{{asɛmtiNe Ɔkyerɛwfo}} | Nhomakorabea | Nneɛma a ɛma wotumi yɛ ade

1

In the reaction H₂ + O₂ ➝ H₂O hydrogen gets:

oxidized

reduced

neither oxidised nor reduced

1

In this compound the oxidation number of chlorine is:

1

The oxidation number of nitrogen in this ion is:

-3

+3

+4

+5

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
Zn²⁺ions
Hg
Hg²⁺ ions
O
O^2- ions

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

5

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

1

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

Tin (Sn)

Nickel (Ni)

Cesium (Cs)

Platinum (Pt)

2

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

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.}

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

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.}

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.}

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

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.

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.

In the reaction H₂ + O₂ ➝ H₂O hydrogen gets:

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

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:

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

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.}