Martin H. Fischer CHAPTER1 Chemical Reactions And Equations
“Facts are not science — as the dictionary is not literature.”Martin H. FischerCHAPTER1Chemical Reactionsand EquationsConsider the following situations of daily life and think what happenswhen – milk is left at room temperature during summers.an iron tawa/pan/nail is left exposed to humid atmosphere.grapes get fermented.food is cooked.food gets digested in our body.we respire.In all the above situations, the nature and the identity of the initialsubstance have somewhat changed. We have already learnt about physicaland chemical changes of matter in our previous classes. Whenever a chemicalchange occurs, we can say that a chemical reaction has taken place.You may perhaps be wondering as to what is actually meant by achemical reaction. How do we come to know that a chemical reactionhas taken place? Let us perform some activities to find the answer tothese questions.Activity 1.1 CAUTION: This Activity needsthe teacher’s assistance. Itwould be better if studentswear eye protection.Clean a magnesium ribbonabout 2 cm long by rubbingit with sandpaper.Hold it with a pair of tongs.Burn it using a spirit lamp orburner and collect the ash soformed in a watch-glass asshown in Fig. 1.1. Burn themagnesium ribbon keeping itas far as possible from youreyes.What do you observe?Figure 1.1Burning of a magnesium ribbon in air and collection of magnesiumoxide in a watch-glass
You must have observed that magnesium ribbon burns with adazzling white flame and changes into a white powder. This powder ismagnesium oxide. It is formed due to the reaction between magnesiumand oxygen present in the air.Activity 1.2 Take lead nitratesolution in a testtube.Add potassiumiodide solutionto this.What do youobserve?Activity 1.3 Take a few zinc granules in a conical flask or a test tube.Add dilute hydrochloric acid or sulphuric acid to this(Fig. 1.2).CAUTION: Handle the acid with care.Do you observe anything happening around the zincgranules?Touch the conical flask or test tube. Is there any change inits temperature?From the above three activities, we can say that any ofthe following observations helps us to determine whethera chemical reaction has taken place – change in statechange in colourevolution of a gaschange in temperature.As we observe the changes around us, we can seethat there is a large variety of chemical reactions takingplace around us. We will study about the various typesof chemical reactions and their symbolic representationin this Chapter.Figure 1.2Formation of hydrogengas by the action ofdilute sulphuric acid onzinc1.1 CHEMIC AL EQUATIONSEQUATIONSActivity 1.1 can be described as – when a magnesium ribbon is burnt inoxygen, it gets converted to magnesium oxide. This description of achemical reaction in a sentence form is quite long. It can be written in ashorter form. The simplest way to do this is to write it in the form of aword-equation.The word-equation for the above reaction would be –Magnesium Oxygen(Reactants) Magnesium oxide(1.1)(Product)The substances that undergo chemical change in the reaction (1.1),magnesium and oxygen, are the reactants. The new substance,magnesium oxide, formed during the reaction, is the product.A word-equation shows change of reactants to products through anarrow placed between them. The reactants are written on the left-handside (LHS) with a plus sign ( ) between them. Similarly, products arewritten on the right-hand side (RHS) with a plus sign ( ) between them.The arrowhead points towards the products, and shows the direction ofthe reaction.2Science
1.1.1 Writing a Chemical EquationIs there any other shorter way for representing chemical equations?Chemical equations can be made more concise and useful if we usechemical formulae instead of words. A chemical equation represents achemical reaction. If you recall formulae of magnesium, oxygen andmagnesium oxide, the above word-equation can be written as –Mg O2 MgO(1.2)Count and compare the number of atoms of each element on theLHS and RHS of the arrow. Is the number of atoms of each element thesame on both the sides? If not, then the equation is unbalanced becausethe mass is not the same on both sides of the equation. Such a chemicalequation is a skeletal chemical equation for a reaction. Equation (1.2) isa skeletal chemical equation for the burning of magnesium in air.1.1.2 Balanced Chemical EquationsRecall the law of conservation of mass that you studied in Class IX; masscan neither be created nor destroyed in a chemical reaction. That is, thetotal mass of the elements present in the products of a chemical reactionhas to be equal to the total mass of the elements present in the reactants.In other words, the number of atoms of each element remains thesame, before and after a chemical reaction. Hence, we need to balance askeletal chemical equation. Is the chemical Eq. (1.2) balanced? Let uslearn about balancing a chemical equation step by step.The word-equation for Activity 1.3 may be represented as –Zinc Sulphuric acid Zinc sulphate HydrogenThe above word-equation may be represented by the followingchemical equation –Zn H2SO4 ZnSO 4 H2(1.3)Let us examine the number of atoms of different elements on bothsides of the arrow.ElementNumber of atoms inreactants (LHS)Number of atomsin products (RHS)ZnHSO12141214As the number of atoms of each element is the same on both sides ofthe arrow, Eq. (1.3) is a balanced chemical equation.Let us try to balance the following chemical equation –Fe H2O Fe3O4 H2Chemical Reactions and Equations(1.4)3
Step I: To balance a chemical equation, first draw boxes around eachformula. Do not change anything inside the boxes while balancing theequation.Fe H2O Fe3O4 H2(1.5)Step II: List the number of atoms of different elements present in theunbalanced equation (1.5).ElementNumber of atomsin reactants (LHS)Number of atomsin products (RHS)121324FeHOStep III: It is often convenient to start balancing with the compoundthat contains the maximum number of atoms. It may be a reactant or aproduct. In that compound, select the element which has the maximumnumber of atoms. Using these criteria, we select Fe3O4 and the elementoxygen in it. There are four oxygen atoms on the RHS and only one onthe LHS.To balance the oxygen atoms –Atoms ofoxygen(i) Initial(ii) To balanceIn reactants1 (in H2O)1 4In products4 (in Fe3O4)4To equalise the number of atoms, it must be remembered that wecannot alter the formulae of the compounds or elements involved in thereactions. For example, to balance oxygen atoms we can put coefficient‘4’ as 4 H2O and not H2O4 or (H2O)4. Now the partly balanced equationbecomes –(1.6)Fe 4 H2O Fe 3O4 H2(partly balanced equation)Step IV: Fe and H atoms are still not balanced. Pick any of these elementsto proceed further. Let us balance hydrogen atoms in the partly balancedequation.To equalise the number of H atoms, make the number of moleculesof hydrogen as four on the RHS.Atoms ofhydrogen(i) Initial(ii) To balanceIn reactants8 (in 4 H2O)8In products2 (in H2)2 4The equation would be –Fe 4 H2O Fe3O4 4 H24(1.7)(partly balanced equation)Science
Step V: Examine the above equation and pick up the third element whichis not balanced. You find that only one element is left to be balanced,that is, iron.Atoms ofironIn reactantsIn products1 (in Fe)1 33 (in Fe3O4)3(i) Initial(ii) To balanceTo equalise Fe, we take three atoms of Fe on the LHS.3 Fe 4 H2O Fe3O4 4 H2(1.8)Step VI: Finally, to check the correctness of the balanced equation, wecount atoms of each element on both sides of the equation.(1.9)3Fe 4H2O Fe3O4 4H2(balanced equation)The numbers of atoms of elements on both sides of Eq. (1.9) areequal. This equation is now balanced. This method of balancing chemicalequations is called hit-and-trial method as we make trials to balancethe equation by using the smallest whole number coefficient.Step VII: Writing Symbols of Physical States Carefully examinethe above balanced Eq. (1.9). Does this equation tell us anything aboutthe physical state of each reactant and product? No information hasbeen given in this equation about their physical states.To make a chemical equation more informative, the physical statesof the reactants and products are mentioned along with their chemicalformulae. The gaseous, liquid, aqueous and solid states of reactantsand products are represented by the notations (g), (l), (aq) and (s),respectively. The word aqueous (aq) is written if the reactant or productis present as a solution in water.The balanced Eq. (1.9) becomes3Fe(s) 4H2O(g) Fe3O4(s) 4H2(g)(1.10)Note that the symbol (g) is used with H2O to indicate that in thisreaction water is used in the form of steam.Usually physical states are not included in a chemical equation unlessit is necessary to specify them.Sometimes the reaction conditions, such as temperature, pressure,catalyst, etc., for the reaction are indicated above and/or below the arrowin the equation. For example –340 atmCO(g) 2H2 (g) CH3 OH(l)(1.11)Sunlight6CO2 (aq) 12H2 O(l) Chlorophyll C6 H12 O6 (aq) 6O2 (aq) 6H2 O(l) (1.12)(Glucose)Using these steps, can you balance Eq. (1.2) given in the text earlier?Chemical Reactions and Equations5
QUESTIONS1.Why should a magnesium ribbon be cleaned before burning in air?2.Write the balanced equation for the following chemical reactions.(i) Hydrogen Chlorine Hydrogen chloride(ii) Barium chloride Aluminium sulphate Barium sulphate Aluminium chloride(iii) Sodium Water Sodium hydroxide Hydrogen3.Write a balanced chemical equation with state symbols for thefollowing reactions.(i) Solutions of barium chloride and sodium sulphate in water reactto give insoluble barium sulphate and the solution of sodiumchloride.?(ii) Sodium hydroxide solution (in water) reacts with hydrochloricacid solution (in water) to produce sodium chloride solution andwater.1.2 TYPES OF CHEMICAL REACTIONSCHEMICALREACTIONSWe have learnt in Class IX that during a chemical reaction atoms of oneelement do not change into those of another element. Nor do atomsdisappear from the mixture or appear from elsewhere. Actually, chemicalreactions involve the breaking and making of bonds between atoms toproduce new substances. You will study about types of bonds formedbetween atoms in Chapters 3 and 4.1.2.1 Combination ReactionActivity 1.4 Figure 1.3Formation of slakedlime by the reaction ofcalcium oxide withwaterTake a small amount of calcium oxideor quick lime in a beaker.Slowly add water to this.Touch the beaker as shown in Fig. 1.3.Do you feel any change in temperature?Calcium oxide reacts vigorously with water to produce slaked lime(calcium hydroxide) releasing a large amount of heat.CaO(s)(Quick lime) H2O(l) Ca(OH)2(aq)(1.13)(Slaked lime)In this reaction, calcium oxide and water combine to form a singleproduct, calcium hydroxide. Such a reaction in which a single productis formed from two or more reactants is known as a combination reaction.6Science
Do You Know?A solution of slaked lime produced by the reaction 1.13 is used for white washingwalls. Calcium hydroxide reacts slowly with the carbon dioxide in air to form a thinlayer of calcium carbonate on the walls. Calcium carbonate is formed after two tothree days of white washing and gives a shiny finish to the walls. It is interesting tonote that the chemical formula for marble is also CaCO3.Ca(OH) 2(aq) CO2(g)(Calciumhydroxide) CaCO3(s) H 2O(l)(1.14)(Calciumcarbonate)Let us discuss some more examples of combination reactions.(i) Burning of coalC(s) O2(g) CO2(g)(ii)(1.15)Formation of water from H2(g) and O2(g)2H2(g) O2(g) 2H 2O(l)(1.16)In simple language we can say that when two or more substances(elements or compounds) combine to form a single product, the reactionsare called combination reactions.In Activity 1.4, we also observed that a large amount of heat is evolved.This makes the reaction mixture warm. Reactions in which heat isreleased along with the formation of products are called exothermicchemical reactions.Other examples of exothermic reactions are –(i) Burning of natural gasCH 4(g) 2O2 (g) CO2 (g) 2H2O (g)(ii)(1.17)Do you know that respiration is an exothermic process?We all know that we need energy to stay alive. We get this energyfrom the food we eat. During digestion, food is broken down into simplersubstances. For example, rice, potatoes and bread containcarbohydrates. These carbohydrates are broken down to form glucose.This glucose combines with oxygen in the cells of our body and providesenergy. The special name of this reaction is respiration, the process ofwhich you will study in Chapter 6.C6H12O6(aq) 6O2(aq) 6CO2(aq) 6H2O(l) energy (1.18)(Glucose)(iii)The decomposition of vegetable matter into compost is also anexample of an exothermic reaction.Identify the type of the reaction taking place in Activity 1.1, whereheat is given out along with the formation of a single product.Chemical Reactions and Equations7
