UNIT 4 TEST 4 (Chemical system & Equillibrium) 2023 SCH4U

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Oct 30, 2023

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Chemical systems & Equilibrium SCH4U Page 1 of 8 Student’s Name : Date: TEST # 04 Knowledge / Understanding Thinking/Inquiry Communication Application Marks 15 15 15 15 60 Part: A Knowledge/ Understanding (Marks-15) Multiple choice (Marks-10) F or each question select the best answer from the four alternatives. -------- 1. Complete the following sentence. A heterogeneous equilibrium involves more than one ------. a. phase b. reactant c. product d. catalyst --------- 2. . For an exothermic reaction that has reached equilibrium, which conditions will result in a shift to the left? a. removing products b. adding reactants c. adding thermal energy d. removing thermal energy -------- 3. Which is an exothermic process? a. ice melting b. water boiling c. water evapo rating d. water vapour condensing -------- 4. The total amount of potential energy and kinetic energy of a substance is called a. energy of motion b. conservation of energy c. energy composition d. thermal energy
Chemical systems & Equilibrium SCH4U Page 2 of 8 ---------- 5. The rate of reaction depends up on a. the concentration and nature of reaction b. the temperature of the reaction c. whether or not a catalyst was used d. all of the above -------6. Which of the following would react most rapidly? a. powered Zn in 1.M HCl at 40 0 C b. powdered Zn in 2.M HCl at 40 0 C c. A lump pf Zn in 2 M HCl at 25 0 C d. A lump of Zn in 1 M HCl at 40 0 C --------7. In a reaction mechanism the rate determining step is always a. the reaction intermediate b. the last step c. the slowest step d. the fastest step ------- 8. When a lit match is touched to the wick of a candle, the candle begins to burn. When the match is removed, the candle continues to burn. In this reaction the match a. behaves as a catalyst b. supplies activation energy c. is part of the rate determining step d. lowers the activation energy barrier ---------9. A chemical system in which both energy and matter can flow in to or out of a system is called as a. open system b. closed system c. isolated system d. a chemical system -------- 10. Which of the following indicates that a chemical reaction system Has reached equilibrium? a. the temperature of the system is decreasing. b. the volume of the system is changing c. the concentration of reactants is decreasing d. the concentration of the product is constant
Chemical systems & Equilibrium SCH4U Page 3 of 8 11. What are buffers? Describe the function of a buffer. (Marks- 3) 12. How did Arrhenius describe acids and bases? (Marks- 2) PART:B. THINKING/ INQUIRY (Marks-15) 1. Indicate whether each statement is true or false. If you think the statement is false, rewrite it to make it true. ( T/I= 5) i. An exothermic reaction hat is at equilibrium will shift to the left when products are removed. ii. In a dynamic equilibrium the concentration of reactants and products are always changing. iii. If the equilibrium constant ,K is equal to 1, the position of equilibrium favours products much more than reactants. iv. The solubility product constant K sp , is a constant for a given substance under all conditions.
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Chemical systems & Equilibrium SCH4U Page 4 of 8 v. The color of an acid base indicator depends on the P H of the solution. 2. What is the difference between a strong acid and a weak acid? ( I=2) 3. A chemist prepares a solution of magnesium oxide. (MgO). Write the hydrolysis reaction equation and predict whether the resulting solution will be acidic , basic or neutral? ( I=3) 4. Why does a wet towel dry out if hung over the back of a chair, but not if left in a plastic bag on the seat of the chair? ( I=2) 5. Write the equilibrium law expression for each of the following reactions. ( I=3) i. SO 2(g) + O 2 (g) -- SO 3 (g)
Chemical systems & Equilibrium SCH4U Page 5 of 8 ii. Ammonia reacts with oxygen to form nitrogen and water vapour. iii. NOBr( g) -- NO (g) + Br 2 (g) PART - C: COMMUNICATION (Marks - 15) 1. Write balanced chemical equations for the following reactions. Also write the equilibrium expressions.(C=4) i. Solid silver chloride dissolves to produce silver ions and chloride ions in solution. ii. Solid hydrogen cyanide dissolves to produce hydrogen ions and cyanide ions in solution. 2. Will an aqueous solution of each of the following salts will be acidic, basic or neutral? (Comm 3) i. sodium nitrate ii. ammonium bromide iii. sodium fluoride.
Chemical systems & Equilibrium SCH4U Page 6 of 8 3. a) Define P H ? (Comm. 1) b) If P H of a solution is 4.8, what is the colour of each of the following indicators in this solution? (Comm. 3) i. Phenolphthalein ii. bromocresol green iii. phenol red. 4. What are indicators? (Comm 1) 5. What are the characteristics of equilibrium? (Comm. 3)
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Chemical systems & Equilibrium SCH4U Page 7 of 8 PART – D: APPLICATION: (Marks - 15) Q1. A chemist dissolved some aspirin in water. The chemist then measured the P H of the solution and found it to be 2.73 at 25 0 C. What are the{ H 3 O + }and {OH -- } of the solution? ( App 5) Q2. A solution of hypochlorous acid HClO (aq) has a concentration of 0.100 mol/L . If the P H of the solution is 4.23 calculate the Ka of hypochlorous acid. ( App 3) Q3. Explain Lechtlier’s principle by taking the example of synthesis of ammonia as an example. ( App 4)
Chemical systems & Equilibrium SCH4U Page 8 of 8 Q4. Write the acid ionization constant equation for the following acids at equilibrium: i. Hydrocyanic acid (HCN) ii. Nitous acid ( HNO 2 )
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