Log in
Chemistry
1
answer
0
watching
155
views
13 Dec 2019

12.1. Balance the following oxidation-reduction reactions using the half-reaction method, then indicate the number of electrons transferred in the balanced oxidation-reduction reaction.

a) MnO4-(aq) + SO2(g) ---> SO42-(aq) + Mn2+(aq) acidic solution

b) MnO4-(aq) + I-(aq) ---> MnO2(s) + IO3-(aq) basic solution

c) Sb(s) + H2SO4(aq) ---> Sb2(SO4)3(s) + SO2(g) acidic solution

d) Br2(aq) ---> BrO3-(aq) + Br-(aq) basic solution

Watch
1
answer
0
watching
155
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Jarrod Robel
Jarrod RobelLv2
17 Dec 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Balance the following oxidation-reduction reaction occurring in an acidic solution using the half reaction method:

CN1-(aq) + MnO4-(aq) ---> CNO1-(aq) + MnO2(s)

Complete and balance the following equations, and identify the oxidation and reducing agents:

a) Cr2O72-(aq) + I- (aq) → 2Cr +3 + IO3- (acidic solution)

b) MnO4-(aq) + CH3OH(aq) →Mn2+(aq) + HCOOH(aq) (acidic solution)

c) I2(s) + ClO- (aq) → IO3- (aq) +Cl- (aq) (acidic solution)

d) As2O3 (s) + 2NO3-(aq) → 2H3AsO4 +N2O3 (acidic solution)

e) MnO4- + H2O +Br- → 2MnO2 + 2OH- + BrO3- (basic solution)

f) Pb(OH)42- (aq) + ClO- (aq) → PbO2(s) + Cl – (aq) (basic solution)

One Class Solution:-

  1. Cr2O72- + I- + → Cr +3 + IO3- (acidic solution)

+6 +3

Cr2O72-→ Cr +3 REDUCTION

-1 +5

I-→ IO3- OXIDATION

Cr2O72- +14 H+ +6 e- → 2Cr +3 + 7H2O

I- + 3H2O → IO3- + 6H++ 6e-

Cr2O72- + 14 H++ I- + 3H2O → 2Cr +3 + IO3- + 6H+ + 7H2O

+6OH- → 6OH-

Cr2O72- + 8H++ I- + 3H2O → 2Cr +3 + IO3- + 7H2O

b)MnO4- + CH3OH →Mn2+ + HCOOH (acidic solution)

+7 +2

MnO4- →Mn2+ REDUCTION

-2 +2

CH3OH → HCOOH OXIDATION

MnO4- + 8H+ + 5e- → Mn2+ + 4H2O ∕. 4

CH3OH + H2O → HCOOH + 4H+ +4 e- ∕ .5

4MnO4- + 32H+ + 20e-+ 5CH3OH + 5H2O→ 4Mn2+ + 5HCOOH + 20H+ +20 e- + 16H2O

+20OH- → 20OH-

4MnO4- + 12H+ + 5CH3OH + → 4Mn2+ + 5HCOOH + 11H2O

c)I2 + OCl- → IO3- + Cl- (acidic solution)

0 +5

I2→ IO3- OXIDATION

+1 -1

OCl- → Cl- REDUCTION

0 +5

I2 + 3H2O → 2IO3- + 6H+ + 5e- / 2

+1 -1

ClO- + H+ + 2 e-→ Cl- + H2O /5

2I2 + 6H2O + 5ClO- + 5H+ + 10 e- → 4IO3- + 12H+ + 10e- + 5Cl- + 5H2O

+5H+ → +5H+

2I2 + 6H2O + 5ClO- → 4IO3- + 7H+ + 5Cl- + 5H2O

d)As2O3 + NO3-→ H3AsO4 + N2O3 (acidic solution)

+3 +5

As2O3→2H3AsO4 OXIDATION

+5 +3

2NO3-→ N2O3 REDUCTION

As2O3 + 5H2O → 2H3AsO4 + 4H++ 4e- /4

2NO3- + 6H+ +4e- → N2O3 + 3H2O /4

As2O3 + 2NO3- + 6H+ +4e- +5H2O → 2H3AsO4 + 4H++ 4e- + N2O3 + 3H2O

+4 OH → +4OH

As2O3 + 2NO3- + 2H+ +2H2O → 2H3AsO4 + N2O3

e)MnO4- + Br- → MnO2 + BrO3- (basic solution)

+7 +4

MnO4- + 2H2O +3e- → MnO2 + 4OH- /2

-1 +5

Br- + 6OH- → BrO3-+ 3H2O + 6e- /1

2MnO4- + 4H2O +6e- + Br- + 6OH- → 2MnO2 + 8OH-+ BrO3-+ 3H2O + 6e-

+ 6 H+ → + 6 H+

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

f) Pb(OH)42- + ClO- → PbO2 + Cl –

+2 +4

Pb(OH)42- → PbO2 + H2O +2 e- oxidation/1

+1 -1

ClO- + H2O +2 e- → Cl – +2 OH- reduction /1

Pb(OH)42- + ClO- + H2O + 2 e- → PbO2 + H2O + Cl – + 2OH- + 2 e-

+H+ → +H+

Pb(OH)42- + ClO- → PbO2 + Cl – + 2OH-+H2O

Complete and balanced the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction.

  1. (Sn2+(aq) → Sn4+(aq) (acidic solution) ,

  2. TiO2(s) → Ti2+(aq), (acidic solution)

  3. ClO3-(aq) → Cl-(aq) , (acidic solution)

  4. N2→ 2NH4+(aq), (acidic solution)

  5. 4OH- (aq) → O2 (g) , (basic solution)

  6. SO32- (aq) → SO42-(aq), (basic solution)

  7. N2(g) →NH3(g), (basic solution)

One Class Solution:-

  1. Sn2+(aq) → Sn4+(aq) +2e-,

  2. TiO2(s) +2e-+ 4H+→ Ti2+ + 2H2O,

  3. ClO3-+ 6H+ + 6e-→ Cl- + 3H2O,

  4. N2+6e-+ 8H+ → 2NH4+,

  5. 4OH- → O2 +2H2O+4e-,

  6. SO32- + 2OH- → SO42-+2e- + H2O,

  7. N2(g) + 6H2O+ 6e- →2NH3(g) + 6OH-(aq),

a) oxidation, b) reduction, c) reduction, d) reduction, e) oxidation, f) oxidation, g) reduction

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in