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E-DAY PROJECT - Redox Practical Investigation

Last updated 10 months ago
16 questions
Note from the author:
I have made and inserted gifs of the simulations for you directly into this Formative. You may use your textbook to complete this assessment.
I have made and inserted gifs of the simulations for you directly into this Formative. You may use your textbook to complete this assessment.
Part A: Reactivity Series
Some metals react readily with others, displacing them out of a solution and sometimes, there is no reaction.
For these simulations you need to observe in each case whether a reaction takes place between the two metals.
Where a reaction does take place, describe your observations. You will also calculate the Eo cell value for each combination.

SIMULATION 1

The reactions of Mg with various metal solutions.
Use the simulation to observe the reactivity of magnesium in each solution.
8

FOR EACH BEAKER:
FIRST record if a reaction takes place or does not take place.
SECOND If a reaction does takes place, record ALL your observations by choosing from the list of options. If there is no obvious change to the colour of a solution or the piece of metal, then no observation about the solution or piece of metal needs to be made.

  • No reaction takes place
  • Reaction takes place
  • Observation: A dark grey deposit forms on the metal
  • Observation: A silvery grey deposit forms on the metal
  • Observation: A reddish-brown deposit forms on the metal
  • Observation: The blue solution becomes lighter in colour
  • Observation: The blue solution becomes darker in colour
  • Observation: The colourless solution turns blue
  • Mg in Mg(NO3)2
  • Mg in Zn(NO3)2
  • Mg in Cu(NO3)2
  • Mg in AgNO3
4

TWO observations were seen in the Mg in Cu(NO3)2 experiment. Explain why each one occurred.

8

Calculate the Eo cell values for each of the redox reactions with magnesium metal. Choose the correct answer (with the correct sign) for each combination from the list of options.

  • - 3,17 V
  • - 2,71 V
  • - 1,61 V
  • - 1,56 V
  • - 1,10 V
  • - 0,46 V
  • 0,00 V
  • + 0,46 V
  • + 1,10 V
  • + 1,56 V
  • + 1,61 V
  • + 2,71 V
  • + 3,17 V
  • Mg in Mg(NO3)2
  • Mg in Zn(NO3)2
  • Mg in AgNO3
  • Mg in Cu(NO3)2

SIMULATION 2

The reactions of Cu with various metal solutions
Use the simulation to observe the reactivity of copper in each solution.
8

FOR EACH BEAKER:
FIRST record if a reaction takes place or does not take place.
SECOND If a reaction takes place, record ALL your observations by choosing from the list of options. If there is no obvious change to the colour of a solution or the piece of metal, then no observation about the solution or piece of metal needs to be made.

  • No reaction takes place
  • Reaction takes place
  • Observation: A dark grey deposit forms on the metal
  • Observation: A silvery grey deposit forms on the metal
  • Observation: A reddish-brown deposit forms on the metal
  • Observation: The blue solution becomes lighter in colour
  • Observation: The blue solution becomes darker in colour
  • Observation: The colourless solution turns blue
  • Cu in Mg(NO3)2
  • Cu in Zn(NO3)2
  • Cu in Cu(NO3)2
  • Cu in AgNO3
8

Calculate the Eo cell values for each of the redox reactions with copper metal. Choose the correct answer (with the correct sign) for each combination from the list of options.

  • - 3,17 V
  • - 2,71 V
  • - 1,61 V
  • - 1,56 V
  • - 1,10 V
  • - 0,46 V
  • 0,00 V
  • + 0,46 V
  • + 1,10 V
  • + 1,56 V
  • + 1,61 V
  • + 2,71 V
  • + 3.17 V
  • Cu in Mg(NO3)2
  • Cu in Zn(NO3)2
  • Cu in Cu(NO3)2
  • Cu in AgNO3

SIMULATION 3

The reactions of Zn with various metal solutions
Use the simulation to observe the reactivity of zinc in each solution.

8

FOR EACH BEAKER:
FIRST record if a reaction takes place or does not take place.
SECOND If a reaction takes place, record ALL your observations by choosing from the list of options. If there is no obvious change to the colour of a solution or the piece of metal, then no observation about the solution or piece of metal needs to be made.

