Use the following data to answer the question: 1) Mg2+(aq) + 2e- --> Mg(s) E0 = -2.38v 2) Zn2+(aq) + 2e- --> Zn(s) E0 = -0.76v 3) Fe2+(aq) + 2e- --> Fe(s) E0 = -0.44v For an electrochemical cell made from reactions 1 & 2, what would be true? a. Zn(s) will be the anode b. Zn2+ would be reduced c. Mg(s) will be reduced d. Mg2+ would be reduced
Use the following data to answer the question: 1) Mg2+(aq) + 2e- --> Mg(s) E0 =...
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);...
Reaction Eo Ag+(aq)+ e-→ Ag(s) 0.80V Zn2+(aq)+ 2e-→Zn(s) -0.76V What would be the cathode reactant in the Voltaic Cell made from the half-reactions above? Question options: a. Zn2+(aq) b. Ag+(aq) c. Ag(s) d. Zn(s)
9) A sol'n in an electrolytic cell contains the ions Cu2+, Fe2+ & Zn2+. If the voltage (initially very low) is turned up, in which order will the metals be plated out onto the cathode? Cu2+(aq)2e-Cu(s); E0.34V Fe"(aq) + 2e-→ Fe(s);E"--0.44V Zn2+(aq) + 2e-→ Zn(s): E。--0.76V 10) How long will it take to produce a sol'n of pH 2.00 by electrolysis of 500 mL of 0.100 M AgN03(aq) at 0.240 Amperes? Anode: 2H2O(l) → 4H-(aq) + O2(g) + 4e-, E°...
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
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Express your answer to three significant figures and in units of kJ/mol. Consider constructing a voltaic cell with one compartment containing a Zn(s) electrode immersed in a Zn2+ aqueous solution and the other compartment containing an Al(s) electrode immersed in an Al3+ aqueous solution. What is the spontaneous reaction in this cell? Group of answer choices Zn + Al3+ → Al...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 59 ∘C , where [Fe2+]=3.10mol L−1 and [Mg2+]=0.210mol L−1 . a) What is the value for the reaction quotient, Q, for the cell? b) What is the value for the temperature, T, in kelvins? c) What is the value for n? d) Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential. Using the table of theoretical values and what you know of the metals to fill in the blanks below. When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2+ + 2e - → Fe would be entered as: Fe^2+ + 2e. → Fe Galvanic Cell Consisting of: Zn²+ + 2e -...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.50 M and [Mg2+]= 0.310 M . A. What is the value for the reaction quotient, Q, for the cell? B. What is the value for the temperature, T, in kelvins? C. What is the value for n? D. Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 87 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M . A) What is the value for the reaction quotient, Q for the cell? B)What is the value for Temperature, T in Kelvins? C)What is the value for n? D) Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) (3 Significant Figures)