2Cl-(aq)----->Cl2(g)+2e-Which statement best describes what is taking place? Get your answers by asking now. 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. Consider this redox reaction: Al + Ag + → Al 3+ + Ag. From which electrode do electrons flow away from and into the external circuit? 0.61 c. 0.068 d. 0.63 e. 0.60 25. Cu(s) E° = +0.34 V Sn2+(aq) + 2 e- ? Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.3×10-4 M). Cu2+(aq) + 2e- ----- Cu(s) mc002-1.jpg Which statement best describes what is taking place? An electrochemical cell is a system consisting of two half cell reactions connected in such a way that chemical reactions either uses or generates an electric current Zn Zn 2+ Cu Cu salt bridge V Measure of emf: “electron pressure” oxidation ANODE e e reduction CATHODE Zn + Cu2+ →Zn2+ + Cu What is the concentration of Sn2+ if Zn2+ is 2.5 X 10-3 M and the cell emf is 0.660 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? These tables, by convention, contain the half-cell potentials for reduction. to identify the half reactions for the equation. Cu2+ + 2e-Cu E = 0.34 V Cr3++ 3e-Cr E = -0.74 V Fe(s) E° = -0.44 V Al3+(aq) + 3 e- ? Consider the reaction below. 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. (The half-reaction is Cu2+ + 2e- --> Cu. Show transcribed image text. Cu (s) 0.34 27 What is the cell potential, Ecell for the following concentrations at 298 K? 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. 88.8 O 243.2 0 -0.46 0 -88.8 none are correct -374.4 4. Which type of reaction occurs in the following equation? (The half-reaction is Cu2+ + 2e- --> Cu. Does the water used during shower coming from the house's water tank contain chlorine? The reaction below was carried out in an acidic solution. E° = 0.34 V) AND 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. At first glance, this equation seems balanced: there is one Ag atom on both sides and one Al atom on both sides. Al(s) E° = -1.66 V . View Available Hint(s) Consider the reaction below. Cu2+)-0.02M (CI1-0.3M [Hg2Cl21-0.005M Express your answer in units of Volts. Remember. Source(s): cu no3 aq gt cu2 aq g: https://shortly.im/L25VO. Which substance loses electrons in a chemical reaction? 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. (Recall that O has an oxidation number of -2. P 4 + 6 CaSiO 3 + 10 CO Identify the following: element oxidized element reduced oxidizing agent reducing agent Balancing Redox Equations: the Half-Reaction Method in acidic solution 1. Solution for 7. Cu(s) E° = +0.34 V. Sn2+(aq) + 2 e- ? Consider a cell given below Cu|Cu2+|| Cl-|Cl2,Pt Write the reactions that occur at anode and cathode. Consider the reaction below. Construct a galvanic (voltaic) cell from the half reactions shown below. 4 b. Solved: Consider the reaction below: Fe (s) + Cu2+ (aq) \rightarrow Cu (s) + Fe2+ (aq) Which species is reduced at the cathode? (This is exactly the same as subtracting the left-hand equation written as a reduction, which is the formally correct procedure.) Hi! Equations can be balanced by using the half-reaction method. Platinum, which is inert to the action of the 1 M HCl, is used as the electrode. What is the value of the equilibrium constant for the cell reaction below at 25°C? Which is an important step in the alternate method for balancing equations in redox reactions? During a redox reaction, the term reduction refers to. Try using these numbers see what you get. Zn -> Zn2 + (aq) + 2e- Cu2+(aq) + 2e -> Cu(s) Hg2CI2(aq) +2 Cu (s) Standard reduction Potentials are given below. needed to form a whole reaction (redox reaction). Before a discussion of the cell reaction, ... and the left-hand half-reaction, written as an oxidation, is added to it. 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? Which of the metal on the list can reduce Fe2+(aq) to Fe(s)? A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. It can be formally divided into separate oxidation and reduction half-reactions. Determine net ionic equations for both half-reactions 2. 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 43.1 kJ; 3.55 × 107 b. Sn(s) E° = -0.14 V Fe2+(aq) + 2 e- ? (3. 