Module 3 Summative Assessment

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Jun 14, 2024

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Chemistry 30 Unit B Module 3 Summative Assessment Page 1 of 13 Module 3 Summative Assessment 1. Write balanced reaction equations, including states, for the following processes. Identify each process as exothermic or endothermic. Answer (6 Marks) Process Reaction Equation Photosynthesis 6 CO2 + 6 H2O + energy -> C6H12O6 + 6 O2 Cellular respiration C6H12O6 + 6 O2 -> 6 CO2 + 6 H2O + energy Complete hydrocarbon combustion of octane in an open system CnHn + O2 -> CO2 + H2O + energy Process Exothermic/Endothermic Photosynthesis Endothermic Cellular respiration Exothermic Complete hydrocarbon combustion Exothermic Lesson 1 2. Enthalpy cannot be directly measured but change in enthalpy can be measured. When measuring the change in enthalpy of a chemical system, which 2 variables must be held constant? As a result, what does the enthalpy change of a chemical system represent? Answer (2 Marks) Marks Maximum Possible Earned % 65
Chemistry 30 Unit B Module 3 Summative Assessment Page 2 of 13 The 2 variables that must be held constant when measuring enthalpy change are temperature and pressure. As a result, the enthalpy change of a chemical system represents the potential energy change of the system. Lesson 2 3. Define activation energy. Sketch a diagram that illustrates the concept of activation energy using the concept of bond energy . Answer (3 Marks) Activation is the minimum amount of energy needed for a reaction to occur. O + O + energy -> O2 Energy Energy needed for bonds to be formed Use the following information to answer the next two questions. When solid potassium is placed in a beaker of water at room temperature, an immediate, violent reaction occurs: 2 2 2 K(s) + 2 H O(l) 2 KOH(aq) + H (g) + energy → 4. Sketch and label an energy pathway diagram for this reaction. Your diagram should include: • labelling of the X and Y axes • general shape of the energy pathway
Chemistry 30 Unit B Module 3 Summative Assessment Page 3 of 13 • labeling of the reactant plateau, the product plateau, the activation energy (Ea) and the change in enthalpy (Δ r H) No specific numerical values are required. Answer (4 Marks) E a 2 K(s)+2 H2O(l) E p (kJ) Δ r H 2 KOH(aq) + H2(g) + energy Reaction progression 2 K(s) + 2 H2O(l) -> 2 KOH (aq) + H2 (g) + energy 5. Refer to the diagram you drew in Question 4. When solid potassium is placed in a beaker of water at room temperature, what should happen to the temperature of the water? Answer (1 Mark) The water should heat up because the potassium would meet the water and the thermal energy in the water would act as the activation energy, turning the K into KOH, releasing energy into the water.
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Chemistry 30 Unit B Module 3 Summative Assessment Page 4 of 13 View the “Catalyst Virtual Investigation” in Module 3 Lesson 2.3 Use the information in the Virtual Investigation to answer Questions 6-14. 6. Research! What are the safety concerns surrounding experiments using hydrogen peroxide? Include the WHMIS symbol(s) that should be displayed on a container of hydrogen peroxide. (Remember to use 2015 WHIMIS symbols) Answer (3 Marks) Safety concerns surrounding experiments using hydrogen peroxide are corrosion and oxidization. Hydrogen peroxide can cause irritation to skin and eyes if it comes in contact with it. Additionally, hydrogen peroxide is a very strong oxidizer, meaning it can intensify fires it comes in contact with. 7. T he “sizzling” sound in this experiment (amplified by the microphone) is caused by _____________________? Answer (1 Mark) The sizzling is caused by the hydrogen peroxide breaking into oxygen gas and water. The oxygen bubbles are what causes the sizzling sound. 8. Identify the liver enzyme that catalyzed the decomposition of hydrogen peroxide. Answer (1 Mark) Catalase is the enzyme that catalyzed the decomposition of hydrogen peroxide.
