Year 12 Chemistry acidic environment Le Chatelier s principle

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1 CD321 cd321 Year 12 Chemistry acidic environment first name last name cd321

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3 3 syllabus Students learn to: Students: 2. While we usually think of the air around us as neutral, the atmosphere naturally contains acidic oxides of carbon, nitrogen and sulfur. The concentrations of these acidic oxides have been increasing since the Industrial Revolution identify oxides of non-metals which act as acids and describe the conditions under which they act as acids analyse the position of these nonmetals in the Periodic Table and outline the relationship between position of elements in the Periodic Table and acidity/basicity of oxides define Le Chatelier s principle identify factors which can affect the equilibrium in a reversible reaction describe the solubility of carbon dioxide in water under various conditions as an equilibrium process and explain in terms of Le Chatelier s principle identify data, plan and perform a first-hand investigation to decarbonate soft drink and gather data to measure the mass changes involved and calculate the volume of gas released at 25 C and 100kPa analyse information from secondary sources to summarise the industrial origins of sulfur dioxide and oxides of nitrogen and evaluate reasons for concern about their release into the environment identify natural and industrial sources of sulfur dioxide and oxides of nitrogen describe, using equations, examples of chemical reactions which release sulfur dioxide and chemical reactions which release oxides of nitrogen assess the evidence which indicates increases in atmospheric concentration of oxides of sulfur and nitrogen calculate volumes of gases given masses of some substances in reactions, and calculate masses of substances given gaseous volumes, in reactions involving gases at 0 C and 100kPa or 25 C and 100kPa explain the formation and effects of acid rain

4 Classification of oxides Metallic oxides Most oxides of metals are bases and, if soluble in water, e.g. Group I oxides and CaO and BaO, they form alkaline solutions. Some insoluble oxides are MgO, CuO, Fe2O3and Ag 2O. They can be neutralised by strong acids to form salts and water. Common basic oxides include: Na O, MgO, CaO, FeOand CuO. For example: 2 CaO s 2HCl CaCl H O 2 2 Soluble basic oxides react with water to form alkaline solutions. Alkaline solutions contain hydroxide ions. Red litmus turns purple in these solutions. All Group I oxides are soluble in water. For example: 2 2 K O s H O 2K 2OH Non-metallic oxides Non-metallic oxides are often acidic (although some are neutral). They can be neutralised by strong bases to form salts and water. Common acidic oxides include: CO 2, NO 2, SO 2, SO 3 and P4O 10. For example: CO g 2KOH K CO H O Phosphorus pentoxide reacts with water to form phosphoric acid. P O s 6H O l 4H PO aq Table (1) summarises properties of metal oxides and non-metal oxides. Property Metal oxide Non-metal oxide Bonding Strong ionic bonds extend throughout the lattice Strong covalent intramolecular bonds (within the molecule). Weak intermolecular forces (between molecules) State at room temperature Solid Gas MP, BP High Low Table (1) Properties of metal oxides and non-metal oxides

5 5 Neutral oxides The neutral non-metallic oxides include: CO, NO and N2O. Amphoteric oxides Some oxides are amphoteric. Amphoteric oxides can be neutralised by either an acid or a base. Common amphoteric oxides include: Al2O 3, ZnO, PbO, SnO and As2O 3. For example: ZnO as a base: ZnO s H SO ZnSO H O A solution of zinc sulfate forms Al O 3H 6H O 2 Al H aq Al O 3H 2O 2Al OH aq Question 1 Which of the following is not correct about metallic oxides? (A) (B) (C) (D) Metallic oxides are basic. Metallic oxides are ionic compounds Metallic oxides react with acids to produce salt and water Metallic oxides do not dissolve in water at all Question 2 Which of the following is correct about acidic oxides? (A) (B) (C) (D) Non-metallic oxides are acidic oxides Acidic oxides react with acids to produce water and salt All non-metallic oxides are acidic Acidic oxides are ionic substances Question 3 Which of the following correctly explains amphoteric oxides? (A) (B) (C) (D) Amphoteric oxides can react with water Amphoteric oxides can be neutralised by either an acid or a base Amphoteric oxides can act as a Bronsted acid or base Amphoteric oxides are non-metallic oxides

6 6 Question 4 Classify the following oxides as acidic, basic, amphoteric or neutral: (a) Zinc oxide Nitrogen monoxide (c) Sulfur trioxide (d) Nickel oxide Question 5 Identify oxides which act as acids and describe the conditions under which they act as acids

7 Periodic trends of oxides The locations of basic, amphoteric and acidic oxides in the periodic table are shown in figure (1). Figure (1) Periodic table and oxide classification General trends of oxides in the Periodic table As metallic character increases, the basic property of an oxide increases. Oxides of elements in left hand side of the Periodic table are basic. Moving to the left of the Periodic table, the basic property of an oxide increases. Oxides of elements in right hand side of the Periodic table are acidic. Some of metallic oxides are amphoteric Some non-metallic oxides are not soluble in water and neutral Group VIII elements do not form oxides.

8 8 The following tables show properties of oxides of main groups in the Periodic Table. Group IV Table (2) Properties of group IV oxides GROUP IV Carbon dioxide CO 2 Silicon dioxide SiO 2 Structure covalent molecular covalent network Physical properties gas at room temperature solid at room temperature Effect on living things essential as a source of carbon for photosynthesis Effect on the rate of emission of CO 2, and atmosphere other greenhouse gases is increasing; in the case of CO 2, this is mainly due to fossil-fuel burning Chemical properties Group V GROUP V and deforestation soluble in water forming an acidic solution containing 5 H2CO3 K a , this accounts for the acidity of carbonated water; reacts with hydroxide ions to form carbonates and hydrogen carbonates in solution almost insoluble 10 about 10 K a forms a wide range of silicates with the hydroxide ion Table (3) Properties of group V oxides Acidic oxides of nitrogen Acidic oxides of phosphorus nitrogen dioxide NO 2, dinitrogen phosphorus (III) oxide P2O 3, trioxide N2O 3, dinitrogen pentoxide phosphorus (IV) oxide PO 4 10 NO 2 5 Structure covalent molecular covalent molecular Effect on NO2 is a serious atmospheric pollutant atmosphere in photochemical smog formation in cities Chemical both the stated oxides of nitrogen are both oxides of phosphorus are water properties water soluble NO 2 3 is the anhydride of soluble; PO 2 3is the anhydride of Acid properties of the oxides nitrous acid HNO 2 (weak acid). 2 5 the anhydride of nitric acid HNO 3 (strong acid) NO 2 5is strongly acidic; NO 2 3 is weakly acidic NO is Note: The acidic nature of the oxides of Group V decreases down the group. orthophosphorous acid H3PO 3; PO 4 10 is the anhydride of orthophosphoric acid H 3 PO 4 PO 2 3 is weakly acidic (weaker than NO 2 3); PO 4 10 is strongly acidic

9 9 Group VI Table (4) Properties of group VI oxides GROUP VI Sulfur dioxide SO 2 Sulfur trioxide SO 3 Structure covalent molecular covalent molecular Physical SO 2 is a gas at room temperature SO 3 is a solid at room temperature properties (melting point 62 C) Effect on atmosphere increases in the amount of sulfur dioxide in the atmosphere have led to 'acid rain', particularly in cities in the Chemical properties Northern Hemisphere SO has a low solubility in water and 2 forms sulfurous acid H2SO 3; it reacts with hydroxide ions to form sulfites and hydrogen sulfites in solution SO 3 dissolves in water to form H SO, which is a strong acid; it 2 4 reacts with hydroxide ions to form sulfates and hydrogen sulfates in solution Group VII With the exception of F2 O, all the oxides are acidic. The oxides of chlorine are strong oxidants. ClO2 is used for bleaching in the paper industry and as a germicide. It is also used as an improving agent for flour. 2ClO 2 H2O HClO 2 HClO 3 Another oxide of chlorine, Cl2O 7, dissolves in water to form a powerful oxidising acid called perchloric acid HClO. 4

10 10 Question 6 Which of the following shows only neutral oxides? (A) CO, NO, NO 2 (B) CO, NO, N 2 O (C) CO 2, NO, N 2 O (D) CO, N 2 O 4, NO 2 Question 7 Complete the following general rules: (a) Oxides of non-metals are oxides. Oxides of metals are oxides. Question 8 Complete the key in the following Periodic Table to show which elements form acidic oxides, basic oxides, amphoteric oxides and which do not form any oxides. (a) (c) (d)

11 11 Question 9 Metals form basic oxides. Basic oxides will dissolve in water to form an hydroxide. Complete the following equation to illustrate this. Magnesium oxide water MgO(s) H O l Question 10 Basic oxides react with acids to form water and a salt. Use an equation to show the reaction of basic magnesium oxide with hydrochloric acid.

12 Equilibrium and Le Chatelier s principle Not all chemical reactions proceed to completion. Many reactions are reversible. As a reaction proceeds, the rate of the forward reaction decreases as the reactants are consumed. The increasing concentration of products leads to an increase in the reverse reaction rate in which reactants are reformed. Eventually, a dynamic equilibrium state is reached when the rate of the forward reaction exactly equals the rate of the reverse reaction. In a reversible reaction there will always be some reactants and products present. The characteristics of a system at equilibrium are: Closed system - no matter or energy can enter or leave. Macroscopic properties are constant - colour, pressure, state and temperature do not change. Concentrations of reactants and products are constant. Microscopic changes continually take place between reactants and products. Rate of forward reaction Rate of reverse reaction.

13 13 When a catalyst is added to a reversible system it lowers the activation energy for both the forward and reverse reactions. The rates of both the forward and reverse reactions are increased equally so that the catalyst does not affect the relative proportions of reactants and products. Le Chatelier s principle If a change is made to an equilibrium system, then the system alters in a way that counteracts the change. Various factors can affect the equilibrium in a reversible reaction. These include the following. Concentration If the concentration of a reactant is increased for a system in equilibrium, then the forward reaction rate increases and the position of the equilibrium is shifted to the product side. If the concentration of a product is increased, the equilibrium shifts back to the side of the reactants.

14 14 Concentration examples A solution of potassium dichromate is prepared. It is orange-yellow in colour. Cr O H O l 2CrO 2H orange yellow Diluting the system with water: The solution becomes more yellow as the additional water causes the equilibrium to shift to the product side. Adding hydrochloric acid: The solution becomes more orange as the additional hydrogen ions causes the equilibrium to shift to the reactant side. A cobalt chloride solution is pink. The addition of concentrated hydrochloric acid (a source of Cl ) causes the system to change from pink to a blue-purple colour. Le Chatelier s principle explains this observation. The addition of more product(cl ) changes the equilibrium. To counteract the change, the concentration of chloride ions must be reduced. This is achieved by some chloride ions reacting with the pink cobalt ions to form the blue cobalt ions. Thus, the equilibrium shifts to the left to counteract the change. 2+ CoCl 6H O Co H O 4Cl Blue pink Total gas pressure In a system involving gases, the application of pressure (by reduction in volume of the vessel) will lead to a shift in the equilibrium that favours the side of the equilibrium with lower amounts of reacting substances. If volume increases, it causes a decrease in pressure. Or if volume decreases, it causes an increase in pressure. Each case will produce the same result of the corresponding pressure effect. Total gas pressure example A mixture of NO2 gas and NO 2 4 gas is in equilibrium. The mixture is pale brown at room temperature. 2NO g N O g Brown colourless If the reaction mixture is placed in a syringe and the volume slowly reduced so as not to heat up the gas, the mixture becomes a much lighter brown as the equilibrium shifts to the right (the product side has fewer molecules than the reactant side).

