Limestone storyboard

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  • Limestone is a naturally occurring sedimentary rock consisting of high levels of calcium as well as magnesium carbonate, along with minerals. Lime production begins by extracting limestone from quarries and mines.
  • Limestone is mainly calcium carbonate, CaCO3, which when heated breaks down to form calcium oxide and carbon dioxide. Calcium oxide reacts with water to produce calcium hydroxide. Limestone and its products have many uses, including being used to make cement, mortar and concrete.
  • Step 1: Thermal decomposition- Calcium carbonate breaks down when heated strongly. This reaction is called thermal decomposition. Here are the equations for the thermal decomposition of calcium carbonate: calcium carbonate+( heat )----->calcium oxide + carbon dioxide CaCO3----> (heat)--->CaO + CO2 Other metal carbonates decompose in the same way, including: sodium carbonate magnesium carbonate copper carbonate
  • Step 2: Hydration or slaking- Calcium oxide reacts with water to form calcium hydroxide, which is an alkali. Here are the equations for this reaction: calcium oxide + water → calcium hydroxide CaO + H2O → Ca(OH)2
  • The last step of the cycle: Once Calcium Hydroxide is formed, adding Carbon dioxide to it will simply cause it to turn back into Calcium carbonate and therefore bring the cycle back to the start. Equations for this reaction: Ca(OH)2+CO2-------->CaCO3
  • buildings and roads
  • Glass: Heat wih sand and sodium carbonate
  • Neutralise acidid soils and lakes
  • limestone
  • concrete: Cement+sand+gravel+water
  • Mortar: Cement+water+sand
  • Cement: Heat with clay
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