Question

Consider the cell: Hg(l) ׀ Hg2SO4(s) ׀ FeSO4(aq) ׀ Fe(s) The standard cell potential (E θ...

Consider the cell: Hg(l) ׀ Hg2SO4(s) ׀ FeSO4(aq) ׀ Fe(s) The standard cell potential (E θ ) for the reduction of Fe2+ is -0.447 V and the standard cell potential for the reduction of Hg2SO4(s) is +0.6125 V.

(a) Write the cell reaction.

(b) If the activity of FeSO4(aq) is 0.0100, calculate the cell potential and the standard Gibbs energy at 25°C.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2...
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2 ] = 0.837 M and [Fe2 ] = 0.0100 M. Standard reduction potentials can be found here. Zn(s)+Fe^2+(aq) <--->Zn^2+(aq)+Fe(s) E= _______ 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
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.210 M...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.210 M . Part A What is the value for the reaction quotient, Q, for the cell? Part B What is the value for the temperature, T, in kelvins? Part C What is the value for n? Part D Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) Part E For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]=...
± Cell Potential and Free Energy Free-energy change, ΔG∘, is related to cell potential, E∘, by...
± Cell Potential and Free Energy Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation ΔG∘=−nFE∘ where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts, ΔG∘ must be in joules since 1 J=1 C⋅V. Part A Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) Express your answer to three significant figures and include the appropriate units. Part B...
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
Consider the following half-reactions: Ag+ (aq) + e- --> Ag(s) E cell = 0.80 VV Cu2+(aq)...
Consider the following half-reactions: Ag+ (aq) + e- --> Ag(s) E cell = 0.80 VV Cu2+(aq) + 2e- --> Cu(s) E cell = 0.34 V Pb2+(aq) + 2e- --> Pb(s) E cell = -0.13 V Fe2+(aq) + 2e- --> Fe(s) E cell = -0.44 V Al3+ (aq) + 3e- --> Al(s) E cell = -1.66 V Which of the above metals or metal ions will oxidize Pb(s)? a. Ag+(aq) and Cu2_(aq) b. Ag(s) and Cu(s) c. Fe2+(aq) and Al3+(aq) d....
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 65 ∘C , where [Fe2+]= 3.40 M and [Mg2+]= 0.110 M...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 65 ∘C , where [Fe2+]= 3.40 M and [Mg2+]= 0.110 M . Part A What is the value for the reaction quotient, Q, for the cell? Part B What is the value for the temperature, T, in kelvins? Part C What is the value for n? Part D Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
What is the standard free energy change and equilibrium constant for the following reaction at 25...
What is the standard free energy change and equilibrium constant for the following reaction at 25 °C? 2Ag+ (aq) + Fe (s)   2 Ag (s) + Fe2+ (aq) Given standard electrode potentials: Ag+ (aq) + e-    Ag (s) E0 = 0.7996 V Fe2+ (aq) + 2 e-    Fe (s) E0 = - 0.447 V
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) -->...
Calculate the equilibrium constant, K, for the following reaction at 25 °C. Fe^3+(aq)+B(s) + 6H2O(l) --> Fe(s) + H3BO3(s) + 3H3O+(aq) The balanced reduction half-reactions for the above equation and their respective standard reduction potential values (E°) are as follows: Fe3+(aq) + 3e- --> Fe (s)... E=-0.04V H3BO3(s) + 3H3O+(aq) + 3e- ---> B(s)+6H20 (l).....E=-0.8698 K=?
1) Fe2+(aq) + 2 Al(s) <==> 2 Al3+(aq) + 3 Fe(s). What is the voltage for...
1) Fe2+(aq) + 2 Al(s) <==> 2 Al3+(aq) + 3 Fe(s). What is the voltage for this cell? 2) What is the Gibbs Free Energy for the above reaction assuming standard conditions? 3. What is the Gibbs Free Energy for the cell in question 1 if the Fe2+ (aq) is [.15] and Al3+ (aq) is [3.80]? 4. Describe what happens within the salt bridge between the two cells. Please show work
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT