-1) Balance the following redox equation in base . In the blank put the correct

Question

-1) Balance the following redox equation in base. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equation.)

MnO4(aq) + Br(aq) + H2O(l)   MnO2(s) + BrO3(aq) + HO(aq)

-2) Balance the following redox equation in acid. In the blank put the correct stochiometric coefficient (0, 1, 2, etc.). (Note: 0 if the species does not appear on that side of the equation.)

PbO2(s) +  I(aq) + H+(aq)   Pb2+(aq) + I2(s) + H2O(l)

-3) In the electrochemical voltaic cell using the reaction, Zn(s) + Cu2+(aq) Zn2+(aq) + Cu(s), match the correct 1/2 reaction that occurs at the anode and cathode.

- 1/2 reaction occuring at anode

- 1/2 reaction occuring at cathode

-4) Using the reduction potentials table in the notes/book, which of the following is the best oxidizing agent?

Cl2

I2

Cl-

I-

Cl2

I2

Cl-

I-

Explanation / Answer

step 1 : identify half cells

MnO4- + 3e- ---> MnO2

+7 + 4

Br- ---> BrO3- + 6e-

-1 +5

step 2: balanec electrons

2MnO4- + 6e- ---> 2MnO2

Br- ---> BrO3- + 6e-

step 3: Balance O

2MnO4- + 6e- ---> 2MnO2 + 4H2O

Br- +3H2O ---> BrO3- + 6e-

step 4: Balance H

2MnO4- + 6e- + 8H+ ---> 2MnO2 + 4H2O

Br- +3H2O ---> BrO3- + 6e- + 6H+

step 5: replaced H+ with OH-

2MnO4- + 6e- + 8H2O ---> 2MnO2 + 4H2O + 8 OH-

Br- +3H2O + 6OH- ---> BrO3- + 6e- + 6H2O

step 6: add both equation

2MnO4- + Br- + H2O ---> 2MnO2 + BrO3- + 2OH-

This is the balanced equation

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