代写Chemistry 30 Unit C Module 6 Summative Assessment代写C/C++程序

Chemistry 30 Unit C

Module 6 Summative Assessment

Lesson 1

Use the following information to answer Questions 1-4.

1.        Match the numbers on the electrochemical cell above with the descriptors below.

2.       Write the anode half-reaction, cathode half-reaction and the net cell reaction.

3.       Calculate the electrical potential of the cell.

4.       Describe four empirical observations that would accompany the operation of this cell.

5.       Write the half-reaction for the standard reference half-cell.

6.        How would the net cell potential for the following cell be affected if the reduction of tin(II) ions had been selected as the reference half-cell?

Mg(s) | Mg(NO3 )2 (aq) || Cd(NO3 )2 (aq) | Cd(s)

View the Virtual Investigation “Building Voltaic Cells” in Module 6 Lesson 1.3 and use the results of the experiments to answer Questions 7 – 10.

7.       Complete the following tables to make predictions about the cells constructed in the Virtual Investigation.

•    Draw and fully label a diagram for each cell.

•    For each cell, indicate the direction of electron flow, cation flow and anion flow.

• Write half-reactions for each half-cell.

• Write a net reaction for each cell.

•   Write the cell notation.

•   Suggest empirical evidence that would indicate a reaction has occurred in each half-cell. Consider parameters such as pH, mass of electrodes, colour of solution(s) etc.

•   Calculate the theoretical standard cell potential.

•    Record the Actual Cell Potential seen in the investigation. If the voltage is fluctuating, record the highest value that you observe.

• System 1 has been completed for you as an exemplar. Be sure to read over this example to help you avoid common mistakes!

System 1 – Exemplar:

Fully Labelled Diagram (Example) It is NOT permitted to copy this diagram for the next Systems. Make sure you are drawing your own diagrams for the remaining Systems.
Oxidation Half- reaction	Zn(s) →Zn2+ (aq) + 2 e-
Reduction Half- reaction	Ag+ (aq) + 1e- →Ag(s)
Net Cell Reaction	2 Ag+ (aq) + Zn(s) → Zn2+ (aq) + 2 Ag(s)
Cell Notation	Zn(s)|Zn2+ (aq)||Ag+ (aq)|Ag(s)
Empirical Evidence	Cathode: Mass of silver electrode increases Anode: Mass of zinc electrode decreases
Theoretical Standard Cell Potential	E 0 cell = E 0 cathode - E 0anode E 0 cell = +0.80 V – (-0.76 V) E 0 cell = + 1.56 V
Observed Cell Potential	1.27 V

System 2

Answer   (11 Marks)

Fully Labelled Diagram
Oxidation Half- reaction
Reduction Half- reaction
Net Cell Reaction
Cell Notation
Empirical Evidence	Anode: Cathode:
Theoretical Standard Cell Potential
Observed Cell Potential

System 3

Answer   (7 Marks)

(No Diagram Required)
Oxidation Half- reaction
Reduction Half- reaction
Net Cell Reaction
Cell Notation
Empirical Evidence	Anode: Cathode:
Theoretical Standard Cell Potential
Observed Cell Potential

System 4

Answer   (11 Marks)

Fully Labelled Diagram
Oxidation Half- reaction
Reduction Half- reaction
Net Cell Reaction
Cell Notation
Empirical Evidence	Anode: Cathode:
Theoretical Standard Cell Potential
Observed Cell Potential

System 5

Answer (7 Marks)

(No Diagram Required)
Oxidation Half- reaction
Reduction Half- reaction
Net Cell Reaction
Cell Notation
Empirical Evidence	Anode: Cathode:
Theoretical Standard Cell Potential
Actual Cell Potential

8.        In this Virtual Investigation, would you expect a difference in the cell potentials if larger cells had been constructed and tested?  Explain.

9.        Identify how each of the following changes would affect the operation of

each cell. Circle either “ Cell will operate the same” OR “ Cell will not operate the same” to identify the result of the change. Explain why you chose your   answer for full marks.

10.     What does the voltmeter read when the salt bridge is removed? Explain why this occurs.

Use the following information to answer the next 4 questions.

Japanese car manufacturer Daihatsu is investigating the use of hydrazine as a fuel for fuel cell electric vehicles.  One main advantage of a hydrazine fuel cell compared to a traditional fuel cell, is the use of cheaper more readily available metal catalysts instead of the traditional, expensive platinum catalyst used for most fuel cells.

11.     Given the net cell reaction and the cathode half-reaction determine the anode half-reaction.

net reaction: N2 H4 (aq) + O2 (g) → N2 (g)  + 2 H2 O(l)

cathode half-reaction: O2 (g) + 2 H2 O(l) + 4 e- → 4 OH-(aq)

Hint: Look at each species in the net reaction and consider which reaction it came from:

cathode or anode. If it did not come from the given cathode reaction, it may have come from the anode reaction.

12.      If the cell potential for the hydrazine fuel cell is 0.73 V, calculate the reduction potential for the half-cell involving hydrazine.

13.       Identify an advantage of using a fuel cell over a primary or secondary cell.

14.      Identify an advantage of using a fuel cell over combustion of fossil fuel.

Perform. the Virtual Investigation “Corrosion” in Module 6 Lesson 1.5 and use the results to answer Questions 15 – 22.

15. For this Virtual Investigation, identify the manipulated variable, the responding variable, and two controlled variables.

Hint: Manipulated variables are conditions that are deliberately changed by the experimenter (what you are testing).  Responding variables are conditions that   change in response to the change in the manipulated variables (the data you

collect).  Controlled variables are conditions that are held constant to ensure an accurate comparison between trials.