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Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NOx), electrolyte connected through a salt bridge...
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)...
Questions 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(8) + Agci(9) - Fel*(0) + Ag(s) + Cl(aq) 0.669 V, Fe(s) + 2ACH() - Tel(aq) + 2A(8) + 2Cl(9) -0.669 V, Fe(s) + 2Ags) - Fed(0) + 3A(s) + 3Cl(aq) -0.225 V,...
Electrochemistry - Equilibrium 1. The electrochemical cell described by the balanced chemical equation has a standard emf (electromotive force) of -0.08 V. Calculate the value (J) for the Wmax that the cell can do under standard conditions. Round your answer to 3 significant figures. St. Red. Pot. (V) Faraday's Constant Hg2+/Hg +0.85 F = 96485 C Fe3+/Fe2+ +0.77 2Fe3+(aq) + Hg(l) → 2Fe2+(aq) + Hg2+(aq) 2. The voltaic cell described by the balanced chemical equation has a standard emf of...
question iii 10. An electrochemical cell consists of a standard Fe/Fe electrode (Fe (aq) (1.OM) IFe (aq) (1.0M) IPt(s) and a copper metal electrode ( concentrations) Cu2 (aq) +2e Cu(s) Fe (aq) le Fe (aq) +0.34 V -034 +0.77V Mark what is the corect balanced equation for the spontaneous reac u (aq) Fe (aq) Cu(s)+Fe2 (aq) C) Cu(s) + Fe (aq) Cu (aq) + Fe (aq) α Cu2+(aq) + 2e → Cu(s) + Fe2+(aq) Cu → Cu2ト+20 94 i) (...
given this electrochemical cell: Concentration of H+ is unknown, Pressure of H2 is constant at 1 atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+ half-cell acting as the cathode. a) write out the oxidization and reduction half reactions, and the overall chemical reaction occurring, and find the initial pH in the H+ | H2 | Pt cell b) What is the equilibrium constant of the reaction happening in the cell? Tl(s) | Tl*(aq, 0.50 mol...
could someone please answer and explain the questions please!! #’s 7,8,9,13,14,17,18,19,20 please and thank you What is the oxidation number for the underlined manganese (A)1 (B)2 (C)4(D)(E)7 When balancing the below half-reaction in 8. Which of the following is true concerning a 1. vanic cc A) Oxidation occurs at the cathode and is (B) Oxidation occurs at the anode and is where anions move towards 2. acidic sol electrons are added to ution, where anions move towards side of.the.cquation. where...