Chemistry 30 Unit B Module 3 Summative Assessment Page 5 of 13 9. Regarding the Catalyst Virtual Investigation, identify the following variables. Hint: Manipulated variables are conditions that are deliberately changed by the experimenter. Responding variables are conditions that change in response to the change in the manipulated variables. Controlled variables are conditions that could have changed but did not because of the intervention of the experimenter. Answer (4 Marks) Manipulated Variable The type of catalyzer used (yeast, liver, manganese dioxide). Responding Variable Speed of H2O2 decomposition. Controlled Variables (Identify two (2)) Pressure of the experiment. Type of solvent used (H2O2) 10. Design a data chart to collect and record data while watching the Catalyst Virtual Investigation. In your chart, list every catalyst used and describe the effect of the catalyst on the relative reaction rate. To gauge the speed of the reaction, use the amount of bubbling (as evidenced by the sound). Answer (3 Marks) Catalyst used Relative reaction rate No catalyst No evidence of decomposition Manganese dioxide High decomposition rate. Yeast Low decomposition rate. Liver Medium decomposition rate. 11. Refer again to the Catalyst Virtual Investigation. For the following system, record the initial and final temperatures. Answer (2 Marks) System Initial temperature ( o C) Final temperature ( o C)
Chemistry 30 Unit B Module 3 Summative Assessment Page 6 of 13 Hydrogen peroxide and manganese dioxide catalyst 21.1 o C 24.2 o C 12. Based on the temperature change of the surroundings, classify the decomposition of hydrogen peroxide as endothermic or exothermic. Answer (1 Mark) It would be an exothermic reaction because the decomposition would break bonds and release heat. 13. Sketch an energy pathway diagram that includes the activation energy and the catalyzed activation energy for the decomposition of hydrogen peroxide. Answer (2 Marks) Normal reaction E p (kJ) E a With catalyst E a catalyzed Reaction Progression H2O2 -> H2 + O2 + energy 14. Suggest how this experiment might be improved. Answer (1 Mark)
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Chemistry 30 Unit B Module 3 Summative Assessment Page 7 of 13 The experiment could be improved by covering up the container so that heat would not be lost to the environment. Use the following information to answer Questions 15-18. Sucrose, commonly known as table sugar, will be hydrolyzed to fructose and glucose in the presence of the enzyme sucrase. The reaction equation for this hydrolysis is sucrase 12 22 11 2 6 12 6 6 12 6 C H O (s) + H O(l) C H O (s) + C H O (s) ⎯⎯⎯→ The energy changes for this reaction are diagramed below. The blue line represents the reaction progress with sucrase and the red line represents the reaction progress without sucrase. 15. The enzyme sucrase will (1 Mark) A. increase the reaction rate of the hydrolysis of sucrose. B. provide an alternate pathway, with higher Ea, for the hydrolysis of sucrose C. lower the value of ΔH.
