1. Balance the following reactions: a) PbO2 +Mn2+ =Pb2+ + MnO-4 (acidic medium) b) Ce4+ + AsO-2 =Ce3+ + AsO3-4 (basic medium) c) C2O2-4 +MnO-4 = Mn2+ +CO2 (acidic medium) d) CN- +MnO-4 = CNO- + MnO2 (acidic medium) e) CrO-2 + ClO- = CrO2-4 + Cl- ( basic medium)
For the following incomplete half reaction equation: PbO2(s) + 4 H+(aq) + SO42-(aq) → PbSO4(s) + 2 H2O (l) On which side should electron(s) be added to make it charge balanced (reactants or products)? How many electrons should be added? (write a number) Is this an example of oxidation or reduction?
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.
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 is The standard cell voltage for the reaction PbSO4(s) → Pb2+ + SO42- V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.
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.
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?
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.
balance pls show work its just to check
HW12 Balance the following redox in acidic/basic medium MnO- + Fe2+ → Mn2+ + Fe3+ (acidic) Cr2O72- + C,H-OH → Cr3+ + CO2 (acidic) Ag + CN- + 02 → Ag(CN)2- (basic) Cr2O72- + S032– → Cr3+ + SO42- (acidic) C1,02 + H2O2 → C102 +02 (basic) MnO4 + C H204 → Mn2+ + CO2 (acidic) Sn + NO3- → SnC162- + NO2 (basic)
2. Balance the following redox equations by the ion-electron half-reaction method: (a) (acid solution): MnO (s) + PbO2 (s) → MnO,- + Pb2+ (b) (acid solution): MnO4 + Mn2+ → MnO2 (s) (c) (basic solution): Al (8) + OH → Al(OH) - + H2(g)
help
2. (4) Given: PbSO4(e)Pb2 (aq) + SO42 (aq) Calculate the equilibrium constant, if AGt for PbSO4(s) is-811 Kj/mole; for Pb2+ (aq) is 24.3 Kj/mole and for SO42 (ag) is -742 Kj/mole. Calculate the solubility of PbSO4, if the pH of the solution is 4.32 and the [NaHSO4] is 0.10 M. Ka for HSO4 1.02 x 10-2 1. (6) From this week's experiment, what would you expect the signs on ΔΗΡ and So for the observed reaction, Na2B O(OH)8 H2o...