代写Chemistry 30 Unit C Module 5 Summative Assessment代写Java编程

Chemistry 30 Unit C

Module 5 Summative Assessment

Lesson 1

View the Virtual Investigation on Oxidation States in Module 5 Lesson 1.5 and use the information to fill in the table in Question 1.

1.        Identify the characteristic colour of the various oxidation states of manganese.

Answer   (3 Marks)

Oxidation State	Colour
+7
+6
+4

2.  Classify each of the following reactions as redox or non-redox.

Answer   (4 Marks)

reaction equation	redox or non-redox
3Cl2(g) + 6NaOH(aq) →5NaCl(aq) + NaClO3(aq) + 3H2O(l)
CO2(g) + H2O(l) → H2CO3(aq)
2 NH4Cl(aq) + Ca(OH)2(aq) →2 NH3(aq) + 2H2O(l) + CaCl2(aq)
2HNO3(aq) + 6HI(aq) →2NO(g) +3 I2(s) + 4H2O(l)

3.  Describe disproportionation. Next, consider the reactions shown in Question 2

above and indicate if any of the reactions demonstrate disproportionation.

Answer   (2 Marks)

Lesson 2 

Use the following information to answer Questions 4 - 7.

In an experiment to study the reactivity of different substances, the following observations were made. 2V3+(aq) + In1+(aq) → 2V2+(aq) + In3+(aq) spontaneous reaction 2 Rh4+(aq) + Tl1+(aq) → 2 Rh3+(aq) + Tl3+(aq) spontaneous reaction  Tl1+(aq) + 2 V3+(aq) → Tl3+(aq) + 2 V2+(aq) no evidence of a reaction Hint: By looking at changes in oxidation numbers, you can determine the OA and RA for each reaction.  Then apply the spontaneity rule. (p. 572-573 in text).

4.  Using the above results, construct a table of reduction half-reactions that

contains four half-reactions. Be sure to include the number of electrons in each half-reaction. Model your table on the set-up shown below:

Answer    (2 Marks)

5.   Identify the reducing agent that has the weakest attraction for electrons.

Answer   (1 Mark)

6.  Identify the oxidizing agent that has the strongest attraction for electrons.

Answer   (1 Mark)

7.  Based on the table you constructed in Question 4, write an equation that represents another spontaneous reaction that could occur.

Answer   (1 Mark)

View the Virtual Investigation “Predicting Redox Reactions” in Module 5 Lesson 2.3 and use the results to answer Questions 8 -12.

8.   Predict the products for each system in the Virtual Investigation. Your response should include

●   All species initially present

●   All oxidizing agents and reducing agents. Identify the Strongest Reducing Agent (SRA) and Strongest Oxidizing Agent (SOA)

●   If the reaction is spontaneous, indicate “yes” and write the half-reactions and the balanced net ionic equation.  If the reaction is non-spontaneous, simply indicate “no” in the blank . Include the half-reactions but it is not necessary to write net ionic equation if the reaction is non-spontaneous.

●   System 1 and 2 have been completed for you as examples. Refer to these examples before completing the rest of the System tables - they will be very helpful in clarifying common mistakes!

System 1 Example - liquid water and solid calcium

Species List	H2 O(l), Ca(s)
Oxidizing agents	H2 O(l) SOA= H2 O(l)
Reducing agents	H2 O(l), Ca(s) SRA= Ca(s)
Spontaneous?	Yes
Reduction half- reaction	2 H2 O(l) + 2e- → H2 (g) + 2 OH-(aq)
Oxidation half- reaction	Ca(s) → Ca2+ (aq) + 2e-
Net ionic equation	2 H2 O(l) + Ca(s) → Ca2+ (aq) + H2 (g) + 2 OH-(aq)

System 2 Example - aqueous hydrochloric acid and solid silver metal

Species List	H+(aq), Cl-(aq), H2 O(l), Ag(s)
Oxidizing agents	H2 O(l), H+(aq) SOA= H+(aq)
Reducing agents	H2 O(l), Ag(s), Cl-(aq), Cl-(aq) + H2 O(l), SRA= Ag(s)
Spontaneous?	No
Reduction half- reaction	2 H+(aq) + 2e- → H2 (g)
Oxidation half- reaction	Ag(s) → Ag1+ (aq) + 1e-
Net ionic equation	Non-spontaneous

System 3 - aqueous hydrochloric acid and solid magnesium metal

Answer   (4 Marks)

Species List
Oxidizing Agents
Reducing agents
Spontaneous?
Reduction half- reaction
Oxidation half- reaction
Net ionic equation

System 4 - Acidified aqueous iron(II) nitrate and aqueous potassium dichromate

Hint: Study the species list carefully and remember to consider combination agents!

Answer   (4 Marks)

Species List
Oxidizing agents
Reducing agents
Spontaneous?
Reduction half- reaction
Oxidation half- reaction
Net ionic equation

System 5 - aqueous hydrogen peroxide and aqueous iron(III) nitrate

Hint: This system is not acidified.

Answer   (4 Marks)

System 6 - aqueous zinc nitrate and aqueous chromium(II) chloride

Answer   (4 Marks)

System 7 - aqueous silver nitrate and solid copper metal

Answer   (4 Marks)

9.  Record your observations from the Virtual Investigation in the following table.

Answer (5 Marks)

10.Describe the diagnostic test that could be used to identify the gas produced in System 1.

Your response should include

●   a description of how the test is performed

●   identity of the gas being tested for

●   the results of the test

Hint: Seepage 805 in your textbook for a list of diagnostic tests.

Answer   (3 Marks)

11.Describe the diagnostic test that could be used to identify the gas produced in System 5.

Your response should include

●   a description of how the test is performed

●   identity of the gas being tested for

●   the results of the test

Hint: Seepage 805 in your textbook for a list of diagnostic tests.

Answer   (3 Marks)

12. Measuring pH change is sometimes used as a diagnostic test. In which of the seven systems might we have used pH change as evidence of a spontaneous reaction?  Explain your reasoning.

Answer   (2 Marks)