Question

The reactions redox Fe3+(aq) + V2+ = Fe2+aq + V3+ aq a) what is the oxidizing...

The reactions redox Fe3+(aq) + V2+ = Fe2+aq + V3+ aq

a) what is the oxidizing agent and rducing agent? Justify ur answer

b) Calculate the standard potential? This reaction is it possible?

Homework Answers

Answer #1

reaction :

Fe+3 (aq) + V2+ (aq)   ---------------->. Fe+2 (aq) + V3+ (aq)

Oxidation : V2+ (aq)   ---------------> V3+ (aq) + e-

Reduction : Fe+3 (aq) + e- ------------> Fe+2 (aq)

here V2+ oxidized and Fe+3 reduced .

a)

Oxidizing agent : Fe+3

Reducing agent : V2+

the element which is being oxidized is called reducing agent . the element which is being reduced is called oxidizing agent.

b)

Eocell = Eored - Eooxidation

         = 0.771 - (- 0.26)

Eocell = 1.03 V

yes , this is possible.

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
Balance each of the following RedOx reactions occurring in acidic conditions: Fe2+(aq) + MnO41-(aq) → Fe3+(aq)...
Balance each of the following RedOx reactions occurring in acidic conditions: Fe2+(aq) + MnO41-(aq) → Fe3+(aq) + Mn2+(aq) Br2(l) + SO2(g) → Br1-(aq) + SO42-(aq) Cu(s) + NO31-(aq) → Cu2+(aq) + NO2(g) HgS(s) + Cl1-(aq) + NO31-(aq) → HgCl42-(aq) + NO2(g) + S(s) Cl2(g) → ClO31-(aq) + Cl1-(aq)
Which of the following is the correct cell diagram for the reaction: 2 Fe2+(aq) + Cl2...
Which of the following is the correct cell diagram for the reaction: 2 Fe2+(aq) + Cl2 (g)  ??> 2 Fe3+(aq) + 2 Cl–(aq) Fe3+(1.0M) | Fe2+(1.0M) || Cl2(g) | Cl–(1.0M) Fe(s) | Fe3+(1.0M), Fe2+(1.0M) || Cl2(g) | Cl–(1.0M) | Pt(s) Pt(s) , Fe3+(1.0M), Fe2+(1.0M) || Cl2(g), Cl–(1.0M) | Pt(s) Fe(s) | Fe3+(1.0M) | Fe2+(1.0M) || Cl2(g) | Cl–(1.0M) | Pt(s) Pt(s) | Fe2+(1.0M), Fe3+(1.0M) || Cl2(g) | Cl–(1.0M) | Pt(s) --------------- Based on the following standard reduction potentials: Fe3+ + 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
Balance these equations for redox reactions occurring in acidic solution. VO43−+Fe2+→VO2++Fe3+ Balance these equations for redox...
Balance these equations for redox reactions occurring in acidic solution. VO43−+Fe2+→VO2++Fe3+ Balance these equations for redox reactions in basic solution. MnO2(s)+ClO3−→MnO4−+Cl−
For each of the following redox reactions in the, identify the oxidizing agent and the reducing...
For each of the following redox reactions in the, identify the oxidizing agent and the reducing agent. 2Na(aq)+2H2O(l)→2NaOH(aq)+H2(g) C(s)+O2(g)→CO2(g) 2MnO−4(aq)+5SO2(g)+2H2O(l)→2Mn2+(aq)+5SO2−4(aq)+4H+(aq)
For a single galvanic cell based on the (unbalanced) reaction: IO3-(aq) + Fe2+(aq) = Fe3+(aq) +...
For a single galvanic cell based on the (unbalanced) reaction: IO3-(aq) + Fe2+(aq) = Fe3+(aq) + I2(s) What is the cell potential when the cell reaches equilibrium?
Specify which of the following are redox reactions and identify the oxidizing agent, the reducing agent,...
Specify which of the following are redox reactions and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a) Ba(s) + MgCl2(aq) --> Mg(s) + BaCl2(aq) b) HNO3(aq) + NH4OH(aq) --> NH4NO3(aq) + H2O(l) c) SiCl4(l) + 2Ca(s) --> 2CaCl2(s) + Si(s) d) 2Cr(s) + 6HCl(aq) --> 2CrCl3(s) + 3H2(g)
When benzene dissolves in water, it can be degraded by various bacteria species through redox reactions...
When benzene dissolves in water, it can be degraded by various bacteria species through redox reactions depending on which oxidizing agents answer the following questions: a. Draw the analogies between benzene degradation by bacteria and organic matter degradation by bacteria discussed in class. Under what conditions is benzene most effectively degraded by bacteria? It is given that the standard free energy change ΔG0 is related to redox potential E0 by the equation ΔG0=-nFEo, where n is the number of electrons...
(a)Two of the reactions in the “Copper Cycle” are classified as oxidation-reduction (“’redox”) reactions. Identify the...
(a)Two of the reactions in the “Copper Cycle” are classified as oxidation-reduction (“’redox”) reactions. Identify the two reactions, and identify the oxidizing agent and the reducing agent in each. (b)Which one of the redox reactions above can be classified as a single displacement reaction? (c)One of the reactions in this experiment is classified as a decomposition reaction. Identify it: (d)One of the reactions in this experiment is classified as a precipitation reaction. Identify it: (e)One of the reactions in this...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction:...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq), given that [Fe3+]=0.05 and [[Cu2+]=0.125M at 25°C, and Fe3++e→Fe2+             E0=0.77 V Cu2+2e→Cu                   E0=0.34 V 4b. Use the information provided in question 4a to calculate the change in free energy (ΔG) and change in entropy (ΔS) for the redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq) What do the ΔG and ΔS values indicate about the spontaneity of the redox reaction?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT