The reaction of potassium with magnesium chloride is an example of a single displacement reaction. It means the elements present at the top of this reactivity series are more reactive than the elements present at the bottom. Reactivity series is a series in which elements are arranged in decreasing order of their reactivity. In these reactions, products can be determined through reactivity series. Single Displacement Reaction – In these reactions, more reactive metal displaces less reactive metal from its salt. For example, hydrochloric acid reacts with sodium hydroxide (base) and forms sodium chloride (salt) and water. Neutralization Reaction – In these reactions, acid and base react with each other and form salt and water. For example, when we burn methane, it gives carbon dioxide and water. It is a reaction between fuel and an oxidant (generally atmospheric oxygen) that produces smoke, water and heat generally. For example, when we burn magnesium ribbon (or magnesium), it gives grey-black ash of magnesium oxide.Ĭombustion Reaction – It is an exothermic reaction that releases energy, generally in the form of heat. Combination and decomposition reactions are opposite of each other. Reaction - 2H 2 O electricity → 2H 2 + O 2Ĭombination Reaction – In a combination reaction, two or more molecules are combined together chemically to form a new substance (compound). In the electrolysis of water, water breaks down into hydrogen and oxygen, which show completely different properties than water. Here, we are covering the most common eight types of chemical reactions, which are part of the class X chemistry syllabus as well.ĭecomposition Reaction – In a decomposition reaction, molecules or compounds break down into two or more than two simpler chemically new substances. Reaction – NH 3 (g) + HCl (g) -> NH 4 Cl (s)Ĭhemical reactions are of many types. For example, ammonia gas reacts with hydrogen chloride gas and forms solid ammonium chloride crystals. Reaction – BaCl 2 + Na 2 SO 4 -> BaSO 4 + NaClĬhange in State – Some chemical reactions are accompanied by a change in state. For example, barium chloride reacts with sodium sulphate and forms sodium chloride and precipitate of barium sulfate. For example, in combustion reactions, energy is released, such as the burning of a fuel.įormation of Precipitate – Some chemical reactions are accompanied by the formation of the precipitate. During a chemical reaction, energy can be evolved or be absorbed. For example, some reactions are exothermic in nature, while some are endothermic.Ĭhange in Energy – Chemical reactions often involve a change in energy. Reaction – Pb(NO 3 ) 2 + 2KI → PbI 2 + 2KNO 3Ĭolourless Colourless Yellow ppt colourlessĬhange in Temperature – Some chemical reactions are accompanied by a change in temperature. For example, when colourless lead nitrate reacts with potassium iodide, it forms a yellow precipitate of lead iodide and colourless potassium nitrate. For example, when zinc reacts with hydrochloric acid, hydrogen gas is evolved with the formation of zinc chloride.Ĭhange in Colour – Some chemical reactions are accompanied by a change in colour. Now understand these characteristics in detail.Įvolution of Gas – Some chemical reactions take place with the evolution of gas. The reaction is given below.Ĭ 6 H 12 O 6 + 6O 2 → 6CO 2 + 6H 2 O + EnergyĬhemical reactions show one or more than one of the following characteristics. For example, Respiration – we inhale oxygen which reacts with glucose and produces carbon dioxide, water and energy. A chemical reaction is a process in which reactants react chemically and convert into products by chemical transformation.
0 Comments
Leave a Reply. |