15 15 Temperature Some reactions are endothermic and others are exothermic. In an endothermic equilibrium, an increase in temperature causes the equilibrium to shift to the product side. In an exothermic equilibrium, an increase in temperature causes the equilibrium to shift to the reactant side. Type of reaction Effect on equilibrium when: Temperature increases Temperature decreases Exothermic reaction Shift left favours reactants Shift right favours products Endothermic reaction Shift right favours products Shift left favours reactants Temperature example Table (5) Effect of temperature on equilibrium The decomposition of magnesium carbonate is an endothermic process. MgCO s heat MgO s CO g 3 2 If the system is heated, then the equilibrium shifts to the right to produce more carbon dioxide gas. Thus, thermal decomposition of magnesium carbonate is favoured by high temperatures. Question 11 Which of the following is a correct statement of Le Chatelier s principle? (A) (B) (C) (D) An equilibrium system will always move to the left when it is heated. Increasing the pressure on a reaction vessel will increase the rate of reaction. The rate of reaction in an equilibrium system depends on the presence or absence of a catalyst. If a system is in equilibrium and it is changed in some way, then the system adjusts to minimise the change. Question 12 How is an equilibrium system represented in a chemical equation?......

16 16 Question 13 Which of the following is incorrect about dynamic equilibrium? (A) (B) (C) (D) Rate of forward reaction is equal to the rate of backward reaction The concentration of reactants is the same as the concentration of products Macroscopic properties are constant Microscopic properties continuously take place Question 14 (a) Which of the following reactions would not be affected by a change in the volume of the container? (A) 2NO2 g N2O4 g (B) H2g I2g 2HI g (C) 2CO2 g H2Ol H2CO3 aq (D) 2SO g O g 2SO g Explain your choice

17 17 Question 15 If the reaction 4NH g 5O 4NOg 6H Og the following changes on: is at equilibrium, what would be the effect of i. the concentrations of all the species, and ii. the rates of the forward and reverse reactions? (a) Adding more O 2 to the system. Reducing the concentration of NO. Question 16 (a) The equation 2SO g H Ol H SO aq represents an equilibrium system established in a closed container. What happens if the size of the container is increased? (A) (B) (C) (D) The equilibrium moves to the left. Less sulfur dioxide is produced. The equilibrium position is unchanged. Sulfurous acid is produced more rapidly. Explain the response of the system to the change.

18 18 Practice Questions Question 17 Which of the following shows only amphteric oxides? (A) Al 2 O 3, ZnO, SO 2 (B) O, N 2 O, CO (C) Al 2 O 3, ZnO, PbO (D) ZnO, MgO, PbO Question 18 Which of the following is incorrect about the general trends of oxides in the Periodic Table? (A) (B) (C) (D) Most oxides of elements in the right hand of the Periodic table are acidic Most oxides of elements in the left hand of the Periodic table are basic As metallic character increases the basic property of an oxide decreases Group VIII elements do not form oxides Question 19 Which of the following sets contains only compounds which are acidic in aqueous solution? (A) (B) (C) (D) Carbon dioxide, sulfur dioxide, dinitrogen monoxide Phosphorus pentoxide, nitrogen dioxide, sulfur dioxide Magnesium oxide, nitrogen monoxide, carbon dioxide Barium oxide, potassium oxide, magnesium oxide Question 20 Which of the following equations correctly shows an oxide dissolving in water to form an acid? (A) 2NO g O2g 2NO2g (B) CO2 g H2Ol H2CO3 aq (C) MgO s H2Ol Mg OH aq 2 (D) SO g H Ol H SO aq

19 19 Question 21 (a) Which two oxides of non-metals are only slightly soluble in water and form neutral solutions? (A) (B) (C) (D) Carbon monoxide and dinitrogen monoxide Carbon dioxide and sulfur dioxide Nitrogen monoxide and carbon dioxide Nitrogen dioxide and nitrogen trioxide State the formula for these two neutral oxides. Question 22 Rank the following oxides from most basic to most acidic. Cl2O 7, Sb2O 3, NO 2, BaO.

20 20 Question 23 Choose 3 oxides of elements in the third period of the Periodic Table. One must be an acidic oxide, one basic and one amphoteric. Use these examples to describe the meaning of these terms and give equations for reactions you describe.

