General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 19, Problem 19.2QP

(a)

Interpretation Introduction

Interpretation: The given redox equation should be balanced by the half-reaction method.

Concept Introduction:

Half-reaction can either be oxidation or reduction reaction of a reactant component in a redox reaction.

Oxidation: Removal of electrons from a chemical species is known as oxidation.

Reduction: Addition of electrons to a chemical species is known as reduction.

Redox reaction: It is a reaction which involves both reduction and oxidation reactions.

To balance the equation, use the following steps:

The general steps involved balancing the redox reactions in both acidic and basic conditions:

  • Write the oxidation number for all of the elements involved in reaction.
  • Based on the change in the oxidation number separate the reaction into reduced and oxidized half-reactions.
  • Balance the atoms other than Oxygen and Hydrogen atom.
  • Balance the Oxygen atoms by adding water on the appropriate side.
  • Balance the hydrogen atoms by adding equal number of H+ on the opposite side.
  • Only in the basic condition, the H+ ions are needed to be balanced further. The H+ ions are balanced by the addition of equal number of OH- ions on both the sides. If there are equal number of H+ and OH- ions on any of the two sides, it will constitute the corresponding number of water molecules.
  • Balance the charge by adding appropriate number of electrons at the appropriate side.
  • Multiply the reduction and oxidation half-reactions, by the whole number such that the number of electrons released in the oxidation half-reaction should be equal to the number of electrons gained in the reduction half-reaction.
  • Add both the oxidation and reduction half-reactions and cancel out the electrons on both the sides of the reaction.
  • Write the final equation and count the number of atoms and check the charge to verify the balanced reaction.

(a)

Expert Solution
Check Mark

Answer to Problem 19.2QP

The balanced redox reaction is 2OH-+H2O+Mn2++H2O2MnO2+H2O+2H2O

Explanation of Solution

The given equation in basic condition is shown below with oxidation states:

Mn2++H2O2MnO2+H2O

The manganese atoms are being balanced on both sides.

Balancing oxygen:

Water molecule is needed to be added to balance the oxygen atom which is shown below:

H2O+Mn2++H2O2MnO2+H2O

Balancing hydrogen:

Now the hydrogen atoms are needed to be balanced by the addition of protons which is shown below:

H2O+Mn2++H2O2MnO2+H2O+2H+

Balancing Protons:

The protons can be balanced by adding the equal number of hydroxide ions on both sides.

2OH-+H2O+Mn2++H2O2MnO2+H2O+2H++2OH-

The equal number of protons and hydroxide ions on one particular side is converted into the equal number of water molecules.

2OH-+H2O+Mn2++H2O2MnO2+H2O+2H2O

So this is the overall balanced reaction.

(b)

Interpretation Introduction

Interpretation: The given redox equation should be balanced by the half-reaction method.

Concept Introduction:

Half-reaction can either be oxidation or reduction reaction of a reactant component in a redox reaction.

Oxidation: Removal of electrons from a chemical species is known as oxidation.

Reduction: Addition of electrons to a chemical species is known as reduction.

Redox reaction: It is a reaction which involves both reduction and oxidation reactions.

To balance the equation, use the following steps:

The general steps involved balancing the redox reactions in both acidic and basic conditions:

  • Write the oxidation number for all of the elements involved in reaction.
  • Based on the change in the oxidation number separate the reaction into reduced and oxidized half-reactions.
  • Balance the atoms other than Oxygen and Hydrogen atom.
  • Balance the Oxygen atoms by adding water on the appropriate side.
  • Balance the hydrogen atoms by adding equal number of H+ on the opposite side.
  • Only in the basic condition, the H+ ions are needed to be balanced further. The H+ ions are balanced by the addition of equal number of OH- ions on both the sides. If there are equal number of H+ and OH- ions on any of the two sides, it will constitute the corresponding number of water molecules.
  • Balance the charge by adding appropriate number of electrons at the appropriate side.
  • Multiply the reduction and oxidation half-reactions, by the whole number such that the number of electrons released in the oxidation half-reaction should be equal to the number of electrons gained in the reduction half-reaction.
  • Add both the oxidation and reduction half-reactions and cancel out the electrons on both the sides of the reaction.
  • Write the final equation and count the number of atoms and check the charge to verify the balanced reaction.

(b)

Expert Solution
Check Mark

Answer to Problem 19.2QP

The balanced redox reaction is e-+H2O+Bi(OH)3+SnO22-SnO32-+Bi+2H2O+OH

Explanation of Solution

The given equation in basic condition is shown below with oxidation states:

Bi(OH)3+SnO22-SnO32-+Bi

Both bismuth and tin atoms are being balanced on both sides.

Balancing oxygen:

Water molecule is needed to be added to balance the oxygen atom which is shown below:

Bi(OH)3+SnO22-SnO32-+Bi+2H2O

Balancing hydrogen:

Now the hydrogen atoms are needed to be balanced by the addition of protons which is shown below:

H++Bi(OH)3+SnO22-SnO32-+Bi+2H2O

Balancing Protons:

The protons can be balanced by adding the equal number of hydroxide ions on both sides.

OH+H++Bi(OH)3+SnO22-SnO32-+Bi+2H2O+OH

The equal number of protons and hydroxide ions on one particular side is converted into the equal number of water molecules.

H2O+Bi(OH)3+SnO22-SnO32-+Bi+2H2O+OH

Balancing charge:

The charge has to be balanced by adding the required number of electrons to the more positively charged side.

e-+H2O+Bi(OH)3+SnO22-SnO32-+Bi+2H2O+OH

So this is the overall balanced reaction.

