The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application today, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H2SO4 (l) → SO3 (g) + H2O (l) ΔH=+113.kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb (s) + PbO2 (s) + 2SO3 (g) → 2PbSO4 (s) ΔH=−775.kJ Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ .
The lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859...
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...
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...
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)
5. The common lead-acid car battery produces a large burst of current, even at low temperatures, and is rechargeable. The reaction that occurs while recharging a "dead" battery is 2PbSO4(s)+2H20)Pb(s) + PbO(s) + 2H2SO40) Use AHoe values from the textbook to calculate AHon rxn
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...
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?