21 21 Question 24 The following is a simplified Periodic table. (a) Which elements in the Periodic table form oxides that react with acids? Which elements in the Periodic table form oxides that react with bases? (c) Which elements in the Periodic table form oxides that react with both acids and bases? (d) Which elements in the Periodic table do not form oxides? (e) Which elements in the Periodic table form oxides that are neutral? Question 25 When does a chemical reaction reach a state of dynamic equilibrium?

22 22 Question 26 Outline any effect of a catalyst on an equilibrium reaction. Question 27 Consider the following equilibrium between the colourless gas dinitrogen tetroxide and the brown N O g 2NO g gas nitrogen dioxide: (a) When a sealed tube containing these gases in equilibrium is heated, the brown colour of the mixture darkens. Which statement explains this change? (A) (B) (C) (D) Equilibrium shifts to the right because the forward reaction is endothermic. Heating causes gases to expand so pressure increases and the reaction shifts right. Equilibrium shifts right because the forward reaction is exothermic. The deepening brown colour is due to the expansion of gases. Explain the effect of temperature changes on equilibrium reactions.

23 23 Question 28 When Ca OCl 2 is used to disinfect swimming pools, the following equilibrium is set up: Ca OCl aq 2H Ol 2HOCl aq Ca OH aq (a) What happens to the ph of the pool water when acid is added? (A) (B) (C) (D) The ph rises as acid is added and then falls. The ph falls and then rises towards its original value. The ph stays constant. The ph rises and stays higher than its original value. Explain your answer.

24 24 Question 29 (a) To which of the following equations would Le Chatelier s principle be applicable? (A) BaO s H2Ol Ba OH aq 2 (B) HCl aq NaOH aq H2Ol NaCl aq (C) CO2 g H2Ol H2CO3 aq (D) Mg s HCl aq MgCl aq H g 2 2 Under what conditions could Le Chatelier's principle be applied to this reaction? Question 30 Complete the following to summarise the characteristics of a reversible system that has reached equilibrium. (a) It is a system - no matter or energy enters or leaves the system. Macroscopic properties (e.g. state, colour, temperature and pressure) stay (c) Concentrations of reactants and products stay (d) Continual change occurs between reactants and products. (e) The rate of forward reaction rate of reaction.

25 25 Question 31 Brown NO 2 gas and colourless NO 2 4 gas are in equilibrium in a closed container at room temperature. The reaction is exothermic NO g N O g Use Le Chatelier s principle to predict the effect of the following changes to this equilibrium: (a) Cooling the vessel with ice. Compressing the gas mixture at constant temperature.

26 26 Question 32 The reaction for the production of carbon monoxide and hydrogen gases is: C s H O g CO g +H g. 2 2 If the system is at equilibrium what would be the effect of the following changes on: i. the concentrations of all the species, and ii. the rates of the forward and reverse reactions? (a) Increasing the volume of the system. Increasing the pressure on the system.

27 27 Question 33 If thesystem 2CO g O g 2CO g 564 kj is at equilibrium, what would be the effect of the following changes on: 2 2 i. the concentrations of all the species, and ii. the rates of the forward and reverse reactions? (a) Increasing the temperature. Reducing the temperature:

28 28 Question 34 Consider the reaction: 2SO g O g 2SO g 99kJ What would be the effect of adding a catalyst (a) Before the system reached equilibrium? After the system reached equilibrium?

29 29 Question 35 The following diagram shows changes in the concentration of a reaction below. N ( g) 3 H ( g) 2 NH ( g) 92 kj mol (a) What happens at the time period between T 1 and T 2 What happens at time T 2? (c) Describe the effect of the changes identified in part on equilibrium and draw changes in the concentrations of reactants and products on the graph above (d) What would be the effect if the temperature is increased on the equilibrium?

30 30 Question 36 The following diagram shows changes in the concentration of a reaction below. PCl ( g) Cl ( g) PCl ( g) 124 kj mol (a) If the volume of the reaction vessel is reduced at time T 1, what would happen to the concentrations of substances and equilibrium? Draw the changes identified in part (a) on the graph above. (c) If the concentration of PCl 5 is reduced at time T 2, what would happen to the equilibrium? (d) Draw the changes identified in part (c) on the graph above.

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