reaction Ag+(aq) + Cu(s) -------- Ag(s) + Cu2+ (aq) mc024-35.jpg. See the answer . A student balances the following redox reaction using half-reactions. Which best describes the oxidizing agent in this reaction? Zn -> Zn2 + (aq) + 2e- Cu2+(aq) + 2e -> Cu(s) Equations can be balanced by using the half-reaction method. Zn !Zn2+ + 2e (oxidation half-reaction, reducing agent) (2) Cu2+ + 2e !Cu (reduction half reaction, oxidizing agent) (3) In a (slightly) more complicated example, copper metal transfers electrons to silver ions, which have an oxidation state of +1. Al + Mn2+ ----- Al3+ + Mn mc031-1.jpg A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. Consider the balanced redox reaction below. 0.64 b. Equations can be balanced by using the half-reaction method. E° (V) +0.34 Consider the following half-reactions: Half-reaction Cu2+ (aq) + 2ē → Cu(s) + 2ē → Sn(s) Fe2+(aq) + 2ē Fe(s) Zn2+(aq) + 2ē Zn(s) A13+ (aq) + 3ē Al(s) Sn2+(aq) -0.14 -0.44 -0.76 -1.66 (a) (b) (c) Based on the Eº values given above, which metal is the most readily oxidized? From which electrode do electrons flow away from and into the external circuit? Briefly explain why amino acid and fatty acid both are considered acid.? Which substance loses electrons in a chemical reaction? Explain the difference between “suspension and Emulsion” OR between “solution and colloid”. A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. Try using these numbers see what you get. c. Write the balanced net ionic equation for this reaction. Use the reduction potentials in Appendix E that are reported to three significant figures. Gold (Au) goes from an oxidation number of +3 to 0 in the reaction below. Balanced half-reactions are well tabulated in handbooks and on the web in a 'Tables of standard electrode potentials'. The following equations are half reactions and reduction potentials. The reaction below was carried out in an acidic solution. The relevant half cell reactions and reduction potentials are: Cu 2+ (aq) + 2e - Cu(s) E ° = 0.34 V Fe 2+ (aq) + 2e - Fe(s) E ° = 0.44 V Calculate the reduction potential (at 25°C) of the half-cell MnO4- (5.00×10-2 M)/ Mn2+ (2.30×10-2 M) at pH = 5.00. Fe(s) E° = -0.44 V Al3+(aq) + 3 e- ? E° = 0.34 V). Problem: An electrochemical cell has the following half cell reactions: Cu2+(aq) +2e- → Cu(s) E°1/2 = +0.34 Zn2+(aq) + 2e- → Zn(s) E°1/2 = -0.76 If the cell operates with the Cu electrode as the cathode and the Zn as the anode, What is the cell potential when the [Cu2+] = 0.001M and the [Zn2+] = 0.1M? determining the half reactions of chemical equations. Given that Cu + 2HCI ------- Cu2+ + 2CI- + H2(g) has an overall reduction potential of -0.34 V, what is a valid prediction about how this reaction works? Mn mc031-1.jpg Oxygen is usually -2 oxidation number for s in the compound NH3 electrons! Fuel cell covalent molecule Cu 2 … solution for 7 concentrations at 298 K procedure )... 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