  • No reaction takes place
  • Reaction takes place
  • Observation: A dark grey deposit forms on the metal
  • Observation: A silvery grey deposit forms on the metal
  • Observation: A reddish-brown deposit forms on the metal
  • Observation: The blue solution becomes lighter in colour
  • Observation: The blue solution becomes darker in colour
  • Observation: The colourless solution turns blue
  • Zn in Mg(NO3)2
  • Zn in Zn(NO3)2
  • Zn in Cu(NO3)2
  • Zn in AgNO3
8

Calculate the Eo cell values for each of the redox reactions with zinc metal. Choose the correct answer (with the correct sign) for each combination from the list of options.

  • - 3,17 V
  • - 2,71 V
  • - 1,61 V
  • - 1,56 V
  • - 1,10 V
  • - 0,46 V
  • 0,00 V
  • + 0,46 V
  • + 1,10 V
  • + 1,56 V
  • + 1,61 V
  • + 2,71 V
  • + 3.17 V
  • Zn in Mg(NO3)2
  • Zn in Zn(NO3)2
  • Zn in Cu(NO3)2
  • Zn in AgNO3

SIMULATION 4

The reactions of Ag with various metal solutions
Use the simulation to observe the reactivity of silver in each solution.

8

FOR EACH BEAKER:
FIRST record if a reaction takes place or does not take place.
SECOND If a reaction takes place, record ALL your observations by choosing from the list of options. If there is no obvious change to the colour of a solution or the piece of metal, then no observation about the solution or piece of metal needs to be made.

  • No reaction takes place
  • Reaction takes place
  • Observation: A dark grey deposit forms on the metal
  • Observation: A silvery grey deposit forms on the metal
  • Observation: A reddish-brown deposit forms on the metal
  • Observation: The blue solution becomes lighter in colour
  • Observation: The blue solution becomes darker in colour
  • Observation: The colourless solution turns blue
  • Ag in Mg(NO3)2
  • Ag in Zn(NO3)2
  • Ag in Cu(NO3)2
  • Ag in AgNO3
8

Calculate the Eo cell values for each of the redox reactions with silver metal. Choose the correct answer (with the correct sign) for each combination from the list of options.

  • - 3,17 V
  • - 2,71 V
  • - 1,61 V
  • - 1,56 V
  • - 1,10 V
  • - 0,46 V
  • 0,00 V
  • + 0,46 V
  • + 1,10 V
  • + 1,56 V
  • + 1,61 V
  • + 2,71 V
  • + 3.17 V
  • Ag in Mg(NO3)2
  • Ag in Zn(NO3)2
  • Ag in Cu(NO3)2
  • Ag in AgNO3
2

Conclusion:

Based on the results of Part A of this investigation, rank the metals in order from most reactive to least reactive:

  1. Cu
  2. Ag
  3. Mg
  4. Zn
Part B: Redox at the molecular level
In this simulation you can observe a redox reaction at the molecular level.

SIMULATION 5

Zn in Cu(NO3)2 at the molecular level

4
Identify the half-reactions for this reaction:
Oxidation 1/2 reaction: _____________________
Reduction 1/2 reaction: ____________________
Other Answer Choices:
Zn2+ + 2e- ➝ Zn
Zn ➝ Zn2+ + 2e-
Cu2+ + 2e- ➝ Cu
Cu ➝ Cu2+ + 2e-
1

Is this reaction spontaneous or non-spontaneous?

5

Explain your answer above by refering to the relative strengths of the reducing agents. Complete the explanation by dragging the appropriate substance into each step of the explanation:

  • Zn
  • Zn2+
  • Cu
  • Cu2+
  • _____ is a better reducing agent
  • than _______
  • Therefore in the presence of _____ ,
  • _______ will/will not [don't need to distinguish]
  • be readily reduced to form ________

Simulation 6

Cu in Zn(NO3)2 at the molecular level

4
Identify the half-reactions for this reaction:
Oxidation 1/2 reaction: ____________________
Reduction 1/2 reaction: ____________________
Other Answer Choices:
Cu2+ + 2e- ➝ Cu
Zn2+ + 2e- ➝ Zn
Cu ➝ Cu2+ + 2e-
Zn ➝ Zn2+ + 2e-
1

Is this reaction spontaneous or non-spontaneous?

5

Explain your answer above by refering to the relative strengths of the reducing agents. Complete the explanation by dragging the appropriate substance into each step of the explanation:

  • Zn
  • Zn2+
  • Cu
  • Cu2+
  • _____ is a better reducing agent
  • than _______
  • Therefore in the presence of _____ ,
  • _______ will/will not [don't need to distinguish]
  • be readily reduced to form ________