To calculate the r of the given reaction,
Lead (II) sulfate reacts with water in the following reaction: 2PbSO4(s) + 2H2O(l) -> Pb(s) +...
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 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. 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 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 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:...
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?
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.
Consider the reaction. Pb(SO4)2+2Zn⟶2ZnSO4+Pb If 0.162 mol of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?
Consider the reaction. Pb(SO4)2+2Zn⟶2ZnSO4+Pb If 0.340 mol of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction? mass: g ZnSO4