{"id":3065,"date":"2023-10-04T10:44:15","date_gmt":"2023-10-04T10:44:15","guid":{"rendered":"http:\/\/localhost\/ecole9ja\/?p=3065"},"modified":"2023-10-04T10:48:29","modified_gmt":"2023-10-04T10:48:29","slug":"week-1-ss2-second-term-chemistry-notes","status":"publish","type":"post","link":"https:\/\/ecolebooks.com\/nigeria\/posts\/week-1-ss2-second-term-chemistry-notes\/","title":{"rendered":"Week 1 – SS2 Second Term Chemistry Notes"},"content":{"rendered":"

SECOND TERM E-LEARNING NOTE
\n<\/strong>SUBJECT: CHEMISTRY\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0CLASS: SS2
\n<\/strong>
\n\u00a0SCHEME OF WORK
\n<\/strong>
\n\u00a0WEEK\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0TOPIC
\n<\/strong><\/p>\n

    \n
  1. Rates of Chemical Reaction\n<\/li>\n<\/ol>\n
      \n
    • Meaning of Rate of Chemical Reaction.\n<\/li>\n
    • Rate Curve.\n<\/li>\n
    • The Collision Theory.\n<\/li>\n
    • \n
      Factors Affecting Rate of Chemical Reactions.\n<\/div>\n

      2. \u00a0\u00a0\u00a0\u00a0Exothermic and Endothermic Reactions\n<\/li>\n

    • Heat Content (Enthalpy) of a Substance.\n<\/li>\n
    • Thermodynamics: First and Second Laws.\n<\/li>\n
    • Entropy and Free Energy.\n<\/li>\n<\/ul>\n
        \n
      1. Chemical Equilibrium\n<\/li>\n<\/ol>\n
          \n
        • Reversible Reactions\n<\/li>\n
        • Le Chatelier’s Principle.\n<\/li>\n
        • Factors Affecting Chemical Equilibrium.\n<\/li>\n
        • Equilibrium Constant.\n<\/li>\n<\/ul>\n
            \n
          1. Oxygen and its Compounds\n<\/li>\n<\/ol>\n
              \n
            • General Properties of Oxygen Family.\n<\/li>\n
            • Electronic Structure and Bonding in Oxygen.\n<\/li>\n
            • Preparation, Properties and Uses of Oxygen.\u00a0\u00a0\u00a0\u00a0\n<\/li>\n
            • Oxides: Classification.\n<\/li>\n<\/ul>\n
                \n
              1. Chlorine and other Halogens\n<\/li>\n<\/ol>\n
                  \n
                • Electronic Configuration of Halogens\n<\/li>\n
                • Physical and Chemical Properties of Halogens.\n<\/li>\n
                • Laboratory and Industrial Preparation of Chlorine.\n<\/li>\n
                • Compound of Chlorine: Hydrogen Chloride.\n<\/li>\n
                • Test for Chlorides.\n<\/li>\n<\/ul>\n
                    \n
                  1. Nitrogen\n<\/li>\n<\/ol>\n
                      \n
                    • General Properties of Nitrogen Family.\n<\/li>\n
                    • Laboratory Preparation and Industrial Preparation of Nitrogen.\n<\/li>\n
                    • Properties and Uses of Nitrogen.\n<\/li>\n
                    • Nitrogen Cycle.\n<\/li>\n<\/ul>\n
                        \n
                      1. Compounds of Nitrogen\n<\/li>\n<\/ol>\n
                          \n
                        • Oxides of Nitrogen\n<\/li>\n
                        • Ammonia: Preparation, Properties and Uses.\n<\/li>\n
                        • Trioxonitrate (V) acid: Preparation, Properties and Uses.\n<\/li>\n<\/ul>\n
                            \n
                          1. Sulphur\n<\/li>\n<\/ol>\n
                              \n
                            • General Properties of Sulphur Group.\n<\/li>\n
                            • Electronic Structure of Members of Sulphur Group.\n<\/li>\n
                            • Allotropes of Sulphur.\n<\/li>\n
                            • Uses of Sulphur.\n<\/li>\n<\/ul>\n
                                \n
                              1. Compounds of Sulphur\n<\/li>\n<\/ol>\n
                                  \n
                                • H2<\/sub>S, SO2<\/sub> and SO3<\/sub>: Preparation, Properties and Uses\n<\/li>\n
                                • Tetraoxosulphate (VI) acid: Industrial Preparation (Contact Process).\n<\/li>\n<\/ul>\n
                                    \n
                                  1. Revision\n<\/li>\n<\/ol>\n

