Question

use the appropriate standard reduction potentials to determine the equlibrium constant at 200.00 K for the...

use the appropriate standard reduction potentials to determine the equlibrium constant at 200.00 K for the following reaction under acidic conditions:


4H+(aq) + MnO2(s) + 2F2+(aq) ------> Mn2+(aq) + 2Fe3+(aq) + 2H2O(l)

Homework Answers

Answer #1

The half reaction of reduction in the process is: MnO2 + 4H+ + 2e- --> Mn2+ + 2H2O; Eº=1.23V

The half reaction of oxidation in the process is: Fe3+ + 1e- --> Fe2+; Eº= 0.77V

In order to form the full reaction we must subtract twice the latter half reaction, so that the stechiometric coefficients match:

Reaction 1: MnO2 + 4H+ + 2e- --> Mn2+ + 2H2O. This reaction has a DGº1

Reaction 2: 2Fe2+ --> 2Fe3+ + 2e-. This reaction has a -2DGº2

Condensated Reaction: MnO2 + 4H+ + 2Fe2+ --> Mn2+ + 2H2O + 2Fe3+. This reaction has a DGº3.

Therefore, we can express DGº3 as DGº1-2DGº2.

Now remember that DGº= -nFEº, and also DGº=-RT ln(Keq), so...

(-8.314J/mol)(200K) ln(Keq) = -2(96485C)(1.23V) - [-1(96485C)(0.77V)]

ln(Keq)= -163059.65 / (-8.314(200)) = 98.0632.

Keq= e^98.0632 = 3.876x1042.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the equilibrium constant for each of the reactions at 25 ?C. Standard Electrode Potentials at...
Calculate the equilibrium constant for each of the reactions at 25 ?C. Standard Electrode Potentials at 25 ?C Reduction Half-Reaction E?(V) Pb2+(aq)+2e? ?Pb(s) -0.13 Mg2+(aq)+2e? ?Mg(s) -2.37 Br2(l)+2e? ?2Br?(aq) 1.09 Cl2(g)+2e? ?2Cl?(aq) 1.36 MnO2(s)+4H+(aq)+2e? ?Mn2+(aq)+2H2O(l) 1.21 Cu2+(aq)+2e? ?Cu(s) 0.16 Part A: Pb2+(aq)+Mg(s)?Pb(s)+Mg2+(aq) Express your answer using three significant figures. Part B: Br2(l)+2Cl?(aq)?2Br?(aq)+Cl2(g) Express your answer using two significant figures. Part C: MnO2(s)+4H+(aq)+Cu(s)?Mn2+(aq)+2H2O(l)+Cu2+(aq) Express your answer using two significant figures.
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...
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
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...
Which species is the strongest oxidizing agent under standard conditions? Half-reaction Eo (V) MnO2(s) + 4H+...
Which species is the strongest oxidizing agent under standard conditions? Half-reaction Eo (V) MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l) 1.22 V SnO2(s) + 2H2O() + 4e– → Sn(s) + 4OH– (aq) -0.95 V Hg2SO4(s) + 2e– → 2Hg(l) + SO42 – (aq) +0.61 V Cr(OH)3(s) + 3e– → Cr(s) + 3OH– (aq) –1.48 V Mn2 2+ + 2e- ⇌ Mn2 -1.18 A. MnO2 B. Sn C. Hg2SO4 D. Cr E. Mn2 2+
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
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
1. Use standard reduction potentials to calculate the standard free energy change in kJ for the...
1. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 3I2(s) + 2Cr(s) -----> 6I-(aq) + 2Cr3+(aq) Answer: _______ kJ K for this reaction would be greater or less than one. 2. Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu2+(aq) + Sn(s) ----> 2Cu+(aq) + Sn2+(aq) Answer: ______ kJ K for this reaction would be greater or less than one.
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at...
Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) Standard Reduction (Electrode) Potentials at 25 oC Half-Cell Reaction Eo (volts) F2(g) + 2 e- 2 F-(aq) 2.87 Ce4+(aq) + e- Ce3+(aq) 1.61 MnO4-(aq) + 8 H+(aq) + 5 e- Mn2+(aq) + 4 H2O(l) 1.51 Cl2(g) + 2 e- 2 Cl-(aq) 1.36 Cr2O72-(aq) + 14 H+(aq) + 6 e- 2 Cr3+(aq) + 7 H2O(l) 1.33 O2(g) + 4 H+(aq) + 4 e- 2 H2O(l) 1.229 Br2(l) + 2 e-...
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