Redox reactions

Last updated about 1 year ago

8 questions

1

5

1

2

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Redox reactions

Last updated about 1 year ago

8 questions

1

In the reaction H2 + O2 ➝ H2O hydrogen gets:

1

In this compound the oxidation number of chlorine is:

1

The oxidation number of nitrogen in this ion is:

5

Zn + HgO → ZnO2 + Hg
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

Zn

5

1

In a spontaneous reaction, which of the following metals would most readily donate its electrons?

2

For the following redox reaction, select the appropriate oxidation and reduction half-reaction:
Zn + Fe3+ → Zn2+ + Fe2+

Zn → Zn2++ 2e-
Fe → Fe2++ 2e-

2

Based on your answer from above:
Zn + Fe3+ → Zn2+ + Fe2+
Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

In the reaction H2 + O2 ➝ H2O hydrogen gets:

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

Zn + HgO → ZnO2 + Hg
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

Zn
Zn2+ ions
Hg
Hg2+ ions
O
O2- ions

Substance being oxidised
Substance being reduced
Spectator ion
Oxidising agent
Reducing agent

4FeCl3 + 3C → 4Fe + 3CCl4
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

Fe
Fe2+ ions
Fe3+ ions
Cl
Cl- ions
C
C2+ ions
C4+ ions

Substance being oxidised
Substance being reduced
Spectator ion
Oxidising agent
Reducing agent

In a spontaneous reaction, which of the following metals would most readily donate its electrons?

For the following redox reaction, select the appropriate oxidation and reduction half-reaction:
Zn + Fe3+ → Zn2+ + Fe2+

Zn → Zn2++ 2e-
Zn2++ 2e- → Zn
Fe → Fe2++ 2e-
Fe → Fe3++ 3e-
Fe2+ → Fe3++ e-
Fe2+ + 2e- → Fe
Fe3+ + 3e- → Fe
Fe3+ + e- → Fe2+

oxidation half-reaction
reduction half-reaction

Based on your answer from above:
Zn + Fe3+ → Zn2+ + Fe2+
Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

+1

+5

+7

Zn2+ ions

Hg

Hg2+ ions

O

O2- ions

Substance being oxidised

Substance being reduced

Spectator ion

Oxidising agent

Reducing agent

     4FeCl3   +   3C →  4Fe   +   3CCl4  
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers. 
Note that not all of the listed substances need to be used and some may be used more than once.

Fe

Fe2+ ions

Fe3+ ions

Cl

Cl- ions

C

C2+ ions

C4+ ions

Substance being oxidised

Substance being reduced

Spectator ion

Oxidising agent

Reducing agent

Zn2++ 2e- → Zn

Fe → Fe3++ 3e-

Fe2+ → Fe3++ e-

Fe2+ + 2e-  → Fe

Fe3+ + 3e- → Fe

Fe3+ + e-  → Fe2+

oxidation half-reaction

reduction half-reaction

Redox reactions

Redox reactions

In the reaction H2 + O2 ➝ H2O hydrogen gets:

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

Zn + HgO → ZnO2 + Hg Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers. Note that not all of the listed substances need to be used and some may be used more than once.

Zn + HgO → ZnO2 + Hg

In a spontaneous reaction, which of the following metals would most readily donate its electrons?

For the following redox reaction, select the appropriate oxidation and reduction half-reaction: Zn + Fe3+ → Zn2+ + Fe2+

Zn + Fe3+ → Zn2+ + Fe2+

Based on your answer from above:Zn + Fe3+ → Zn2+ + Fe2+Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

Zn + Fe3+ → Zn2+ + Fe2+

Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

In the reaction H2 + O2 ➝ H2O hydrogen gets:

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

Zn + HgO → ZnO2 + Hg Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers. Note that not all of the listed substances need to be used and some may be used more than once.

Zn + HgO → ZnO2 + Hg

4FeCl3 + 3C → 4Fe + 3CCl4 Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers. Note that not all of the listed substances need to be used and some may be used more than once.

4FeCl3 + 3C → 4Fe + 3CCl4

In a spontaneous reaction, which of the following metals would most readily donate its electrons?

For the following redox reaction, select the appropriate oxidation and reduction half-reaction: Zn + Fe3+ → Zn2+ + Fe2+

Zn + Fe3+ → Zn2+ + Fe2+

Based on your answer from above:Zn + Fe3+ → Zn2+ + Fe2+Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

Zn + Fe3+ → Zn2+ + Fe2+

Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

4FeCl3 + 3C → 4Fe + 3CCl4

Zn + HgO → ZnO2 + Hg
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

For the following redox reaction, select the appropriate oxidation and reduction half-reaction:
Zn + Fe3+ → Zn2+ + Fe2+

Based on your answer from above:
Zn + Fe3+ → Zn2+ + Fe2+
Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.

Zn + HgO → ZnO2 + Hg
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

4FeCl3 + 3C → 4Fe + 3CCl4
Identify ONE substance being oxidised, ONE being reduced, ONE spectator ion, ONE oxidising agent and ONE reducing agent from the list of possible answers.
Note that not all of the listed substances need to be used and some may be used more than once.

For the following redox reaction, select the appropriate oxidation and reduction half-reaction:
Zn + Fe3+ → Zn2+ + Fe2+

Based on your answer from above:
Zn + Fe3+ → Zn2+ + Fe2+
Explain clearly how you would balance the electrons in this reaction in order to obtain the net ionic equation.