The standard half-cell reactions of lead acid battery is: 2) Half-cell reduction reaction form: red 1.69...
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...
5. A lead storage battery involves the following two half-reactions: PbSO4(s) + 2e → Pb(s) + SO42- (aq); E = -0.36 V PbO2(s) + 4H*(aq) + SO42 (aq) + 2e → PbSO4(s) + 2H2O(1); E° = 1.69 V In the lead battery during the discharge reaction: A) PbSO4 is the cathode. B) PbSO4 is the anode. C) Pb is the anode. D) PbO, is the anode. E) H2SO4 is the cathode.
18. Identify the oxidant and reductant of the following reaction in a lead-acid battery. Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l)
A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted to lead(II). This reaction is facilitated by the presence of sulfuric acid, H2SO4, as shown by the reaction Pb+PbO2+2H2SO4→2PbSO4+2H2O. Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 2.80 A of current is drawn from the battery for 5.50 hours ?
A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted to lead(II). This reaction is facilitated by the presence of sulfuric acid, H2SO4, as shown by the reaction Pb+PbO2+2H2SO4→2PbSO4+2H2O PART A Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 3.90 A of current is drawn from the battery for 6.00 hours ?
A lead-acid battery uses a redox reaction in whichlead(0) and lead(IV) are both converted to lead(II). This reaction is facilitated by the presence of sulfuric acid, H2SO4, as shown by the reaction Pb+PbO2+2H2SO4→2PbSO4+2H2O Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 4.00 A of current is drawn from the battery for 5.50 hours ?
A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted to lead(II). This reaction is facilitated by the presence of sulfuric acid, H2SO4, as shown by the reaction Pb+PbO2+2H2SO4→2PbSO4+2H2O Part A Suppose that a fully charged lead-acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 2.70 A of current is drawn from the battery for 5.00 hours ? Express your answer with the appropriate...
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...
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...
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.