Question

The temperature dependence of the standard state cell potential for a lead storage battery is E°/...

The temperature dependence of the standard state cell potential for a lead storage battery is E°/ (V) = 2.1191 + 1.62 x 10^-4 [ T/ (°C) ] + 8.5x10^-7 [T/ (°C) ]^2 Calculate ∆rG0, ∆rS°,ΔrH°, ∆rCp0 at 25°C for the reaction Pb(s) + PbO2(s) + 2H2SO4(aq) = 2PbSO4(s) + 2H2O(l)

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
The cell reaction for the lead-acid battery is as shown below: PbO2 (s) + Pb (s)...
The cell reaction for the lead-acid battery is as shown below: PbO2 (s) + Pb (s) + 2 H2SO4 (aq) -> 2 PbSO4 (s) + 2 H2O (l)             What will Ecell be for this reaction when [H2SO4] = 1.5 M?
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.
Using the reaction and the E∘ given below 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)      E∘=0.46 V what is the cell potential at...
Using the reaction and the E∘ given below 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g)      E∘=0.46 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]= 3.10×10−2M , [Co2+]= 0.732 M , and [Cl−]= 0.544 M and the pressure of Cl2 is PCl2= 9.80 atm ? 2)At 57.0 ∘C , what is the maximum value of Q needed to produce a non-negative E value for the reaction SO4^2−(aq)+4H+(aq)+2Br−(aq)⇌Br2(aq)+SO2(g)+2H2O(l) In other words, what is Q when E=0 at this temperature?
A concentration cell has both electrodes made of lead and is based on the following half-cell...
A concentration cell has both electrodes made of lead and is based on the following half-cell reaction. Pb2+(aq) + 2 e− → Pb(s) (a) If [Pb2+ ] = 2.20 M at the cathode and [Pb2+ ] = 0.00740 M at the anode, what is the cell potential of the concentration cell at 298.15 K? V (b) What is the cell potential of the cell when the concentration of Pb2+ ions is the same in the cathode and anode compartments? V
1) For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g). E∘=0.483 V what is the cell potential at 25 ∘C if...
1) 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+]= 0.685 M , [Co2+]= 0.417 M , and [Cl−]= 7.70×10−2M and the pressure of Cl2 is PCl2= 6.60 atm ? 2)Part A At 63.0 ∘C , what is the maximum value of the reaction quotient, Q , needed to produce a non-negative E value for the reaction SO42−(aq)+4H+(aq)+2Br−(aq)⇌Br2(aq)+SO2(g)+2H2O(l) In other words, what is Q when E=0 at this temperature?Express your answer...
Please show work Calculate the cell potential for the following reaction that takes place in an...
Please show work Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mn(s) ∣ Mn2+(aq, 1.28 M) ∥ Ag+(aq, 0.000837 M) ∣ Ag(s) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mn(s) Mn2+(aq, 1.28 M) Ag+(aq, 0.000837 M) Ag(s) 1.98 V 0.00 V 1.79 V -0.84 V -1.28 V
A) What is the calculated value of the cell potential at 298K for an electrochemical cell...
A) What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 8.15×10-4 atm, the Cl- concentration is 1.48M, and the Pb2+ concentration is 1.07M ? Cl2(g) + Pb(s) ---> 2Cl-(aq) + Pb2+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given:____ ( TRUE/FALSE ) B)What is the calculated value of the cell potential at 298K for an electrochemical cell with...
Calculate the standard cell potential for each of the electrochemical cells. Part A 2Ag+(aq)+Pb(s)?2Ag(s)+Pb2+(aq) Express your...
Calculate the standard cell potential for each of the electrochemical cells. Part A 2Ag+(aq)+Pb(s)?2Ag(s)+Pb2+(aq) Express your answer using two significant figures. Part B 2ClO2(g)+2I?(aq)?2ClO?2(aq)+I2(s) Express your answer using two significant figures. Part C O2(g)+4H+(aq)+2Zn(s)?2H2O(l)+2Zn2+(aq)
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.11 M )+2e− Red:...
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.11 M )+2e− Red: MnO−4(aq, 1.70 M )+4H+(aq, 2.6 M )+3e−→ MnO2(s)+2H2O(l) Part A Compute the cell potential at 25 ∘C. Please show all work. Thank you.
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.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT