series of redox reactions. On a separate sheet of paper, organize your data to r

Question

series of redox reactions. On a separate sheet of paper, organize your data to record the test tube number and your observations for the 8 reaction mixtures in Table 27.1. Use the appropriate half-reactions (one for solution A and another for solution B) that appear under Reducing Agents and Oxidizing Agents in the Introduction. Add the two half-reactions such that the electrons gained by one solution equal the electrons lost by the other-this sum provides the overall balanced equation Write a balanced redox equation for each observed reaction: [Box the oxidizing agent in each writen equation. Submit this with the completed Report Sheet

Explanation / Answer

For the given set of reactions,

Test tube 1

balanced equation,

2ClO- + 2HCl + Fe(NH4)2SO4 ---> 2HClO + FeCl2 + (NH4)2SO4

Oxidizing agent = ClO-

Test tube 2

balanced equation,

3Cl2 + 3H2O + KI ---> HIO3 + KCl + 5HCl

Oxidizing agent = Cl2

Test tube 3,

balanced equation,

2KMnO4 + 8H2SO4 + 10Fe(NH4)2SO4 ---> K2SO4 + 5Fe2(SO4)3 + 10(NH4)2SO4 + 2MnSO4 + 8H2O

Oxidizing agent = KMnO4

Test tube 4,

balanced equation,

KMnO4 + 2H2SO4 + 2K2C2O4 ---> 4CO2 + 2K2SO4 + KMnO2 + 2H2O

Test tube 5,

No reaction

Test tube 6

balanced equation,

8KI + 5H2SO4 --> 4K2SO4 + 4I2 + H2S + 4H2O

oxidizing agent : H2SO4

Test tube 7,

balanced equation,

3H2O2 + 3H2SO4 + Fe(NH4)2SO4 --> (NH4)2SO4 + Fe(SO4)3 + 6H2O

oxidizing agent : H2O2

Test tube 8,

H2O2 + H2SO4 + 2KI --> K2SO4 + 2H2O + I2

oxidizing agent : H2O2

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