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Chemical Reactions and Equations
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We have already learnt about physical and chemical changes of matter in our previous classes.
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Whenever a chemical change occurs, we can say that a chemical reaction has taken place.
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You may perhaps be wondering as to what is actually meant by a chemical reaction.
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How do we come to know that a chemical reaction has taken place?
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Let us perform some activities to find the answer to these questions.
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CAUTION:
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This Activity needs the teacher’s assistance.
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It would be better if students wear eye protection.
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Clean a magnesium ribbon about 2 cm long by rubbing it with sandpaper.
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Hold it with a pair of tongs.
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Consider the following situations of daily life and think what happens when –
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Burn it using a spirit lamp or burner and collect the ash so formed in a watch-glass.
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Burn the magnesium ribbon keeping it as far as possible from your eyes.
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What do you observe?
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Burning of a magnesium ribbon in air and collection of magnesium oxide in a watch-glass
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You must have observed that magnesium ribbon burns with a dazzling white flame and changes into a white powder.
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This powder is magnesium oxide.
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It is formed due to the reaction between magnesium and oxygen present in the air.
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Take lead nitrate solution in a test tube.
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Add potassium iodide solution to this.
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What do you observe?
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milk is left at room temperature during summers.
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Take a few zinc granules in a conical flask or a test tube.
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Add dilute hydrochloric acid or sulphuric acid to this.
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Do you observe anything happening around the zinc granules?
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Touch the conical flask or test tube. Is there any change in its temperature?
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From the above three activities, we can say that any of the following observations helps us to determine whether a chemical reaction has taken place –
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change in state
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change in colour
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evolution of a gas
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change in temperature.
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As we observe the changes around us, we can see that there is a large variety of chemical reactions taking place around us.
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an iron tawa/pan/nail is left exposed to humid atmosphere.
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We will study about the various types of chemical reactions and their symbolic representation in this Chapter.
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Formation of hydrogen
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when a magnesium ribbon is burnt in gas by the action of dilute sulphuric acid on oxygen, it gets converted to magnesium oxide.
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grapes get fermented.
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food is cooked.
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food gets digested in our body.
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we respire.
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In all the above situations, the nature and the identity of the initial substance have somewhat changed.
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Do you feel any change in temperature?
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Let us discuss some more examples of combination reactions.
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In simple language we can say that when two or more substances (elements or compounds) combine to form a single product, the reactions are called combination reactions.
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we also observed that a large amount of heat is evolved.
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This makes the reaction mixture warm.
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Reactions in which heat is released along with the formation of products are called exothermic
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chemical reactions.
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We all know that we need energy to stay alive.
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We get this energy from the food we eat.
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During digestion, food is broken down into simpler substances.
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For example, rice, potatoes and bread contain carbohydrates.
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Formation of slaked lime by the reaction of calcium oxide with Calcium oxide reacts vigorously with water to produce slaked lime water (calcium hydroxide) releasing a large amount of heat.
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These carbohydrates are broken down to form glucose.
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This glucose combines with oxygen in the cells of our body and provides energy.
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The decomposition of vegetable matter into compost is also an example of an exothermic reaction.
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Decomposition Reaction
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Take about 2 g ferrous sulphate crystals in a dry boiling tube.
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Note the colour of the ferrous sulphate crystals.
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Heat the boiling tube over the flame of a burner or spirit lamp.
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Observe the colour of the crystals after heating.
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Have you noticed that the green colour of the ferrous sulphate crystals?
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Correct way of heating the boiling tube has changed.
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In this reaction, calcium oxide and water combine to form a single product, calcium hydroxide.
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You can also smell the characteristic odour of burning containing crystals sulphur of ferrous sulphate.
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Ferrous sulphate crystals lose water when heated and the colour of the crystals changes.
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It then decomposes to ferric oxide, sulphur dioxide and sulphur trioxide.
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Ferric oxide is a solid, while SO2 and SO3 are gases.
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 112-151 (34).mp3
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Decomposition of calcium carbonate to calcium oxide and carbon dioxide on heating is an important decomposition reaction used in various industries.
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 112-151 (4).mp3
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Such a reaction in which a single product is formed from two or more reactants is known as a combination reaction.
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 112-151 (5).mp3
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Do You Know?
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A solution of slaked lime produced by the reaction is used for white washing walls.
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 112-151 (7).mp3
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Calcium hydroxide reacts slowly with the carbon dioxide in air to form a thin layer of calcium carbonate on the walls.
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Calcium carbonate is formed after two to three days of white washing and gives a shiny finish to the walls.
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It is interesting to note that the chemical formula for marble is also CaCO3.
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Calcium oxide is called lime or quick lime.
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It has many uses – one is in the manufacture of cement.
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When a decomposition reaction is carried out by heating, it is called thermal decomposition.
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Take about 2 g lead nitrate powder in a boiling tube.
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Hold the boiling tube with a pair of tongs and heat it over a flame.
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What do you observe?
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Note down the change, if any.
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Fill the mug with water such that the electrodes are immersed.
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Add a few drops of dilute sulphuric acid to the water.
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Take two test tubes filled with water and invert them over the two carbon electrodes.
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Switch on the current and leave the apparatus undisturbed for some time.
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You will observe the formation of bubbles at both the electrodes.
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These bubbles displace water in the Electrolysis of water test tubes.
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Is the volume of the gas collected the same in both the test tubes?
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Once the test tubes are filled with the respective gases, remove them carefully.
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Test these gases one by one by bringing a burning candle close to the mouth of the test tubes.
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CAUTION:
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You will observe the emission of brown fumes.
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This step must be performed carefully by the teacher.
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What happens in each case?
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 152-197 (22).mp3
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Which gas is present in each test tube?
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 152-197 (23).mp3
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Take about 2 g silver chloride in a china dish.
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 152-197 (24).mp3
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What is its colour?
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/storage/hf-datasets-cache/all/datasets/90464960732238-config-parquet-and-info-Achitha-10th_science_tami-3da38f41/downloads/extracted/d9d4926c0124d2e04cd19b14dc563fffc63a20ec0a8fb643177acf601be9c5d5/train/chapter 1 152-197 (25).mp3
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Place this china dish in sunlight for some time.
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