HomeworkLib
Question

3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+...

3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+ = +0.771V, Eo Ce4+/Ce3+ = + 1.44V

a) Draw the complete cell represented by the above line diagram and label all the components.

b) Write the half-cell reactions and complete redox reaction of the cell.

c) Calculate the standard cell potential.

d) Calculate the cell potential at the non-standard conditions provided above.

e) Was the cell reaction spontaneous?

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

E cell = +ve > Spenatenores E cell = -ve Ron Spontaneous Switch ANODE voltmeter Nat NO3- Cathod Pt Salt bridge feat fe3tte:fe2+ + Cett (0.025m Co.035m) fe3+ + Cest 0.25m) co-osomy Ray Ecell = Ecel -0.0591 log Qc cell = t cell Ecell = Fielu - 0.0591thank you very much.hope this will help you,good luck

0 0
Add a comment
Know the answer?
Add Answer to:
3. For the cell represented by Pt|Fe3+(0.25 M), Fe2+(0.025 M)||Ce4+(0.035 M), Ce3+(0.050 M)|Pt E o (Fe3+/Fe2+...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential...

    Consider the cell Pt(s)|H2(g,1atm)|H+(aq,a=1)|Fe3+(aq),Fe2+(aq)|Pt(s) given that Fe3++e−⇌Fe2+ and E∘=0.771V at 298.15 K. If the cell potential is 0.683 V, what is the ratio of Fe2+(aq) to Fe3+(aq)? What is the ratio of these concentrations if the cell potential is 0.807 V?

  • A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the fo...

    A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the formation of Fe3+ and Ce3+. A Pt indicator electrode and a saturated calomel electrode are used to monitor the titration. Write the balanced titration reaction titration reaction:> Complete the two half-reactions that occur at the Pt indicator electrode. Write the half-reactions as reductions half-reaction: Ce e half-reaction: Fe e- E 0.767 V Select the two equations that can be...

  • For the following cell:                      Zn | Zn2+ (1.0 M) || Fe3+ (1.0 M), Fe2+ (1.0...

    For the following cell:                      Zn | Zn2+ (1.0 M) || Fe3+ (1.0 M), Fe2+ (1.0 M) | Pt Write the half-reactions and the balanced net reaction for the cell. Identify which species is oxidized. Which is reduced? Which is the reducing reagent? Oxidizing reagent? Draw the electrochemical cell. Label the anode and cathode. Indicate the direction of electron and ion flow. Calculate the standard cell potential. Is the reaction spontaneous?

  • Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77...

    Using the following standard reduction potentials: Fe3+ (aq) + e. → Fe2+ (aq) Eo = +0.77 V Pb2+ (aq) + 2 e. → Pb(s) E。--0.13 V Calculate the standard cell potential for the galvanie cell reaction given below, and determine whether or not this reaction is spostaneous under standard conditions. Pb2+ (aq) + 2 Fe2+ (aq) → 2 Fe3+ (aq) + Pb(s) ⓔ A. E.-0.90 V, nonspontaneous OB. E-0.90 V, spontaneous C. Eo +0.90 V, nonspontaneous OD0.90 V, spontaneous

  • What is the cell potential for the following reaction when [Fe2+] = 0.25 M and [Fe3+]...

    What is the cell potential for the following reaction when [Fe2+] = 0.25 M and [Fe3+] = 0.01 M? You may use the standard reduction potentials on your data sheet. Fe(s) + 2 Fe3+(aq) → 3 Fe2+(aq)

  • Using the following standard reduction potentials Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq)...

    Using the following standard reduction potentials Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 V calculate the standard cell potential for the galvanic cell reaction given below, and determine whether or not this reaction is spontaneous under standard conditions. Pb2+(aq) + 2 Fe2+(aq) → 2 Fe3+(aq) + Pb(s) Group of answer choices E° = -0.90 V, spontaneous E° = -0.90 V, nonspontaneous E° = +0.90 V, nonspontaneous E° = +0.90...

  • Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the...

    Consider the following cell: Pt(s) | Fe3+ (aq). Fe2(aq) | CIF (aq) C12(e) Pt(s) If the standard reduction potentials of the Fe3+/Fe2+ and Cl2/Cl" couples are +0.77 and +1.36 V, respectively, calculate the value of Efor the given cell. +1.00 V O +1.77 v +0.59 V +2.13 V +0.95 V

  • Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) |...

    Consider the following electrochemical cell: Pt | Cu2+ (aq) | Cu+ (aq) || Fe2+ (aq) | Fe3+ (aq)| Pt The cell is constructed by preparing one half-cell with a solution containing 8.33 * 10-3 M FeCl3 and 1.67*10-2 M FeCl2, and preparing the other half-cell with a solution containing 8.33*10-3 M CuCl2 and 0.025 M CuCl. Calculate the cell potential once the half-cells are connected to each other. E°(Cu2+/Cu+) = 0.16 V; E°(Fe2+/Fe3+) = 0.77 V

  • 7.50 Consider the following cell. Pt Cu2+, Cu+ Fe2+, Fe3+ | Pt (a) What is the cell reaction? (b) What is the standard...

    7.50 Consider the following cell. Pt Cu2+, Cu+ Fe2+, Fe3+ | Pt (a) What is the cell reaction? (b) What is the standard electro- motive force of the cell at 298.15 K? (c) Calculate Ar Gº for the cell reaction from the standard electromotive force. (d) Calcu- late ArGº for the cell reaction using the AfGº values for the ions in Table C.2. (e) Calculate ArGº for the cell reaction using the AfHº values and Sº values in Table C.2.

  • 4. Calculate the cell potential for the half cells Fe3+/Fe2+ and MnO4- /Mn2+, where the Mn...

    4. Calculate the cell potential for the half cells Fe3+/Fe2+ and MnO4- /Mn2+, where the Mn process occurs at the cathode, under the following conditions and predict whether the reaction is spontaneous: [Fe3+] = 1.0 M, [Fe2+] = 0.1 M, [MnO4 - ] = 0.01 M [Mn2+] = 1 x 10-4 M [H+ ] = 1 x 10-3 M Fe3+ + e− → Fe2+ +0.700 V MnO4 − (aq) + 8 H+ (aq)+ 5e− → Mn2+ (aq) + 4 H2O(l)...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT