QUESTION 31Calculate Ecell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.E° = 1.77 VH202(aq)+ 2H*(aq) + 2e = 2H20();Fe3+(aq) + e = Fe2*(aq);E° = 0.77 VOverall reaction:2FE3*(aq) + 2H20() – H202(aq) + 2H*(aq) + 2Fe2+(ag)E cell = +1.00 V, nonspontaneousE cell =-1.00 V, nonspontaneousE° cell = +1.00 V, nonspontaneousE cell =-1.00 V, spontaneous

Given, Overall cell reaction is : Calculate E0cell and also predict that, the reaction is…

Calculate E cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H202(aq) + 2H*(aq) + 2e¯ = 2H2O(); E° = 1.77 V Fe*(aq) + e = Fe2*(aq); E° = 0.77 V Overall reaction: 2Fe*(aq) + 2H20() → H202(aq) + 2H*(aq) + 2Fe²+(aq) E° cell = +1.00 V, nonspontaneous E cell =-1.00 V, nonspontaneous E cell = +1.00 V, nonspontaneous O E° cell =-1.00 V, spontaneous

Calculate E cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H202(aq) + 2H(aq) + 2e¯ = 2H2O(); E° = 1.77 V Fe(aq) + e = Fe2(aq); E° = 0.77 V Overall reaction: 2Fe(aq) + 2H20() → H202(aq) + 2H*(aq) + 2Fe²+(aq) E° cell = +1.00 V, nonspontaneous E cell =-1.00 V, nonspontaneous E cell = +1.00 V, nonspontaneous O E° cell =-1.00 V, 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

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
Decide whether or not each metal dissolves in 1 mol L-1 HIO3(aq). Standard Electrode Potentials at 25 °C Reduction Half-Reaction E° (V) Au3+ (aq) +3e → Au(s) 1.50 IO3 (aq)+6H+(aq) + 5e7 →12 (s) + 3H2O(1) 1.20 Ni²+(aq) + 2e → Ni(s) -0.23
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Given: Half cell reaction E (V) Ag+(aq) + e- ---> Ag(s) 0.80 Cu+2(aq) + 2 e- ---> Cu(s) 0.34 Zn+2(aq) + 2 e- ---> Zn(s) -0.76 Ni+2(aq) + 2 e- ---> Ni(s) -0.23 (a) Pick up two of the above listed half-cells to build a voltaic cell that would have a maximum overall cell potential. Write the overall reaction equation. (b) Draw a detailed cell diagram and indicate which electrode is anode and which is cathode, and indicate the (-) electrode and the (+) electrode.
A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | AI3+(aq) || Ni2*(aq) | Ni(s) Which of the following reactions occurs at the cathode? Al(s) Al3*(ag) + 3e- O Ni2*(aq) + 2e- Ni(s) Al3+(aq) + 3e Al(s) > Ni(s) Ni2*(aq) + 2e
Calculate the value of the equilibrium constant (K) at 25 °C for the following cell reaction: Sn(s) + Pb2+(aq) → Sn2+(aq) + Pb(s); E°cell = 0.014 V
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
Determine the redox reaction represented by the following cell notation. Al(s) 1 Al³+ (aq) // Fe³+ (aq) | Fe(s) // is the salt bridge Fe(s) + Al3+(aq) → Al(s) + Fe3+(aq) 2Fe(s) + Al3+(aq) → Al(s) + Fe3+(aq) Al(s) + Fe3+(aq) → Fe(s) + Al3+(aq) 3Al(s) + 2Fe3+(aq) → 2Fe(s) + 3A13+(aq) 2Al(s) + Fe3+(aq) → Fe(s) + 2A13+(aq)
What would be produced by an electrolytic cell involving the following half-reactions: Pb2+(aq) + 2e- → Pb(s) E° = -0.13 V2H+(aq) + 2e- → H2(g) E° = 0.00 V a)Pb2+(aq) and H+(aq) b)Pb2+(aq) only c)Pb2+(aq) and H2(g) d)Pb(s) only e)Pb(s) and H+(aq) f)H+(aq) only g)Pb(s) and H2(g)
Determine the cell potential of an electrochemical cell based on the following two half-reactions: Oxidation: Ni (s) ⟶⟶ Ni2+ (aq, 2.0 M) + 2e- Reduction: VO2+ (aq, 0.010 M) + 2H+ (aq, 1.0 M) + e- →→ VO2+ (aq, 2.0 M) + H2O (l)
The redox reaction below has a ΔG° value of 315. kJ. Determine the standard cell potential(E°cell) for this reaction. A2+(aq) + 2B2+(aq) → A4+(aq) + 2B+(aq) Given the reaction below, complete the line notation. Co(s) + Cu2+(aq) → Cu+(aq) + Co2+(aq)