1. Lead oxide may be reduced according to the following: PbO2(s) + 4H+ + 2e- =...

1. Lead oxide may be reduced according to the following: PbO2(s) + 4H+ + 2e- = 2H2O + Pb2+ Eo = 1.55 V After a solution of PbO2 is aerated (pO2 = 0.21 atm, pe = 20.75) for a period of time it is observed that Pb2+ = 10-4 mole/L. What is the pH of the solution? Note: pe = Eo / 0.059. (5 points)

Expert Solution

Amanda K answered 6 months ago

Chromium (III) oxide may be reduced by mixing with hydrogen gas. The products formed are solid...

Chromium (III) oxide may be reduced by mixing with hydrogen gas. The products formed are solid chromium and water. What mass of solid chromium in pounds can be prepared from one ton of chromium (III) oxide?

NO3-(aq)+4H+(aq)+3e->NO(g)+2H2O(l) E=0.96V ClO2(g)+e->ClO2-(aq) E=0.95V Cu2+(aq)+2e->Cu(s) E=0.34V 2H+(aq)+2e->H2(g) E=0.00V Pb2+(aq)+2e->Pb(s) E=-0.13V Fe2+(aq)+2e->Fe(s) E=-0.45V Use appropriate data to...

NO3-(aq)+4H+(aq)+3e->NO(g)+2H2O(l) E=0.96V ClO2(g)+e->ClO2-(aq) E=0.95V Cu2+(aq)+2e->Cu(s) E=0.34V 2H+(aq)+2e->H2(g) E=0.00V Pb2+(aq)+2e->Pb(s) E=-0.13V Fe2+(aq)+2e->Fe(s) E=-0.45V Use appropriate data to calculate E?cell for the reaction. 3Cu(s)+2NO3-(aq)+8H+(aq)->3Cu2+(aq)+2NO(g)+4H2O(l) Express your answer using two decimal places.

1. Using the acidic reaction below: Pb(s) + PbO2(s) + SO42-(aq) -> PbSO4(s) Calculate the number...

1. Using the acidic reaction below: Pb(s) + PbO2(s) + SO42-(aq) -> PbSO4(s) Calculate the number of moles of lead required to produce 974.39 grams of PbSO4(s) . 2. Pb(s) + PbO2(s) + SO42-(aq) -> PbSO4(s) Calculate the number of moles of PbSO4(s) produced if 254.15 grams of Pb and 182.88 grams of PbO2(s) were reacted.

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

1. When solid lead(II) sulfide ore burns in oxygen gas, the products are solid lead(II) oxide...

1. When solid lead(II) sulfide ore burns in oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas 2PbS(s)+3O2(g)→2PbO(s)+2SO2(g) A.How many grams of oxygen are required to react with 26.0 g of lead(II) sulfide? B.How many grams of sulfur dioxide can be produced when 61.0 g of lead(II) sulfide reacts? C.How many grams of lead(II) sulfide are used to produce 121 g of lead(II) oxide? 2. Pentane gas, C5H12, undergoes combustion with oxygen to produce carbon dioxide and...

An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq,Pb(s)→Pb2+(aq, 0.15 MM )+2e−)+2e− Red:...

An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq,Pb(s)→Pb2+(aq, 0.15 MM )+2e−)+2e− Red: MnO−4(aq,MnO4−(aq, 1.80 MM )+4H+(aq,)+4H+(aq, 1.9 MM )+3e−→)+3e−→ MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C∘C.

Balance each of the following redox reactions occurring in acidic solution. PbO2(s) + I?(aq) ? Pb2+(aq)...

Balance each of the following redox reactions occurring in acidic solution. PbO2(s) + I?(aq) ? Pb2+(aq) + I2(s) SO32?(aq) + MnO4?(aq) ? SO42?(aq) + Mn2+(aq) S2O32?(aq) + Cl2(g) ? SO42?(aq) + Cl?(aq)

In the following reaction, the atom being reduced is __________ Ni (s) + CuCl2(aq) ---------------------> Cu (s) +...

In the following reaction, the atom being reduced is __________ Ni (s) + CuCl2(aq) ---------------------> Cu (s) + NiCl2 (aq)

Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) +...

Given the following standard reduction potentials: Pb2+ (aq) +2e- ---> Pb (s) E= -.126V PbSO4(s) + 2e- ---> Pb(s) + SO42- (aq) E= -.356V Determine the Ksp for PbSO4(s) at 25 degrees C

1. Antimony reacts with sulfur according to the following reaction: 2Sb(s) + 3S(s) → Sb2S3(s)

1. Antimony reacts with sulfur according to the following reaction:2Sb(s) + 3S(s) → Sb2S3(s)What is the mass percent yield from 2.57 g of Sb in excess S, if 1.72 g of Sb2S3 is obtained? Sb2S3 is 340. g/mol 2. For the following reaction at 25 oC, ΔHo = -1667 kJ and ΔSo = 184 J/KA +4B → 3C + 3D What is ΔGo at 238 oC in kJ?

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