                                    \u00a0REFERENCES<\/strong><\/p>\n

                                      \n
                                    • New School Chemistry for Senior Secondary School by O.Y.Ababio (6th<\/sup> edition)\n<\/li>\n
                                    • Calculations on Chemistry by E.U. Akusoba and G.O. Ewelukwa\n<\/li>\n
                                    • WASSCE past Questions and Answers on Chemistry\n<\/li>\n
                                    • \n
                                      UTME past Questions and Answers on Chemistry\n<\/div>\n

                                      \u00a0
                                      \n\u00a0<\/li>\n<\/ul>\n

                                      WEEK ONE\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<\/strong>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0DATE: <\/strong>_________
                                      \nTOPIC<\/strong>: RATE OF REACTION<\/strong>
                                      \n\tCONTENT<\/strong><\/p>\n

                                        \n
                                      • Meaning of Rate of Chemical Reaction.\n<\/li>\n
                                      • Rate Curve.\n<\/li>\n
                                      • The Collision Theory.\n<\/li>\n
                                      • Factors Affecting Rate of Chemical Reactions\n<\/li>\n<\/ul>\n

                                        MEANING OF RATE OF REACTION
                                        \n<\/strong>The rate of a chemical reaction is the number of moles of reactants converted or products formed per unit time. <\/p>\n

                                        \u00a0Usually, rate of reaction is determined experimentally by measuring change in concentration of one of the components in the reaction with time. <\/p>\n

                                        \u00a0Thus,
                                        \nRate of reaction = change in concentration of reactant or product (mol\/dm3<\/sup>)
                                        \n\t Time taken for the change (seconds)
                                        \nThe unit of the rate of reaction is mol\/dm-3<\/sup>s-1<\/sup> or g dm-3<\/sup>s \u20131<\/sup>.
                                        \nRate of reaction can also be expressed as:
                                        \nRate of reaction = change in number of mole or mass of reactant or product
                                        \n\t Time taken for the change
                                        \nThen the unit of rate is mols-1<\/sup> or gs-1
                                        \n<\/sup>
                                        \n\u00a0EXAMPLE<\/strong>: When 0.5g of calcium trioxocarbonate (IV) was added to excess dilute hydrochloric acid, carbon (IV) oxide was evolved. The complete reaction took 5 minutes. What was the rate of reaction?
                                        \nSOLUTION:
                                        \nRate of reaction = change in mass of reactant
                                        \n\t Time taken for the change
                                        \n\u00a0\u00a0\u00a0\u00a0= (0.5 \u2013 0)g = 0.5
                                        \n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a05×60 300
                                        \n\u00a0\u00a0\u00a0\u00a0= 1.67 x 10-3<\/sup> gs-1
                                        \n<\/sup>
                                        \n\u00a0WAYS OF MEASURING REACTION RATE
                                        \n<\/strong>Concentration is one of the properties of a reaction that can change with time.
                                        \nThe following properties can also change with time and can thus be used to measure rate of reaction.<\/p>\n

                                          \n
                                        1. Decrease in mass of reaction system\n<\/li>\n
                                        2. Volume of gaseous product\n<\/li>\n
                                        3. Amount of precipitate formed\n<\/li>\n
                                        4. Change in colour intensity\n<\/li>\n
                                        5. Change in pH\n<\/li>\n
                                        6. Change in total gas pressure\n<\/li>\n<\/ol>\n

                                          \u00a0RATE CURVE
                                          \n<\/strong>The rate curve is a graphical illustration of the rate of a reaction.
                                          \nThe following graph illustrate rate curve\"\"\/<\/p>\n

                                          \u00a0\"\"\/<\/p>\n

                                          \u00a0
                                          \n\u00a0
                                          \n\u00a0
                                          \n\u00a0
                                          \n\u00a0\"\"\/<\/p>\n

                                          \u00a0FEATURES OF RATE CURVE
                                          \n<\/strong><\/p>\n

