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5. A lead storage battery involves the following two half-reactions: PbSO4(s) + 2e → Pb(s) +...
The standard half-cell reactions of lead acid battery is: 2) ЕФN Half-cell reduction reaction form: red PbOo2.(s) 4H+ + so2 4, (aq) PbSO4,()+2H20 Red 2e 1.69 Рo) + So?- 4.(aq) -Ox -0.36 Pbs04.(s)2e Pb()PbO2,(s)+ 2H2SO4,(ag) 2P6SO4.(6) +2H20D 2.05 Tot. a) Determine the full cell reaction of lead acid batter and the total cell potential when discharging the battery b) The half-cell potentials are given according to a reference potential. Describe this reference potential. What is the point of a reference...
The standard half-cell reactions of lead acid battery is: 2) Half-cell reduction reaction form: red 1.69 +4Ht +so +2ePbSO4,()+2H2O) РЬОог.0) Red (aq) -Ox. PbSO4.()+2e Pb)+SO -0.36 4.(aq) Pb()+PbO2.(s)+2H2SO4.(ag) Tot. 2PBSO4.()+ 2H20() 2.05 a) Determine the full cell reaction of lead acid batter and the total cell potential when discharging the battery. I b) The half-cell potentials are given according to a reference potential. Describe this reference potential. What is the point of a reference potential?
You want to make a battery using the following reactions: PbO2 + 4H+ + SO42- + 2e ---> PbSO4(s) + 2H20 Ni2+ + 2e ---> Ni ° = +1.69 E° = -0.25 Which is being reduced? Which is being oxidized? Which is the anode? Which is the cathode? What is the formula to calculate Eºcell? What is Eºcell?
The spontaneous galvanic cell of a lead storage battery (a typical car battery) is composed of the following reduction half reactions reduced 1.69 v Pb02 (s)+ HSO, (aq)+3 Ha0 (aq) + 2 e Pbs04 (s)+5 H20) PbSO4 (s) + H3O (aq) 2 e Pb (s)+HSO (aq)+ H20 (I) E reduced 0.36 V How much current (in A) does a cell phone charger for your car use if your car dies after 14 hours of leaving the phone plugged in without...
Question 22 (5 points) Given the following half reactions: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = 1.69V PbO2 + 4H+ + 2e- → Pb2+ + 2H2O E° = 1 .46V Calculate the Ksp for PbSO4 at 25 degrees C. Please enter your answer in scientific notation, such as 1.2E10 or 1.2E-10 and keep two significant figures.
What mass of lead sulfate (PbSO4) is formed in a lead-acid storage battery when 1.00 g of Pb undergoes oxidation? Hint: Lead-Acid batter cell: Pb(s) + PbO2(s) + 2 H2SO4(aq) – 2 PbSO4(s) + 2 H2 O(1) Hint #2: Convert grams to moles and then moles back into grams.
Problem 2 (chapter 18.3, 2 points): The lead-acid battery is commonly used in cars. One electrode is a lead grid filled with spongy lead Pb(s). The other electrode is a lead grid filled with spongy lead oxide PbO2(s). The net reaction that occurs is: Pb(s)+PbO (s+2H(aq) 2HSO (aq) ->2PbSO4(s2H 0(0) a) Write down the half reactions that occur at each electrode. b) Identify the oxidation state of Pb in each of the species: Pb(s), PbO2(s) and PbSO4(s). Explain. c) Identify...
Question 10 0.5 pts What mass of lead sulfate (PbSO4) is formed in a lead-acid storage battery when 1.00 g of Pb undergoes oxidation? Hint: Lead-Acid batter cell: Pb(s) + PbO2(s) + 2 H2SO4(aq) → 2 PbSO4(s) + 2 H2O(1) Hint #2: Convert grams to moles and then moles back into grams. Mass of PbSO4 formed = 0.007 grams Mass of PbSO4 formed = 0.275 grams Mass of PbSO4 formed = 1.225 grams Mass of PbSO4 formed = 2.275 grams...
Use the following lead-acid battery cell to answer the related questions: PbO2 (s) │PbSO4 (s) │H2SO4 (aq) (1 M) ‖ H2SO4 (aq) (1 M)│Pb (s) │PbSO4 (s) A. (5 pts) Determine the Cell potential for the battery at 25°C B. (5 pts) A high output alternator for a KIA soul can produce 220 Amp current. How long would it take to recharge/reform 4.03 kg of Pb at that rate (assuming your battery is near dead)?
Question 20 (5 points) Using the following standard reduction potentials: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = +1.69 V PbO2 + 4H+ + 2e → Pb2+ + 2H20 E° = +1.46 V The standard cell voltage for the reaction PbSO4(s) Pb2+ + SO42- is V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.