1.2.2 Decomposition ReactionActivity 1.5 Figure 1.4Correct way of heatingthe boiling tubecontaining crystalsof ferrous sulphateand of smelling theodourTake about 2 g ferrous sulphate crystalsin a dry boiling tube.Note the colour of the ferrous sulphatecrystals.Heat the boiling tube over the flame ofa burner or spirit lamp as shown inFig. 1.4.Observe the colour of the crystals afterheating.Have you noticed that the green colour of the ferrous sulphate crystalshas changed? You can also smell the characteristic odour of burningsulphur.Heat2FeSO4(s) Fe2O3(s) SO2(g) SO3(g)(Ferrous sulphate)(1.19)(Ferric oxide)In this reaction you can observe that a single reactant breaks downto give simpler products. This is a decomposition reaction. Ferroussulphate crystals (FeSO4, 7H2O) lose water when heated and the colourof the crystals changes. It then decomposes to ferric oxide (Fe2O3),sulphur dioxide (SO2) and sulphur trioxide (SO3). Ferric oxide is a solid,while SO2 and SO3 are gases.Decomposition of calcium carbonate to calcium oxide and carbondioxide on heating is an important decomposition reaction used invarious industries. Calcium oxide is called lime or quick lime. It hasmany uses – one is in the manufacture of cement. When a decompositionreaction is carried out by heating, it is called thermal decomposition.HeatCaCO3(s) CaO(s)(Limestone) CO2(g)(1.20)(Quick lime)Another example of a thermal decomposition reaction is givenin Activity 1.6.Activity 1.6 Figure 1.5Heating of lead nitrate andemission of nitrogen dioxide8Take about 2 g lead nitrate powder in a boilingtube.Hold the boiling tube with a pair of tongs andheat it over a flame, as shown in Fig. 1.5.What do you observe? Note down the change,if any.You will observe the emission of brown fumes.These fumes are of nitrogen dioxide (NO2). Thereaction that takes place is –Science
Heat2Pb(NO3) 2(s) 2PbO(s)(Lead nitrate)(Lead oxide)4NO2(g) O 2(g) (Nitrogendioxide)(1.21)(Oxygen)Let us perform some more decomposition reactions as given inActivities 1.7 and 1.8.Activity 1.7 Take a plastic mug. Drill two holes at itsbase and fit rubber stoppers in these holes.Insert carbon electrodes in these rubberstoppers as shown in Fig. 1.6.Connect these electrodes to a 6 voltbattery.Fill the mug with water such that theelectrodes are immersed. Add a few dropsof dilute sulphuric acid to the water.Take two test tubes filled with water andinvert them over the two carbon electrodes.Switch on the current and leave theapparatus undisturbed for some time.You will observe the formation of bubblesat both the electrodes. These bubbles displace water in thetest tubes.Is the volume of the gas collected the same in both the test tubes?Once the test tubes are filled with the respective gases, removethem carefully.Test these gases one by one by bringing a burning candle closeto the mouth of the test tubes.CAUTION: This step must be performed carefully by the teacher.What happens in each case?Which gas is present in each test tube?Figure 1.6Electrolysis of waterActivity 1.8 Take about 2 g silver chloride in a china dish.What is its colour?Place this china dish in sunlight for some time(Fig. 1.7).Observe the colour of the silver chloride after sometime.Figure 1.7You will see that white silver chloride turns grey in sunlight. This is Silver chloride turns greydue to the decomposition of silver chloride into silver and chlorine by in sunlight to form silvermetallight.Sunlight2AgCl(s) 2Ag(s) Cl2(g)Chemical Reactions and Equations(1.22)9