(c)

Interpretation Introduction

Interpretation: The given redox equation should be balanced by the half-reaction method.

Concept Introduction:

Half-reaction can either be oxidation or reduction reaction of a reactant component in a redox reaction.

Oxidation: Removal of electrons from a chemical species is known as oxidation.

Reduction: Addition of electrons to a chemical species is known as reduction.

Redox reaction: It is a reaction which involves both reduction and oxidation reactions.

To balance the equation, use the following steps:

The general steps involved balancing the redox reactions in both acidic and basic conditions:

  • Write the oxidation number for all of the elements involved in reaction.
  • Based on the change in the oxidation number separate the reaction into reduced and oxidized half-reactions.
  • Balance the atoms other than Oxygen and Hydrogen atom.
  • Balance the Oxygen atoms by adding water on the appropriate side.
  • Balance the hydrogen atoms by adding equal number of H+ on the opposite side.
  • Only in the basic condition, the H+ ions are needed to be balanced further. The H+ ions are balanced by the addition of equal number of OH- ions on both the sides. If there are equal number of H+ and OH- ions on any of the two sides, it will constitute the corresponding number of water molecules.
  • Balance the charge by adding appropriate number of electrons at the appropriate side.
  • Multiply the reduction and oxidation half-reactions, by the whole number such that the number of electrons released in the oxidation half-reaction should be equal to the number of electrons gained in the reduction half-reaction.
  • Add both the oxidation and reduction half-reactions and cancel out the electrons on both the sides of the reaction.
  • Write the final equation and count the number of atoms and check the charge to verify the balanced reaction.

(c)

Expert Solution
Check Mark

Answer to Problem 19.2QP

The balanced redox reaction is 6C2O42-+28H++2Cr2O72-4Cr3++14H2O+12CO2

Explanation of Solution

The given equation in acidic condition is given below:

Cr2O72-+C2O42-Cr3++CO2

The half reactions are:

Oxidation half-reaction is:

C2O42-CO2

Balancing carbon:

C2O42-2CO2

Balancing charge:

C2O42-2CO2+2e-

Reduction half-reaction is:

Cr2O72-Cr3+

Balancing chromium:

Cr2O72-2Cr3+

Balancing oxygen:

Cr2O72-2Cr3++7H2O

Balancing hydrogen:

14H++Cr2O72-2Cr3++7H2O

Balancing charge:

6e-+14H++Cr2O72-2Cr3++7H2O

Determining the overall balanced equation:

The balanced reduction half-reaction is 6e-+14H++Cr2O72-2Cr3++7H2O

The balanced oxidation half-reaction is C2O42-2CO2+2e-

2(6e-+14H++Cr2O72-2Cr3++7H2O)6(C2O42-2CO2+2e-)

6C2O42-+12e+28H++2Cr2O72-4Cr3++14H2O+12CO2+12e

6C2O42-+28H++2Cr2O72-4Cr3++14H2O+12CO2Thisistheoverallbalancedequation in the acidic condition.

(d)

Interpretation Introduction

Interpretation: The given redox equation should be balanced by the half-reaction method.

Concept Introduction:

Half-reaction can either be oxidation or reduction reaction of a reactant component in a redox reaction.

Oxidation: Removal of electrons from a chemical species is known as oxidation.

Reduction: Addition of electrons to a chemical species is known as reduction.

Redox reaction: It is a reaction which involves both reduction and oxidation reactions.

To balance the equation, use the following steps:

The general steps involved balancing the redox reactions in both acidic and basic conditions:

  • Write the oxidation number for all of the elements involved in reaction.
  • Based on the change in the oxidation number separate the reaction into reduced and oxidized half-reactions.
  • Balance the atoms other than Oxygen and Hydrogen atom.
  • Balance the Oxygen atoms by adding water on the appropriate side.
  • Balance the hydrogen atoms by adding equal number of H+ on the opposite side.
  • Only in the basic condition, the H+ ions are needed to be balanced further. The H+ ions are balanced by the addition of equal number of OH- ions on both the sides. If there are equal number of H+ and OH- ions on any of the two sides, it will constitute the corresponding number of water molecules.
  • Balance the charge by adding appropriate number of electrons at the appropriate side.
  • Multiply the reduction and oxidation half-reactions, by the whole number such that the number of electrons released in the oxidation half-reaction should be equal to the number of electrons gained in the reduction half-reaction.
  • Add both the oxidation and reduction half-reactions and cancel out the electrons on both the sides of the reaction.
  • Write the final equation and count the number of atoms and check the charge to verify the balanced reaction.

(d)

Expert Solution
Check Mark

Answer to Problem 19.2QP

The balanced redox reaction is 2H++ClO3-+Cl-Cl2+ClO2+H2O

Explanation of Solution

The given equation in acidic condition is given below:

ClO3-+Cl-Cl2+ClO2

The chlorine atoms are being balanced.

Balancing Oxygen:

Water molecule is needed to be added to balance the oxygen atom which is shown below:

ClO3-+Cl-Cl2+ClO2+H2O

Balancing Hydrogen:

Now the hydrogen atoms are needed to be balanced by the addition of protons which is shown below:

2H++ClO3-+Cl-Cl2+ClO2+H2O

This is the overall balanced reaction.

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Chapter 19 Solutions

General Chemistry

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