Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials.4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4H+Fe3+ + e-= Fe²+E° = 0.771 V0, + 2 H* + 2 e¯2 H,0E° = 1.229 VE° =VK =Is the overall reaction spontaneous as written?AG° =spontaneousnot spontaneous

Answered: Image /qna-images/answer/e4886b26-8e0e-4868-a6ad-78d76f15ae27.jpg

Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4Ht Fe3+ + e-= Fe2+ E° = 0.771 V 0, + 2H* + 2e H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneof as written? AG° = spontaneous not spontaneous

Determine E°, AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fe3+ + 2 H,0 4 Fe²+ + O, + 4Ht Fe3+ + e-= Fe2+ E° = 0.771 V 0, + 2H* + 2e H,0 E° = 1.229 V E° = V K = Is the overall reaction spontaneof as written? AG° = spontaneous not spontaneous

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...

See similar textbooks

Similar questions

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 2 K(s) + I2 (s) --> 2K+(aq) + 2 I-(aq) K+(aq)+e- ---> K(s) E°= -2.93 V I2(s)+2 e- ---> 2I-(aq) E°= +0.54 V +5.32 V -5.32 V +1.85 V +3.47 V +6.40 V
Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1 atm) || X3+(1 M) | X(s) If the standard cell emf is minus3.26 V, what is the standard reduction potential at 25oC for X3+ + 3e- → X(s) -3.26 V 3.26 V 1.36 V 1.90 V -1.90 V
For a galvanic cell, given the following 2C1O3 +12H + 10e Cl₂ + 6H₂O S2082 +2e2SO4²- half-reactions and their standard reduction potentials: E°= +1.47 volt S E° +1.96 volt Calculate the value of the equilibrium constant, K.
What is the expected standard cell potential for the following unbalanced reaction under basic conditions? MnO4-(aq) + Fe+2(aq) ----> Fe+3 (aq) + MnO2(s) Given: Fe3+ + e- ----> Fe2+ E1/2 = 0.771 VMnO4-+ 2 H2O + 3e- ----> MnO2 + 4OH- E1/2 = 0.558 V
a) Balance the following reactions. b) Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. c) Identify the reactions with K > 1 among the following redox reactions. d) Write the line representations for the Galvanic cells, indicating the anode and cathode. Cl2 + Br- --> Cl- + Br2 MnO4- + H+ + Ce3+ --> Ce4+ + Mn2+ + H2O Pb2+ -->Pb + Pb4+ NO3- + H+ + Zn --> Zn2+ + NO2 + H2O
What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal place. Cu(s) + 2Ag (aq) ⇒ Cu²+ (aq) + 2 Ag (s) Note: Reference the Standard reduction potentials at 25 °C table for additional information. K = x10 X S
4. The cell diagram for an electrochemical cell is given below: Mn(s) | Mn* (aq, 1.0 mol dm) || Ag* (aq, 1.0 mol dm)|Ag (s) In the above cell, the standard electrode potential of the silver hal f-cell is =0.80 V. E°cell = +1.98 V Write the equation for the reaction occurring at the anode and cathode. Write the overall cell equation Determine the standard electrode potential of the Mn2*/Mn half-cell What is the strongest oxidizing agent in the above cell? What is the strongest reducing agent in the above cell? a) 1) ii) b) i) i1) c) After the cell was used, the change in mass of the silver electrode was found to be 5.40 IS g Caleulate the change in mass of the manganese electrode.
Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V
The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
For the galvanic cell: Zn(s) + 2Tl+(aq) 2Tl(s) + Zn2+(aq) Eocell = 0.42 V The standard reduction potential for the half cell Zn2+(aq) + 2e– Zn(s) is Eored = –0.76 V What is the standard reduction potential for Tl+(aq) + e– Tl(s) Eored = ? V a. +0.17 V b. –0.17 V c. –0.34 V d. +0.34 V
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V