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Chemical Reactions and Equations Class 10 Notes Science Chapter 1 - Learn CBSE

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Solution: During respiration, glucose combines with oxygen in the cells of our body to form carbon dioxide and water along with the production of energy. Write equations for decomposition reactions. Solution: Essentially, decomposition reactions are the opposite of combination reactions.

A compound decomposes i. Most decomposition reactions are endothermic. Another example of decomposition reaction is the heating of calcium carbonate sea shells, chalk :. Question 12 Write one equation each for decomposition reactions in which energy is supplied in the form of heat, light or electricity? Solution: When calcium carbonate is heated, it decomposes to give calcium oxide and carbon dioxide:.

Write relevant equations for the above? Solution: The difference between the displacement and double displacement reactions is that in a displacement reaction one element displaces another by virtue of it being more reactive whereas in a double displacement two anions and two cations switch places between two compounds respectively.

Thus Zn displaces Cu in the salt form. Zn is more reactive than Cu. Question 14 In the refining of silver, the recovery of silver from silver nitrate solution involves displacement by copper metal. Explain by giving examples: Solution: A precipitation reaction is a reaction in which soluble ions in separate solutions are mixed together to form an insoluble compound that settles out of solution as a solid. This insoluble compound is called a precipitate.

An example of a precipitation reaction Aqueous silver nitrate AgNO3 , when added to a solution containing potassium chloride KCl , precipitates a white solid, and silver chloride is observed.

Solution: The shiny brown colored element X is copper metal Cu. When copper metal is heated in air, it forms a black colored compound copper oxide.

So, the black colored compound is the copper oxide or copper II oxide, CuO. Question 17 Why do we apply paint on iron articles?

Solution: Rust is a soft and porous substance, which gradually falls from the surface of an iron object, and then the iron below starts rusting. Thus, rusting of iron or corrosion of iron is a continuous process which, if not prevented in time, eats up the whole iron object. So, when we apply paint on iron articles it reduces the rusting of iron.

Question 18 Oil and fat containing food items are flushed with nitrogen. Solution: Packaging fat and oil containing foods in nitrogen gas can prevent rancidity. When the fat and oil present in food materials gets oxidised in air , their oxidation products have an unpleasant smell and taste. When it is surrounded by unreactive gas, nitrogen, there is no oxygen of air to cause its oxidation and make it rancid.

Question 19 Explain the following terms with one example each. Corrosion b. Rancidity Solution: a. Corrosion is the process in which metals are eaten up gradually by the action of air, moisture or a chemical on their surface.

Corrosion is caused mainly by the oxidation of metals by the oxygen of air. Example: Rusting of iron is the most common form of corrosion. This is called rusting of iron. The condition produced by aerial oxidation of fat and oil in food which is marked by an unpleasant smell and taste is called rancidity.

Example: Rancidity can be retarded by keeping food in a refrigerator. The refrigerator has a low temperature inside it. When the food is kept in a refrigerator, the oxidation of fat and oil in it is slowed down due to low temperature. So, the development of rancidity due to oxidation is retarded. Question 20 Why should a magnesium ribbon be cleaned before burning in air?

Solution: To remove the oxide layer and facilitates rapid burning. Question 21 Write the balanced equation for the following chemical reactions. Question 22 Write a balanced chemical equation and state symbols for the following reactions. Solutions of barium chloride and sodium sulphate in water react to give insoluble barium sulphate and the solution of sodium chloride b.

Sodium hydroxide solution in water reacts with hydrochloric acid solution in water to produce sodium chloride solution and water. Question 24 Why does the colour of copper sulphate solution change when an iron nail is dipped into it?

Solution: In this reaction, iron displaces copper from copper sulphate solution. The deep blue colour of copper sulphate solution fades due to the formation of light green solution of iron sulphate.

A red-brown coating of copper metal is formed on the surface of the iron metal. This displacement reaction occurs because iron is more reactive than copper. Question 25 Identify the substances that are oxidised and the substances that are reduced in the following reactions.