                                            \n
                                          1. It passes through the origin. This is because there is no change in concentration or mass at the start of reaction.\n<\/li>\n
                                          2. It steeps at first, this because the rate is fast at the beginning.\n<\/li>\n
                                          3. It becomes less steep later. This is because the rate slows down.\n<\/li>\n
                                          4. It finally becomes horizontally. This is because the reaction has reached the end points.\n<\/li>\n<\/ol>\n

                                            \u00a0The following can be determined from the rate curve<\/p>\n

                                              \n
                                            1. Average rate of reaction\n<\/li>\n<\/ol>\n

                                              Average rate = total number of mole \/ mass involved
                                              \n\t\u00a0\u00a0\u00a0\u00a0Time taken <\/p>\n

                                                \n
                                              1. Rate at a particular instant during the reaction\n<\/li>\n<\/ol>\n

                                                Rate at instant = Gradient at a point on the curve
                                                \nWhen the rate of reaction has direct variation with concentration, then
                                                \n Rate of reaction \u03b1[Concentration of A]
                                                \n R \u03b1 [A]
                                                \n R = k[A]
                                                \nWhere k is called Rate constant<\/p>\n

                                                \u00a0EVALUATION
                                                \n<\/strong><\/p>\n

                                                  \n
                                                1. What is rate of reaction?\n<\/li>\n
                                                2. \n
                                                  State two ways of measuring reaction rate\n<\/div>\n

                                                  \u00a0<\/li>\n<\/ol>\n

                                                  COLLISION THEORY
                                                  \n<\/strong>The collision theory states that for a chemical reaction to occur the reactant particles must collide and they must collide with a certain minimum amount of energy known as activation
                                                  \nenergy.<\/p>\n

                                                  \u00a0Reacting particles are in continuous motion, thus they possess energy and they also collide with one another. Not all collisions result into chemical reaction. Collisions, which result into chemical reaction, are called EFFECTIVE COLLISIONS. Minimum amount of energy required by reacting particles for chemical reaction to occur is called ACTIVATION ENERGY. Activation energy is the ENERGY BARRIER the reactants must overcome for reaction to occur. It is the minimum energy required for bond breaking for chemical reaction to occur. <\/p>\n

                                                  \u00a0Chemical reaction occur only when the energy of the colliding reactant particles is equal to or more than the activation energy. Activation energy must be equal to energy barriers also for chemical reaction to occur.<\/p>\n

                                                  \u00a0Every reaction has its own energy of activation. Reactions with low activation energy have high rate of reaction and occur spontaneously. Reaction with high activation energy have low rate of reaction and are not spontaneous.<\/p>\n

                                                  \u00a0The graph below illustrates the concepts of the activation energy for endothermic and exothermic reactions.<\/p>\n

                                                  \u00a0EXOTHERMIC REACTION\u00a0\u00a0\u00a0\u00a0ENDOTHERMIC REACTION<\/p>\n

                                                  \u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0
                                                  \n\u00a0From graph, it can be seen that
                                                  \n1. \u00a0\u00a0\u00a0\u00a0Both exothermic and endothermic reactions generally require an initial input of energy to overcome the activation energy barriers.
                                                  \n2. \u00a0\u00a0\u00a0\u00a0Exothermic reaction once started proceed without any further external energy supply e.g burning of kerosene
                                                  \n3.Endothermic reaction proceeds with continuous supply of external energy e.g cooking of rice.<\/p>\n

                                                  \u00a0EVALUATION
                                                  \n<\/strong><\/p>\n

                                                    \n
                                                  1. State collision theory.\n<\/li>\n
                                                  2. Graphically differentiate exothermic reaction from endothermic reaction.\n<\/li>\n<\/ol>\n

                                                    \u00a0FACTORS AFFECTING RATE OF REACTION
                                                    \n<\/strong>From the collision theory, it can be seen that rates of reaction depends on the following features.<\/p>\n

                                                      \n
                                                    1. The energy of the particle.\n<\/li>\n
                                                    2. The frequency of collision of the reaction.\n<\/li>\n
                                                    3. The activation energy of the reaction.\n<\/li>\n<\/ol>\n

                                                      \u00a0These features of a chemical reaction are in turn affected by some factors, which can make them to change and consequently affect the rate of reaction. These are factors that affect the rate of reactions. Some important ones are:<\/p>\n

