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
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
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
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
The following reaction is non-spontaneous as written when the components are in their standard states, the cell potential is -0.16 V. Which of the following is true? Co(s) + Fe²*(aq) 2 Co²* (aq) + Fe(s) E =-0.16 V A. the reaction is spontaneous if [Co2+/[Fe2+] > 3.91x10-6 В. the reaction is spontaneous if [Co2+]/[Fe2+] -6 C. the reaction is spontaneous if [Co2+/[Fe2*] > 2.56x105 D. the reaction is spontaneous if [Co2*]/[Fe2+] 5