Part EWhat is the cell potential for the reactionMg(s) + Fe (aq)→Mg (aq) ++Fe(s)at 45 °C when [Fe"] 3.00 M and (Mg"] 0.310 M.Express your answer to three significant figures and include the appropriate units.> View Available Hint(s)HAE 1.97VSubmitPrevious AnswersX Incorrect; Try Again; 5 attempts remainingYou may have used a version of the Nernst equation that is only valid at 298 K. Be sure that you are using thecorrect Kelvin temperature in the Nernst equation.You may need to review Conversion Between Celsius and Kelvin.Provide Feedback

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What is the cell potential for the reaction Mg(s) +Fe2 (aq)→Mg+ (aq) + Fe(s) at 45 °C when (Fe"]=3.00 M and Mg+] 0.310 M. Express your answer to three significant figures and include the appropriate units. > View Availlable Hint(s) 1.97 V

What is the cell potential for the reaction Mg(s) +Fe2 (aq)→Mg+ (aq) + Fe(s) at 45 °C when (Fe"]=3.00 M and Mg+] 0.310 M. Express your answer to three significant figures and include the appropriate units. > View Availlable Hint(s) 1.97 V

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following half-reactions: Half-reaction E° (V) Ag*(aq) + e" Co2*(aq) + 2e → Ag(s) 0.799V → Co(s) |-0.280V Zn2*(aq) + 2e → Zn(s) -0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Zn2*(aq) oxidize Ag(s) to Ag"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
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Part A If a voltaic cell is created between a Am"/Am electrode and a Fe*/Fe electrode, what species is being oxidized? O Am"(ag) O Fe(s) O Fe"(ag) O Am(s)
Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s)+Cu2+(aq)⟶Cu(s) +Zn2+(aq) Eocell=1.1032 V What is the cell potential for a cell with a 2.214 M solution of Zn2+(aq) and 0.1456 M solution of Cu2+(aq) at 437.7 K?
Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F*(aq) 2.870V Co2+*(aq) + 2e → Co(s) |-0.28OV 2+ Mg"(aq) + 2e → Mg(s) -2.37OV (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F2(g) to F"(aq)? (6) Which species can be reduced by Co(s)? If none, leave box blank.
Consider the following half-reactions: Half-reaction ° (V) Br2(1) + 2e → 2Br°(aq) |1.080V Sn²+ (aq) + 2e . Sn(s) |-0.140V Zn2*(aq) + 2e → Zn(s)|-0.763V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Br2(0) oxidize Zn(s) to Zn2*(aq)? (6) Which species can be oxidized by Sn2*(aq)? If none, leave box blank.
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)
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