question iii 10. An electrochemical cell consists of a standard Fe/Fe electrode (Fe (aq) (1.OM) IFe...
In the following cell, A is a standard Cu2+Cu electrode connected to a standard hydrogen electrode. If the voltmeter reading is +0.34 V, which half-reaction occurs in the left-hand cell compartment? Given: Standard reduction potential of the H1/H2 and Cu2*/Cu couples are 0.00 and +0.34 V, respectively. Holo H2(g) --> 2H+ (aq) + 2e7 2H(aq) + 2e --> H2(g) Cu(s) --> Cu2(aq) + 2e Cu2(aq) + 2e --> Cu(s)
The following data were measured using a nickel electrode as the standard: Cu2+(aq) + 2e- ⟶ Cu(s) Ni2+(aq) + 2e- ⟶ Ni(s) Fe2+(aq) + 2e- ⟶ Fe(s) Al3+(aq) + 3e- ⟶ Al(s) The copper and aluminum electrodes are connected in a battery. A) Which is the anode? Cathode? Why? B) Which is oxidized? Reduced? Why? C) What will the battery voltage be? Eo =0.62V Eo =0.00V Eo =-0.15V Eo =-1.38V D) Write a balanced net ionic equation for the reaction...
Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO3)2 electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction: (If needed, refer to Table 17-1.) 0.669 V, Fe(s) + AgCl(s) → Fe2+(aq)+ Ag(s) + Cl-(aq) 0.669 V, Fe(s) + 2AgCl(s) → Fe2+(aq)+ 2Ag(s) + 2Cl-(aq) –0.225 V, Fe(s) + 2AgCl(s) → Fe2+(aq)+ 2Ag(s) + 2Cl-(aq) 0.259 V, Fe(s)+ 3AgCl(s) → Fe3+(aq)+...
Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO3)2 electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction: (If needed, refer to Table 17-1.) 0.669 V, Fe(s) + 2AgCl(s) → Fe2+(aq) + 2Ag(s) + 2Cl-(aq) –0.669 V, Fe(s) + 2AgCl(s) → Fe2+(aq) + 3Ag(s) + 3Cl-(aq) –0.225 V, Fe(s) + 2AgCl(s) → Fe2+(aq) + 2Ag(s) + 2Cl-(aq) 0.669 V, Fe(s)...
For the electrochemical cell, Fe(s)| Fe2+ (aq)|| Cu2+ (aq)| Cu+ (aq) | Pt(s), determine the equlibrium constant (Keq) at 25°C for the reaction that occurs.
In a copper-zinc voltaic cell, one half-cell consists of a ZnZn electrode inserted in a solution of zinc sulfate and the other half-cell consists of a CuCu electrode inserted in a copper sulfate solution. These two half-cells are separated by a salt bridge. At the zinc electrode (anode), ZnZn metal undergoes oxidation by losing two electrons and enters the solution as Zn2+Zn2+ ions. The oxidation half-cell reaction that takes place at the anode is Zn(s)→Zn2+(aq)+2e−Zn(s)→Zn2+(aq)+2e− The CuCu ions undergo reduction...
Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NOx), electrolyte connected through a salt bridge to a Ag wire coated in Agcl(s) immersed in an aqueous KOI solution. Is the standard cell and balanced galvanic cell reaction: (If needed, refer to Table 17-1.) 0.669 V, Fe(s) + ACI(S) - Fe2+ (aq) + Ao(s) + Cl(aq) 0.259 V, Fe(s) + 3ACI(S) - Fel(aq) + 3A(S) + 3(aq) -0.669 V, Fe(s) + 2ACI(S) - Fe2+ (aq) + 3A(s) + 3Cl(aq) -0.225...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
*A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.070 V at 298 K. A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [NH. If a standard hydrogen electrode is used as the cathode, the cell potential,...
Half-Reaction Fe2+(aq) + 2e Fe(s) Hg2+ (aq) + 2e Hg() Ag+ (aq) + e + Ag(s) Cu2+ (aq) + 2e + Cu(s) Zn2+ (aq) + 2e → Zn(s) E (V) -0.44 0.86 0.80 0.34 - 0.76 Using the table, calculate Eºcell for the following electrochemical cell under standard conditions voltmeter a) 1.24 V Fe. salt bridge Ag b) -1.24 V c) 2.04 V d) - 2.04 V Ag a b С