Write the banalced net ionic equation for the following reactions and lable the oxidizing agent.


Write the banalced net ionic equation for the following reactions and lable the oxidizing agent.

1. Effect of HSO3 on Br2 : 2NaHSO3 + Br2 —> 2NaBr + 2 HSO3

2. Effect of HSO3 on H2O2 : HSO3 +H2O2 +OH- —> SO4 2- + 2H2O

3. Effect of HSO3- on Cr2O7 2: Cr2O7 2- + 14 H+ —> 2Cr 3+ + 7H2O

4. Effect of MnO4- on H2O2 : 2KMnO4+ 5H2O2+ 3H2SO4 —> 2MnSO4 +K2SO4 +5O2 +8H2O

Step 1 of 2

Given data: given is the reaction

 

  1. 2NaHSO3+Br2⟶2NaBr+2HSO3
  2. HSO3+H2O2+OH−⟶SO4 2−+2H2O
  3. Cr2O7 2−+14H+⟶2Cr3++7H2O
  4. 2KMnO4+5H2O2+3H2SO4→2MnSO4+K2SO4+5O2+8H2O

 

Find: balance net ionic equation

Explanation:

To write the balanced net ionic equations for the given reactions and label the oxidizing agent, we need to first write the balanced overall equations, and then identify the species that are oxidized and reduced.

 

Step 2 of 2

Let’s write the balanced net ionic equations for the given reactions and identify the oxidizing agents:

1. Effect of HSO3−​ on Br2​:

2NaHSO3​+Br2​⟶2NaBr + 2HSO3−

Net Ionic Equation:

Br2​+2HSO3−​⟶2Br− +2HSO3−​

 

In this reaction, Br2​ is the oxidizing agent.

2. Effect of HSO3−​ on H2​O2​:
HSO3−​+ H2​O2​+OH−⟶SO42−​+2H2​O

Net Ionic Equation:

HSO3−​+H2​O2​⟶SO42−​+2H+

 

In this reaction, HSO3−​ is the reducing agent.

3. Effect of HSO3−​ on Cr2​O72−​:

Cr2​O72−​+14H+⟶2Cr3+ +7H2​O

 

Net Ionic Equation:

Cr2​O72−​+6H+⟶2Cr3+ +3H2​O

 

In this reaction, Cr2​O72−​ is the oxidizing agent.

4. Effect of MnO4−​ on H2​O2​:

2KMnO4​+5H2​O2​+3H2​SO4​⟶2MnSO4​+K2​SO4​+5O2​+8H2​O

 

Net Ionic Equation:

2MnO4−​+5H2​O2​+6H+⟶2Mn2+ +5O2​+8H2​O

 

In this reaction, MnO4−​ is the oxidizing agent.

Explanation:

The net ionic equation is obtained by eliminating spectator ions (ions that do not participate in the chemical change). The species that undergo a change are included in the net ionic equation. The oxidizing agent is the species that gets reduced (gains electrons) in the reaction.

 

Final solution

Therefore, the net ionic equations are:

 

  1. Br2​+2HSO3−​⟶2Br− +2HSO3−​

2 HSO3−​+H2​O2​⟶SO42−​+2H+

3 Cr2​O72−​+6H+⟶2Cr3+ +3H2​O

4 2MnO4−​+5H2​O2​+6H+⟶2Mn2+ +5O2​+8H2​O

 

In each reaction, the species that undergoes reduction is the oxidizing agent. So, the oxidizing agents are:

  1. Br2
  2. H2O2
  3. Cr2O72−
  4. MnO4-

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