2Cl-(aq)----->Cl2(g)+2e-Which statement best describes what is taking place? is both an oxidizing and a reducing agent. Calculate [Cu2+] when E cell is 0.22 V. chemistry 2 Fe(s) E° = -0.44 V Al3+(aq) + 3 e- ? Chlorine is losing electrons and being reduced. The #sf(Cu|Cu^(2+))# half cell has the least +ve value so this will shift right to left and give out electrons. Multiply each half reaction to make the number of electrons equal. Zn(s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s) Cu2+→Cu+2e−… Consider the hall reactions below for a chemical reaction ... What is the overall equation for this chemical reaction? A. Cu2+ B. Cu C. Fe2+ D. Fe Which… A voltaic cell is constructed with an Ag/Ag+ half-cell and a Pb/Pb2+ half-cell. The two half-reactions can be combined just like two algebraic equations, with the arrow serving as the equals sign. Mg(s)E° = -2.37 V Which of the above metals or metal ions will oxidize Fe(s)? b. 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. Consider this redox reaction: Al + Ag + → Al 3+ + Ag. E o reduction of Cu2+ = + 0.339 V. Look up the standard reduction potential for the reverse of the oxidation reaction and change the sign. --half reaction 1 answer below » Consider the following half-reactions: Cu2+(aq) + 2 e- ? Which of the following is not an oxidation-reduction reaction? In order to oxidize Fe(S) the half reaction voltage of that compound must be GREATER than that of Fe(s). Write the balanced reduction half reaction that occurs. chemistry. Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.3×10-4 M). Ion-electron equations are found on page 11 of the Data Booklet. It is not balanced for charge or for number of atoms. When aqueous copper(II)chloride reacts with aqueous ammonium phosphate, soluble ammonium chloride forms and copper(II) … Copper is being reduced. Balance the following oxidation-reduction reactions, which occur in basic solution, using the half-reaction method. spontaneous reaction generates an electric current. Balance the following oxidation-reduction reaction that occurs in acidic solution using the half-reaction method. 1 0. Consider the half reactions below for a chemical reaction. Al(s) E° = -1.66 V Mg2+(aq) + 2 e- ? Oxidation involves the LOSS of electrons (OIL): Fe Fe2+ + 2e Mg Mg2+ + 2e The ion-electron equation for oxidation must be written in reverse. … 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. E° = 0.34 V). The Nernst equation can be applied to half-reactions. Use the reduction potentials in Appendix E that are reported to three significant figures. 1 Approved Answer. E° = 1.51 V). a) C... Dec 14 2011 05:36 PM. Is this reaction an… Equations can be balanced by using the half-reaction method. The voltage is defined as zero for all temperatures. 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). REDOX Reactions A REDOX reaction involves two half reactions - oxidation and reduction. the reaction is spontaneous and will proceed without any energy input. Chlorine (Cl) is the oxidizing agent because it gains an electron. A student balances the following redox reaction using half-reactions. To find the emf of the cell, subtract the least +ve #sf(E^@)# value from the most +ve: A battery that cannot be recharged is a fuel cell. Consider the reaction that occurs when copper is added to nitric acid. a. Calculate [Cu2+] when E cell is 0.22 V. chemistry 2. What is the reducing agent in the following reaction? Identify the element oxidized and the element reduced. 2Hg(I) + 2 Cu2 + (aq) +2CI-(aq)? See the answer . 0.64 b. Solution for In the galvanic cell using the redox reaction below, the cathode half-reaction is _____. What is the formula to create hydo-clormethane ? This is a redox reaction in which octane (C8H18) is oxidized. 321 The measured voltage is +0.060 V. Taking [ Cu 2 … Balance Redox Reactions (Half Reactions) Example: Balance the two half reactions and redox reaction equation of the titration of an acidic solution of Na 2 C 2 O 4 (sodium oxalate, colorless) with KMnO 4 (deep purple). Calculate the reduction potential (at 25°C) of the half-cell Cu/Cu2+ (1.3×10-4 M). Which answer best describes what is happening in the following reaction? a. [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 Consider the reaction below. A silver ion gains electrons more easily and is a stronger oxidizing agent than a chromium(III) ion. 2. (Recall that H usually has an oxidation number of +1.). the one that is oxidized, which is the reducing agent. Question: 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. Add the half-reactions together. Which of the following substances is the most powerful oxidizing agent? 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