Silver bromide also behaves in the same way.Sunlight2AgBr(s) 2Ag(s) Br2(g)(1.23)The above reactions are used in black and white photography.What form of energy is causing these decomposition reactions?We have seen that the decomposition reactions require energy eitherin the form of heat, light or electricity for breaking down the reactants.Reactions in which energy is absorbed are known as endothermicreactions.Carry out the following ActivityTake about 2 g barium hydroxide in a test tube. Add 1 g of ammonium chloride and mixwith the help of a glass rod. Touch the bottom of the test tube with your palm. What do youfeel? Is this an exothermic or endothermic reaction?Q1.UESTIONSA solution of a substance ‘X’ is used for white washing.(i) Name the substance ‘X’ and write its formula.(ii) Write the reaction of the substance ‘X’ named in (i) above withwater.2.Why is the amount of gas collected in one of the test tubes in Activity1.7 double of the amount collected in the other? Name this gas.1.2.3 Displacement Reaction?Activity 1.9 Figure 1.8(a) Iron nails dipped in copper sulphate solution10Take three iron nails and clean them byrubbing with sand paper.Take two test tubes marked as (A) and(B). In each test tube, take about 10 mLcopper sulphate solution.Tie two iron nails with a thread andimmerse them carefully in the coppersulphate solution in test tube B forabout 20 minutes [Fig. 1.8 (a)]. Keep oneiron nail aside for comparison.After 20 minutes, take out the iron nailsfrom the copper sulphate solution.Compare the intensity of the blue colourof copper sulphate solutions in test tubes(A) and (B), [Fig. 1.8 (b)].Also, compare the colour of the iron nailsdipped in the copper sulphate solutionwith the one kept aside [Fig. 1.8 (b)].Science
Figure 1.8 (b) Iron nails and copper sulphate solutions compared before and after the experimentWhy does the iron nail become brownish in colour and the blue colourof copper sulphate solution fade?The following chemical reaction takes place in this Activity–Fe(s) CuSO4(aq) (Copper sulphate)FeSO4(aq) Cu(s)(1.24)(Iron sulphate)In this reaction, iron has displaced or removed another element,copper, from copper sulphate solution. This reaction is known asdisplacement reaction.Other examples of displacement reactions areZn(s) CuSO4(aq) ZnSO4(aq) Cu(s)(1.25)(Copper sulphate)Pb(s) CuCl2(aq) (Copper chloride)(Zinc sulphate)PbCl2(aq) Cu(s)(1.26)(Lead chloride)Zinc and lead are more reactive elements than copper. They displacecopper from its compounds.1.2.4 Double Displacement ReactionActivity 1.10 Take about 3 mL of sodium sulphatesolution in a test tube.In another test tube, take about 3 mL ofbarium chloride solution.Mix the two solutions (Fig. 1.9).What do you observe?You will observe that a white substance, which isinsoluble in water, is formed. This insoluble substanceformed is known as a precipitate. Any reaction thatproduces a precipitate can be called a precipitation reaction.Na2SO4(aq) BaCl2(aq) BaSO4(s) 2NaCl(aq)(Sodiumsulphate)(Bariumchloride)Chemical Reactions and Equations(Bariumsulphate)(1.27)Figure 1.9Formation of bariumsulphate and sodiumchloride(Sodiumchloride)11
What causes this? The white precipitate of BaSO4 is formed by the2 reaction of SO2–4 and Ba . The other product formed is sodium chloridewhich remains in the solution. Such reactions in which there is anexchange of ions between t
Chemical Reactions and Equations CHAPTER1 C onsider the following situations of daily life and think what happens when – milk is left at room temperature during summers. an iron tawa/pan/nail is left exposed to humid atmosphere. grapes get fermented. food is cooked. food gets digested in our body. we respire. In all the abo
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Test. 5. One Is Known As Volumetric Karl Fischer Titration. The Other Method Is Known As Coulometric Karl Fischer Titration. KF METHODS Volumetric Titration Coulometric . PRINCIPLE OF WORKING 1. The Principle Of Karl Fischer . Amount Of Karl Fischer Reagent To Reach The Characteristic Endpoint. 2. Weight Accurately 150 - 350 Mg Of Sodium .
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Chemical Formulas and Equations continued How Are Chemical Formulas Used to Write Chemical Equations? Scientists use chemical equations to describe reac-tions. A chemical equation uses chemical symbols and formulas as a short way to show what happens in a chemical reaction. A chemical equation shows that atoms are only rearranged in a chemical .
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