The addition of oxygen is Called oxidation. So the substance that is oxidized is sodium Na. In this reaction, copper oxide CuO gives the oxygen required for the oxidation of hydrogen; therefore, copper oxide is the oxidizing agent. Hydrogen is responsible for removing oxygen from copper oxide; therefore, hydrogen is the reducing agent here. Question 1. When crystals of lead nitrate are heated strongly in a dry test tube a crystals immediately melt b a brown residue is left c white fumes appear in the test tube d a yellow residue is left Answer: b Pungent smelling, brown fumes are evolved due to NO 2 gas and brown coloured residue of lead oxide PbO is left.

Question 2. A dilute ferrous sulphate solution was gradually added to the beaker containing acidified permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation? In acidic medium, KMnO 4 oxidises ferrous sulphate to ferric sulphate.

Question 3. Dilute hydrochloric acid is added to granulated zinc taken in a test tube. The following observations are recorded. Point out the correct observation. HCl to form zinc chloride and bubbles of colourless and odourless hydrogen gas is evolved. Question 4. When a magnesium ribbon is burnt in air, the ash formed is a black b white c yellow d pink Answer: b When a Mg ribbon is burnt in air, the ash formed is of magnesium oxide which is white in colour.

Question 5. Three beakers labelled as A, B and C each containing 25 mL of water were taken. A small amount of NaOH, anhyd. It was observed that there was an increase in the temperature of the solutions contained in beakers A and B whereas, in case of beaker C, the temperature of the solution falls.

In beakers A and B, exothermic process has occurred. In beakers A and B, endothermic process has occurred. In beaker C, the exothermic process has occurred. In beaker C, endothermic process has occurred. Question 6. Which of the following will be required to identify the gas evolved when dilute hydrochloric acid reacts with zinc metal?

HCl, zinc metal forms zinc chloride and hydrogen gas is evolved. Presence of hydrogen gas can be checked by a burning splinter because H 4 gas burnt in a splinter with a pop sound. Question 7. And the colour of the solution fades away.

This is an example of displacement reaction. Question 8. What happens when ferrous sulphate crystals are heated? Question 9. The colour of the precipitate formed when barium chloride solution is mixed with sodium sulphate solution is [CCE ] a blue b black c white d green Answer: c This is an example of a double displacement reaction and a white precipitate of barium sulphate is formed.

Question How the colour changes when the gases after thermal decomposition of ferrous sulphate come in contact with an acidified solution of potassium dichromate? Answer: c The color changes from orange to green due to the formation of iron III sulphate.

The representation of chemical reaction by means of symbols of substances in the form of formulae is called chemical equation. Balanced Chemical Equation. A balanced chemical equation has equal number of atom of each element participating in the reaction on both left and right hand sides of the reaction. According to Law of Conservation of Mass, total mass of the elements present in the products of a chemical reaction has to be equal to the total mass of the element present in the reactants.

Rusting When iron reacts with oxygen and moisture it forms a red substance called rust. Corrosion Metals on coming in contact with oxygen, water, acids or gases presents in air changes its surface. This is called corrosion for e. Prevention � painting, galvanization, oiling, greasing. Rancidity Oil and fats on exposure to air show a change in taste and smell. This property is known as rancidity.

Prevention � adding antioxidants, Vacuum packing, refrigeration, flushing food with nitrogen. The transformation of chemical substance into a new chemical substance by making and breaking of bonds between different atom is known a chemical reaction. Combination Reaction When two elements or one compound and one element or two compounds combine to form a new product.

Exothermic Reactions Reactions producing energy are called exothermic reactions. Most of the combination reactions are exothermic in nature. Oxidation Gain of oxygen or removal of hydrogen is called oxidation eg.

Reduction Gain of hydrogen or removal of oxygen is called reduction. Redox Reactions A chemical reaction in which both oxidation and reduction takes place simultaneously are called redox reactions. Decomposition Reaction When a compound-split into two or more simple products for example Decomposition reaction require energy either in the form of heat, light or electricity for decomposing the reactions.

Endothermic Reactions Reactions which require energy to occur are known as endothermic reactions. Displacement Reactions It takes place when a more reactive metal displaces a less reactive metal.

Double Displacement Reactions In this reactions ions are exchanged between two reactants and forming new compounds. Precipitation Reaction : In some reactions, an insoluble mass is formed which is known as precipitate and such reactions are called precipitation reaction. Thorough knowledge and good practice will help you score full marks on the questions asked in this chapter. The above notes will help you to excel in exams.

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