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Redox Reactions Practice

This document provides information and questions about redox reactions. It begins by asking the reader to determine oxidation numbers in various compounds and identify oxidizing and reducing agents. It then asks the reader to write balanced equations for several redox reactions involving species like Fe, Zn, Cr, and I. Finally, it asks the reader to complete and balance redox reactions using the half-reaction method, including reactions involving Zn, I, Mn, Br, Cr, and S species.

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Jeevika
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365 views8 pages

Redox Reactions Practice

This document provides information and questions about redox reactions. It begins by asking the reader to determine oxidation numbers in various compounds and identify oxidizing and reducing agents. It then asks the reader to write balanced equations for several redox reactions involving species like Fe, Zn, Cr, and I. Finally, it asks the reader to complete and balance redox reactions using the half-reaction method, including reactions involving Zn, I, Mn, Br, Cr, and S species.

Uploaded by

Jeevika
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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REDOX REACTIONS

WORKSHEET
BALANCE ATLEAST 2 EQUATIONS PER
DAY
1.Determine the oxidation number of
the elements in each of the following
compounds:

a. H2CO3

b. N2

c. Zn(OH)42-

d. NO2-

e. LiH

f. Fe3O4

1. Identify the species being oxidized


and reduced in each of the following
reactions:

a. Cr+ + Sn4+ Cr3+ + Sn2+

b. 3 Hg2+ + 2 Fe (s) 3 Hg2 + 2 Fe3+


c. 2 As (s) + 3 Cl2 (g) 2 AsCl3

2. Would you use an oxidizing agent


or reducing agent in order for the
following reactions to occur?

a. ClO3- ClO2

b. SO42- S2-

c. Mn2+ MnO2

d. Zn ZnCl2

3. Write balance equations for the


following redox reactions:

a. NaBr + Cl2 NaCl + Br2

b. Fe2O3 + CO Fe + CO2 in acidic


solution
c. CO + I2O5 CO2 + I2 in basic
solution

4. Write balanced equations for the


following reactions:
a. Cr(OH)3 + Br2 CrO42- + Br- in
basic solution
b. O2 + Sb H2O2 + SbO2- in basic
solution
c. HCOOH + MnO4- CO2 + Mn2+ in
acidic solution
d. ClO2- ClO2 + Cl- in acidic solution

5. Write the balanced half reactions


of the following reactions:

a. NiO2 + 2 H2O + Fe Ni(OH)2 +


Fe(OH)2 in basic solution

b. CO2 + 2 NH2OH CO + N2 + 3 H2O


in basic solution

c. 2 H+ + H2O2 + 2 Fe2+ 2 Fe3+ + 2


H2O in acidic solution

d. H+ + 2 H2O + 2 MnO4- + 5 SO2 2


Mn2+ + 5 HSO4- acidic solution

Complete and balance the following redox


reactions using the half-equation
method:
1Zn(s)+H+(aq)→Zn2++H2(g) (acidic
solution)
_________________________________________
(reduction)
________________________________________
oxidation)
(overall)
2I−(aq)+NO2−(aq)→I2(s)+NO(g) (acidic
solution)
_________________________________________
(reduction)
_________________________________________
(oxidation)
_________________________________________
(overall)
3MnO4−(aq)+Cl−(aq)→Mn2+(aq)+Cl2(g)
(acidic solution)
Do the same reaction in basic solution:
4Br2(l)→BrO3−(aq)+Br−(aq)Br2(l)→BrO3−+
Br(aq)− (basic solution)
5CrO42-+S2−→Cr3++SO42− (acidic solution)
6H2O2+NO−2→H2O+NO−3 (acidic solution)
7. CuF2 + NH3 → Cu3N + NH4F + N2
8. Ca3(PO4)2 + SiO2 + C → P4 + CaSiO3 +
CO
Balance each of the given reaction by
oxidation number method ac well as half
reaction method

Acidic medium
• P4 + HNO3 + H2O → H3PO4 + NO

• Sb2S3 + H+ + NO3- → Sb2O5 + HSO4- + NO

• Cr2O72- + H2C2O4 → Cr3+ + CO2

• Mn2+ + S2O82- + H2O → MnO4- + HSO4-

• MnO4- + SCN- → Mn2+ + HSO4- + NO3- + CO2

• CH3CH2OH + Cr2O72- + H+ → CH3COOH +

Cr3+
• CaSO4+ C(s) → CaS(s) + CO2(g)

Basic medium
• I- + OCl- → I2 + Cl- + H2O

• CH3OH + MnO4- → CO32- + MnO42-

• CrI3 + Cl2 → CrO42- + IO4- + Cl-

• Zn + NO3- → Zn(OH)42- + NH3

• MnO4- + SO32- → MnO2 + SO42-

• Pb(OH)42- + ClO- → PbO2 + Cl- + OH-

• MnO4- + Br- → MnO2 + BrO3- + OH-

• Cr(OH)3 + ClO3- → CrO42- + Cl-

• H2O2 + ClO4- → O2 + ClO2-

• ClO3- + N2H4→NO + Cl-

• N2H4 + Fe(CN)63- + OH- → N2 + Fe(CN)64-


• XeF6 + OH-→ Xe + XeO64- + F-
S8 → S2-+S2O32-

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