                                                        \n
                                                      1. Nature of reactants.\n<\/li>\n
                                                      2. Concentration \/ pressure (for gases) of reactants.\n<\/li>\n
                                                      3. Surface area of reactants\n<\/li>\n
                                                      4. Temperature of reaction mixture\n<\/li>\n
                                                      5. Presence of light\n<\/li>\n
                                                      6. Presence of catalysts\n<\/li>\n<\/ol>\n

                                                        To study the effect of any one of these factors on rate of reaction all other factors must be kept constant.<\/p>\n

                                                        \u00a0EFFECT OF NATURE OF REACTANTS
                                                        \n<\/strong>If all other factors are kept constant, different substances will have different rate of reaction with dilute HCl, for example. When dilute HCl reacts with zinc, iron and gold under the same condition, hydrogen gas is evolved fast with zinc, slow with iron and no gas evolved with gold.<\/p>\n

                                                        \u00a0The difference in rate of reaction is due to the chemical nature of the elements as they naturally posses different amount of energy content.<\/p>\n

                                                        \u00a0EFFECT OF CONCENTRATION OF REACTANTS
                                                        \n<\/strong>The frequency of collision among particles is high when the particles are crowded in a small space, i.e high concentration. This leads to high effective collision and thus high rate of reaction. An increase or decrease in the concentration of the reactants will result in corresponding increase or decrease in effective collisions of the reactants and hence the reaction rate.<\/p>\n

                                                        \u00a0EFFECT OF SURFACE AREA OF REACTANTS
                                                        \n<\/strong>This is a very important factor to be considered when a solid is involved in a chemical reaction. Lumped solids offer small surface area of contact for reaction while powdered solids offer large surface area for reaction. Rate of reaction is slow with lumped solid but high with powdered solids.<\/p>\n

                                                        \u00a0EFFECT OF TEMPERATURE
                                                        \n<\/strong>Increasing the temperature of a system can lead to an increase in reaction rate in two ways. When heat is raised, energy in form of heat is supplied to the reactant particles, so that<\/p>\n

                                                          \n
                                                        1. The number of particles with energy equal to or greater than the activation energy increases.\n<\/li>\n
                                                        2. The velocity of all the reactant particles increases due to the greater kinetic energy, leading to a higher frequency of collision.\n<\/li>\n<\/ol>\n

                                                          As a result, the number of effective collisions increases and the reaction proceeds at a faster rate. Decreases in temperature leads to decrease rate of reactions.<\/p>\n

                                                          \u00a0EFFECT OF LIGHT
                                                          \n<\/strong>Some reactions are influenced by light. The rate of reaction is high when the lights intensity is high, low when the intensity is low and does not proceed at all in the absence of light. Such reactions are known as photochemical reaction. Examples of photochemical reactions
                                                          \ninclude.<\/p>\n

                                                            \n
                                                          1. Reaction between hydrogen and chlorine and\n<\/li>\n
                                                          2. Decomposition of hydrogen peroxide\n<\/li>\n
                                                          3. Reactions between methane and chlorine\n<\/li>\n
                                                          4. Photosynthesis in plant\n<\/li>\n
                                                          5. \n
                                                            Conversion of silver halides to grey metallic silver.\n<\/div>\n

                                                            \u00a0<\/li>\n<\/ol>\n

                                                            EFFECT OF CATALYST
                                                            \n<\/strong>A Catalyst is a substance, which alters the rate of a reaction, but itself does not undergo any change at the end of the reaction.
                                                            \nA positive catalyst increases the rate of reaction by lowering the activation energy of the reaction whereas, the one which increases the activation energy is known as a negative catalyst or an inhibitor.
                                                            \nThe diagram below illustrates the energy profile for catalyzed and uncatalyzed exothermic and endothermic reactions <\/p>\n

                                                            \u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0
                                                            \n\u00a0EXOTHERMIC REACTION ENDOTHERMIC REACTION<\/p>\n

                                                            \u00a0GENERAL EVALUATION\/REVISION
                                                            \n<\/strong><\/p>\n

