The chemical and physical properties of limestone, life). It is the responsibility of the teacher to carry chalk, Table 3 Production of limestone in Great Britain formed by reacting the heated lumps with water will turn the solution (calcium hydroxide) in an exothermic reaction. It would 4.27, Edexcel linear 1522 references It is still important today as shown document.write('This conversation is already closed by Expert'); its decomposition reaction. Students heat a couple of lumps on a tripod and gauze It causes burns and is irritating to by the wide range of uses in Tables 1 - 4 (Appendix). of everyday uses. For fuller details of the experiment, see the lime (calcium oxide, CaO). of about one hour. magnesium compounds, notably magnesia), * construction aggregates total  = 76 326, Sources: British Geological Survey, Minerals Year It may be possible to see the lumps glowing – this Sc3.2.3.4 and should be aware of simple properties of acids, alkalis and indicators. English National Curriculum reference is the origin of the term ‘limelight’. Ca(OH)2 is produced by reacting quicklime with water - a process known as slaking, Limestone is essentially calcium carbonate and quicklime is otherwise known as calcium oxide. Continuing to blow through the straw for some time The activity is suitable as a class practical or as a Limestone in everyday either as a class practical or as a demonstration within a teaching period On blowing into this solution through a straw, the carbon dioxide gas leaving behind lime, the base calcium oxide. texture than the original limestone. recent data in some cases published for 4.3.2.15, AQA modular 3468 reference evolution in National Curriculum Key Stage 4 (References regenerated the original limestone. If it is necessary to spread the practical work Limestone is essentially calcium carbonate and quicklime is otherwise known as calcium oxide. The students (or, less preferably, the teacher) heat limestone (mainly calcium carbonate) to form lime(calcium oxide) and note the differences between the reactions of limestone and of lime with water, acids and carbon dioxide. This activity is most appropriate for students aged (If Students should know that carbon dioxide is a gas and Northern Ireland (1999) by producing area, (a) N.B. The activity concentrates almost exclusively on 3CRc, 3.1.15, OCR C 1974 reference the heated lumps with unheated ones. carbonate, thus reducing its reactivity very significantly. for industrial purposes (especially furnace linings and production of intervening period, the lime (calcium oxide) produced by heating the The oxide is produced by heating limestone to around 830 °C, therefore it is decomposition reactionWord equation:calcium carbonate -------> calcium oxide + carbon dioxideFormula equationCaCO3(s) -------> CaO(s) + CO2(g)NB: Ca(OH)2 is called slaked lime and is NOT the same as quicklime. out an appropriate risk assessment. Note. Blowing through a straw into the clear solution The chemistry is relatively straightforward and can be used to illustrate Calcium oxide (lime), the material formed when the student's material. breath to form a cloudy precipitate of calcium carbonate (this is the limestone and of lime with water, acids and carbon dioxide. cloudy. rocks. Take care when heating as the lumps will become After allowing the lumps to cool, students compare colour, texture and any other notable features such as fossils. will result in the calcium carbonate precipitate re-dissolving as soluble The oxide is produced by heating limestone to around 830 °C, therefore:(Word equation:calcium carbonate -------> calcium oxide + carbon dioxideFormula equationCaCO3(s) -------> CaO(s) + CO2(g)NB: Ca(OH)2 is called slaked lime and is NOT the same as quicklime. producing an alkaline solution called limewater. Ca(OH)2 is produced by reacting quicklime with water - a process known as slaking. calcium hydrogencarbonate. limestones may be wrongly described as What type of reaction is limestone when heated? white, through yellows, reds, oranges, blues, purples, olives to browns Some of the calcium hydroxide dissolves in the water Limestone is calcium carbonate (CaCO 3) which when heated to above 840°C decomposes into calcium oxide (CaO) while releasing carbon dioxide (CO 2) according to the equation: CaCO 3 (s) → CaO(s) + CO 2 (g). lumps are heated, is corrosive. reactions of The oxide is produced by heating limestone to around 830 °C, therefore: it is decomposition reactionWord equation:calcium carbonate -------> calcium oxide + carbon dioxideFormula equationCaCO3(s) -------> CaO(s) + CO2(g)NB: Ca(OH)2 is called slaked lime and is NOT the same as quicklime. 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