Chemistry 30 Unit B Module 3 Summative Assessment Page 8 of 13 D. change the reaction from exothermic to endothermic Answer: A 16. Because it lowers the activation energy, the enzyme sucrase is classified as a _______. Answer (1 Mark) Catalyst. 17. Describe how adding a catalyst to a reaction system affects the enthalpy change for the overall reaction. Answer (2 Marks) Adding a catalyst does not affect the enthalpy change because catalysts only lower the activation energy needed for a reaction, and would not affect the enthalpy change for the overall reaction. 18. Identify which energy value is indicated by each of the numbers in the above energy pathway diagram. Answer (5 Marks) Number Energy value 3 Change in enthalpy for both forward and reverse reaction 4 Uncatalyzed activation energy for the forward reaction 5 Uncatalyzed activation energy for the reverse reaction 2 catalyzed activation energy for the reverse reaction 1 catalyzed activation energy for the forward reaction
Chemistry 30 Unit B Module 3 Summative Assessment Page 9 of 13 Lesson 3 Use the following information to answer Questions 19-23 Dinitrogen pentaoxide, N 2 O 5 (g), is a strong oxidizer that forms explosive mixtures with organic compounds and ammonium salts. At standard state, dinitrogen pentaoxide decomposes into NO 2 and O 2 according to the following equation. 2 5 2 2 2 N O (g) + 219 kJ 4 NO (g) + O (g) → 19. The above reaction is __i__ and the standard enthalpy of reaction is __ii__. The statement above is completed by the information in row_____. (1 Mark) Row i ii A. endothermic r H o = + 219 kJ B. endothermic r H o = - 219 kJ C. exothermic r H o = + 219 kJ D. exothermic r H o = - 219 kJ 20. Calculate the standard molar enthalpy of reaction for dinitrogen pentaoxide. Answer (2 marks) +219kJ/2 mol N2O5(g) = +109.5kJ/mol N2O5(g) 21. Sketch and label a chemical potential energy diagram for the standard molar enthalpy of reaction for dinitrogen pentoxide. Indicate the enthalpy change using r as a subscript. Answer (3 marks)
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Chemistry 30 Unit B Module 3 Summative Assessment Page 10 of 13 E p (kJ) E a E r Reaction progression 2 N2O5(g) + 219kJ -> 4 NO2(g) + O2(g) 22. When 10.0 mol of nitrogen dioxide is produced in the above reaction, the enthalpy change is ____kJ Answer (1 Mark) 547.5 kJ 23. Is energy absorbed or released in the above reaction? Answer (1 Mark) Energy is absorbed. Use the following information to answer Questions 24 to 27.
Chemistry 30 Unit B Module 3 Summative Assessment Page 11 of 13 Galvanizing is the process of coating an object with zinc. When exposed to oxygen, zinc forms an oxide coating that protects the metal from further corrosion. At standard state, this reaction is represented by the following equation. 1 2 2 Zn(s) + O (g) ZnO(s) + 350.5kJ → 24. Sketch and label a chemical potential energy diagram for the process shown in the previous information box. Indicate the standard enthalpy of reaction using r as a subscript. Answer (3 marks) E p E a E r Reaction progression Zn(s) + ½ O2 -> ZnO(s) + 350.5kJ
Chemistry 30 Unit B Module 3 Summative Assessment Page 12 of 13 25. The formation of zinc oxide is classified as an __i_(endothermic/exothermic) reaction, and the reactants have __ii__ (less/more) potential energy than the products. Answer (2 Marks) i Exothermic ii less 26. When the above reaction occurs, it is expected that the temperature of the surroundings will __i__ (decrease/increase). This change in temperature would indicate that the surroundings are undergoing a change in __ii__ (kinetic/potential) energy . Answer (2 Marks) i Increase ii kinematic 27. Calculate the standard enthalpy of reaction when 25.0 g of zinc oxide is produced. Show all work for full marks. Answer (2 Marks) 350.5kJ/1mol=350.5x25g=8762.5kJ/mol
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Chemistry 30 Unit B Module 3 Summative Assessment Page 13 of 13 Lesson 4 Use the following information to answer Questions 28 and 29. Welding utilizes a variety of fuels. Two such fuels identified for comparison are acetylene (ethyne C 2 H 2 (g)) and propylene (propene C 3 H 6 (g)). Fuel Molar enthalpy of combustion (kJ/mol) acetylene -1 300.8 propylene -2 058.1 28. Calculate and compare the values of the enthalpy of combustion in kJ/g for each fuel. Answer (3 Marks) Acetylene: -1300.8kJ/mol x 1/26.038 g/mol= 49.96 kJ/g Propylene: -2058.1kJ/mol x 1/42.081g/mol= 48.91kJ/g 29. Describe two other factors that can be used to evaluate the fuel. Answer (2 Marks) 1. Which fuel is more economically viable? 2. Which fuel is more readily available?

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