                                                              \n
                                                            1. List and explain three factors that can affect the rate of reaction of the following reaction: CaCO3(s)<\/sub> + 2HCl(aq)<\/sub>\u2192 CaCl2(aq)<\/sub> + H2<\/sub>O(l)<\/sub> + CO2(g)<\/sub>\n\t\t<\/li>\n
                                                            2. In a chemical reaction, after 10seconds, 6moles from the initial concentration of 16moles of the reactant disappeared. Calculate the rate of the reaction.\n<\/li>\n
                                                            3. State THREE characteristics of catalyst.\n<\/li>\n
                                                            4. What is the volume in dm3<\/sup> of 8g of oxygen gas at s.t.p?\n<\/li>\n
                                                            5. Calculate the percentage of water in sodium trioxocarbonate (VI) heptahydrate\n<\/li>\n<\/ol>\n

                                                              \u00a0READING ASSIGNMENT<\/strong>: New School Chemistry for Senior Secondary School by O.Y.Ababio (6th<\/sup> edition) pages 250-261<\/p>\n

                                                              \u00a0WEEKEND ASSIGNMENT
                                                              \n<\/strong>SECTION A: <\/strong>Write the correct option ONLY
                                                              \n\t\t<\/strong><\/p>\n

                                                                \n
                                                              1. The minimum amount of energy that colliding molecules must possess for their collisions to be effective is a. thermal energy b. collision energy\n<\/li>\n<\/ol>\n

                                                                c. activation energy d. kinetic energy
                                                                \n2.Zn(s)<\/sub> + H2<\/sub>SO4(aq)<\/sub> \u2192 ZnSO4(aq)<\/sub> + H2(g)<\/sub>
                                                                \n\t\u00a0\u00a0\u00a0\u00a0The rate of evolution of hydrogen gas in the above reaction will be greatly increased if a. the zinc is in the form of pellets b. a smaller volume of H2SO4 is used c. the reaction flask is immersed in an ice bath d. the zinc is in powdered form
                                                                \n\t\t<\/sup><\/p>\n

                                                                  \n
                                                                1. The units of rate of reactions is a. moldm-3<\/sup>s-1<\/sup> b. mol-1<\/sup>s-1<\/sup> c. mol-1<\/sup> d. smol-1<\/sup>\n\t\t<\/li>\n
                                                                2. \n
                                                                  If 2g of zinc granules was reacted with excess dilute HCl to evolve hydrogen gas which\n<\/div>\n

                                                                  came to completion after 5min. Calculate the rate of the chemical reaction in ghr-1<\/sup>
                                                                  \n\t\t\ta. 48ghr-1<\/sup> b. 12ghr-1<\/sup> c. 24ghr-d<\/sup> d 240ghr-1<\/sup>\n\t\t\t<\/li>\n

                                                                3. What do we do to increase the surface area of solid reactants to high rate of reaction? a. grinding them into powder b. subjecting the reactants to high pressure c. altering the directing of the reaction d. using reactants of different densities.\n<\/li>\n<\/ol>\n

                                                                  \u00a0SECTION B
                                                                  \n<\/strong>1a.\u00a0\u00a0\u00a0\u00a0Define rate of reaction
                                                                  \n b.\u00a0\u00a0\u00a0\u00a0State the collision theory
                                                                  \n2a.\u00a0\u00a0\u00a0\u00a0Explain in terms of collision theory, how rate of gaseous reaction is affected by an increase in pressure
                                                                  \n b.\u00a0\u00a0\u00a0\u00a0Give the reason why red-hot iron wool reacts more readily with oxygen than red-hot iron nail
                                                                  \n
                                                                  \n\t\t<\/strong>\u00a0<\/p>\n","protected":false},"excerpt":{"rendered":"

                                                                  SECOND TERM E-LEARNING NOTE SUBJECT: CHEMISTRY\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0CLASS: SS2 \u00a0SCHEME OF WORK \u00a0WEEK\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0TOPIC Rates of Chemical Reaction…<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1,248],"tags":[],"class_list":["post-3065","post","type-post","status-publish","format-standard","hentry","category-posts","category-second-term-ss2-chemistry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3065","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/comments?post=3065"}],"version-history":[{"count":1,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3065\/revisions"}],"predecessor-version":[{"id":3066,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3065\/revisions\/3066"}],"wp:attachment":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/media?parent=3065"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/categories?post=3065"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/tags?post=3065"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}