Equations can be balanced by using the half-reaction method. Solved: Consider the reaction below: Fe (s) + Cu2+ (aq) \rightarrow Cu (s) + Fe2+ (aq) Which species is reduced at the cathode? Fe(s) E° = -0.44 V. Al3+(aq) + 3 e- ? *Consider that: (a) The reaction … 1 0. (Recall that O has an oxidation number of -2. The cell is at equilibrium. Which step should be completed first when using this method? needed to form a whole reaction (redox reaction). Oxygen is usually -2. Calculate the e.m.f of this cell. (This is exactly the same as subtracting the left-hand equation written as a reduction, which is the formally correct procedure.) Social Studies, 22.06.2019 06:00, isaiahromero15. Copper is being reduced. 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? Cu(s) E° = +0.34 V Sn2+(aq) + 2 e- ? Consider a cell given below Cu|Cu^2+|| Cl^-|Cl2,Pt Write the reactions that occur at anode and cathode ← Prev Question Next Question → 0 votes . What is the final, balanced equation that is formed by combining these two half reactions? 88.8 O 243.2 0 -0.46 0 -88.8 None Are Correct -374.4. Solution for Consider the redox reaction Fe(s) + Cu2+(aq) -----> Fe2+(aq) + Cu(s) Which substance gets oxidozed? Mg(s)E° = -2.37 V Which of the above metals or metal ions will oxidize Fe(s)? E. How many of these battery designs involve zinc: Leclanche cell, alkaline, mercury, lithium-ion? 4. CuS(s) +6 NO3−(aq)+8H+(aq)=== Cu2+(aq) + 6NO2(g) + SO2(g)+4H2O charge conservation both ends of the … Calculate the cell potential at 25°C when the concentration of Ag+ in the compartment on the right is the following.c. Which rule for assigning oxidation numbers is correct? E° = 0.34 V). Which of the following is not an oxidation-reduction reaction? The voltage is defined as zero for all temperatures. −43.1 kJ; 1.37 × 1043 c. 86.3 kJ; 7.92 × 10−16 d. 86.3 kJ; 2.00 × 1086 e. −86.3 kJ; 1.34 × 1015. Fe(s) E° = -0.44 V Al3+(aq) + 3 e- ? Remember. Chlorine is gaining electrons and being oxidized. A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. 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). What is the reducing agent in 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. Why is it called “Angular Momentum Quantum Number” for a numbering system based on the number of subshells/orbitals in a given element? a. 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. Which half reaction correctly describes the reduction that is taking place? 7.4 × 10^61. 5 years ago. When aqueous copper(II)chloride reacts with aqueous ammonium phosphate, soluble ammonium chloride forms and copper(II) … Is this reaction an… E o reduction of Zn2+ = - 0.762 V (The half-reaction is Cu2+ + 2e- --> Cu. Ion-electron equations are found on page 11 of the Data Booklet. In the reaction equation BrO-3(aq) --------- Br-(aq) + BrO-4(aq), how many oxidation states does the disproportionate substance have throughout the reaction? 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