Question

3) The corrosion of iron is an electrochemical process that involves the standard reduction potentials given...

3) The corrosion of iron is an electrochemical process that involves the standard reduction potentials given here at 25 °C. Fe2+(aq) + 2e– → Fe(s) E° = –0.44 V O2(g) + 4H+ (aq) + 4e– → 2H2O(l) E° = +1.23 V

a. Calculate the voltage for the standard cell based on the corrosion reaction. 2Fe(s) + O2(g) + 4H+ (aq) → 2Fe2+(aq) + 2H2O(l)

b. Calculate the voltage if the reaction in Part a occurs at pH = 4.00 but all other concentrations are maintained as they were in the standard cell.

c. For the reaction Fe(OH)2(s) + 2e– → Fe(s) + 2OH– (aq), E° = –0.88 V. Use this information with one of the given standard potentials in Appendix ** to calculate the Ksp of Fe(OH)2.

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Solution :

All the best buddy please upvote it

0 0
Know the answer?
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
Similar Questions
For the following reactions and given standard reduction potentials O2(g) + 4H+(aq) + 2Cu(s)  2Cu2+(aq)...
For the following reactions and given standard reduction potentials O2(g) + 4H+(aq) + 2Cu(s)  2Cu2+(aq) + 2H2O(l) O2(g) + 4H+(aq) + 4e-  2H2O(l)       E° = 1.23 V Cu2+ + 2e-  Cu(s)    E° = 0.34 V a. Calculate E°cell b. Calculate ΔG° at 254 K
Use the standard reduction potentials to determine what is observed at the cathode during the electrolysis...
Use the standard reduction potentials to determine what is observed at the cathode during the electrolysis of a 1.0 M solution of KBr that contains phenolphthalein. What observation(s) is(are) made? O2 (g) + 4H+ (aq) + 4e- --> 2H2O (l) E°​ = 1.23 V Br2 (l) + 2e- --> 2Br​- (aq) E°​ = 1.07 V 2H2O (l) + 2e- --> H2 (g) + 2OH​- E° = -0.80 V K+ (aq) + e- --> K(s) E°​ = -2.92 V (A) Solid...
The process of corrosion can be viewed as an electrochemical cell with cathodic reactions such as:...
The process of corrosion can be viewed as an electrochemical cell with cathodic reactions such as: O2+2H2O+4e−⟶4OH− at +1.229 V H++e−⟶1/2H2(g) at 0 V M2++2e−⟶M(s) Where M is a metal. If this is the case, and we assume iron serves as the anode, Fe0(s)⟶Fe+2(aq)+2e− at −0.447 V what must be true of the cathode reactions for corrosion to occur? a. The standard reduction potential of the cathode must be less than 0 V. b.  The standard reduction potential of the cathode...
Constants Fe2+ + 2e− = Fe(s) E º =−0.44 V; O + 4H+ + 4e− 2H2O...
Constants Fe2+ + 2e− = Fe(s) E º =−0.44 V; O + 4H+ + 4e− 2H2O E º =−1.23 V 2)In acid solution, the half cells Fe2+(aq) | Fe(s) and O2(g) | H2O are linked to create a spontaneous, galvanic cell. a) Calculate Eºcell _____________ b) Which reaction occurs at the cathode _______________________________ c) Write the overall reaction for the cell ___________________________________ d) Write the shorthand notation for the anode (anode || cathode).
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard...
Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction: Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s) Fe2+(aq)+2e−→Fe(s) −0.45 Ni2+(aq)+2e−→Ni(s) −0.26
Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses...
Use standard reduction potentials (shown below) to calculate the potential of a nickel-cadmium cell that uses a basic electrolyte that has a 3.2 M hydroxide concentration. Cd(OH)2(s) + 2e- → Cd(s) + 2OH-(aq) Eº = -0.83 V NiO(OH)s) + H2O(l) + e- → Ni(OH)2(s) + OH-(aq) Eº = 0.52 V
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s) Standard Reduction Potentials...
Part A Calculate the equilibrium constant at 25 ∘C for the reaction Fe(s)+2Ag+(aq)→Fe2+(aq)+2Ag(s) Standard Reduction Potentials at 25 ∘C Fe2+(aq)+2e−→Fe(s) E∘= −0.45 V Ag+(aq)+e−→Ag(s) E∘= 0.80 V
Using the following standard reduction potentials, Fe3+(aq) + e- --> Fe2+ (aq) E = + 0.77...
Using the following standard reduction potentials, Fe3+(aq) + e- --> Fe2+ (aq) E = + 0.77 V Ni2+ (aq) + 2e- (aq) --> Ni(s) E = - 0.26 V Calculate the standard cell potential for the galvanic cell reaction given below and determine weather or not if the reaction is spontaneous under standard conditions. Ni2+ (aq) + 2 Fe2+ (aq) --> 2 Fe3+ (aq) + Ni(s)   SHOW ALL WORK
Corrosion is the electrolytic oxidation of metals by air, the half equation for the rusting of...
Corrosion is the electrolytic oxidation of metals by air, the half equation for the rusting of iron is shown below: 1/2 O2 (g) + H2O (l) + 2e- --> 2OH- (aq) Eo = 0.40V Fe2+ (aq) + 2e ---> Fe (s) Eo = -0.44V Write the overall equation for the rusting process and calculate the emf of this reaction under standard conditions. Standard conditions arent normally found in the environment, where the pressure of O2 (g) is 0.2 atm, pH...
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual...
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual Half-Cell Potentials Cell Reactions5 ΔG (kJ)6 (Cu) Electrode Standard Potential (V)2 Metal Electrode Experimental Potential (V)3 Metal Electrode Theoretical Potential (V)4 Metal Electrode Potential % Error Cu | Sn 0.469 0.34 V 0.34-0.469 =-0.129 Cathode:       Cu2+ + 2e- -> Cu Anode:            Sn ->Sn2++ 2e- Net:          Cu2+ + Sn -> Cu + Sn2+ Cu | Al 0.796 0.34 V 0.34-0.796 =-0.456 Cathode:   Cu2+ +...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT