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Decomposition of to calcium oxide and c...

Decomposition of __________ to calcium oxide and carbon dioxide is used in various industries.

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calcium carbonate
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The decomposition of calcium carbonate to calcium oxide and carbon dioxide is a redox reaction .True/False

Answer question numbers (a) - (d) on the basis of your understanding of the following paragraph and related studied concepts. Green colour of ferrous sulphate crystals changes on heating.Also the smell of characteristic odour of burning sulphur is felt. 2FeSO_(4)(s)overset("Heat")(to)Fe_(2)O_(3)(s)+SO_(2)(g)+SO_(3)(g) In this reaction, you can observe that a single reactant breaks down to give simpler products. This is a decomposition reaction. Ferrous sulphate crystals (FeSO_(4).7H_(2)O) lose water when heated and the colour of the crystals changes. It then decomposes to ferric oxide (Fe_(2)O_(3)) , sulphur dioxide (SO_(2)) and sulphur trioxide (SO_(3)) . Ferric oxide is a solid, while SO_(2) and SO_(3) are gases. Decomposition of calcium carbonate to calcium oxide and carbon dioxide on heating is an important decomposition reaction used in various industries. Calcium oxide is called lime or quick lime. It has many uses -one is in the manufacture of cement. When a decomposition reaction is carried out by heating, it is called thermal decomposition. underset("(Limestone)")(CaCO_(3))(s)overset("Heat")(to)underset("(Quick lime)")(CaO(s))+CO_(2)(g) What is the difference between decomposition reaction and thermal decomposition ?

Knowledge Check

  • carbon in carbon dioxide is

    A
    `sp` hybridization
    B
    `sp^(2)` hybridization
    C
    `sp^(3)` hybridization
    D
    `d^(2)sp^(3)` hybridised.

  • Decomposition of urea into ammonia and carbon dioxide is catalysed by

    A
    Biochemical catalyst
    B
    Inorganic catalyst
    C
    Shape selective catalyst
    D
    All of these

  • Sodium carbonate is used in ____industries.

    A
    paper
    B
    paint
    C
    textile
    D
    all of these

    • Similar Questions

    Explore conceptually related problems

    Answer question numbers (a) - (d) on the basis of your understanding of the following paragraph and related studied concepts. Green colour of ferrous sulphate crystals changes on heating.Also the smell of characteristic odour of burning sulphur is felt. 2FeSO_(4)(s)overset("Heat")(to)Fe_(2)O_(3)(s)+SO_(2)(g)+SO_(3)(g) In this reaction, you can observe that a single reactant breaks down to give simpler products. This is a decomposition reaction. Ferrous sulphate crystals (FeSO_(4).7H_(2)O) lose water when heated and the colour of the crystals changes. It then decomposes to ferric oxide (Fe_(2)O_(3)) , sulphur dioxide (SO_(2)) and sulphur trioxide (SO_(3)) . Ferric oxide is a solid, while SO_(2) and SO_(3) are gases. Decomposition of calcium carbonate to calcium oxide and carbon dioxide on heating is an important decomposition reaction used in various industries. Calcium oxide is called lime or quick lime. It has many uses -one is in the manufacture of cement. When a decomposition reaction is carried out by heating, it is called thermal decomposition. underset("(Limestone)")(CaCO_(3))(s)overset("Heat")(to)underset("(Quick lime)")(CaO(s))+CO_(2)(g) What is meant by a decomposition reaction ?

    Answer question numbers (a) - (d) on the basis of your understanding of the following paragraph and related studied concepts. Green colour of ferrous sulphate crystals changes on heating.Also the smell of characteristic odour of burning sulphur is felt. 2FeSO_(4)(s)overset("Heat")(to)Fe_(2)O_(3)(s)+SO_(2)(g)+SO_(3)(g) In this reaction, you can observe that a single reactant breaks down to give simpler products. This is a decomposition reaction. Ferrous sulphate crystals (FeSO_(4).7H_(2)O) lose water when heated and the colour of the crystals changes. It then decomposes to ferric oxide (Fe_(2)O_(3)) , sulphur dioxide (SO_(2)) and sulphur trioxide (SO_(3)) . Ferric oxide is a solid, while SO_(2) and SO_(3) are gases. Decomposition of calcium carbonate to calcium oxide and carbon dioxide on heating is an important decomposition reaction used in various industries. Calcium oxide is called lime or quick lime. It has many uses -one is in the manufacture of cement. When a decomposition reaction is carried out by heating, it is called thermal decomposition. underset("(Limestone)")(CaCO_(3))(s)overset("Heat")(to)underset("(Quick lime)")(CaO(s))+CO_(2)(g) How much quick lime is obtained when 50 g of limestone is heated strongly ?

    Answer question numbers (a) - (d) on the basis of your understanding of the following paragraph and related studied concepts. Green colour of ferrous sulphate crystals changes on heating.Also the smell of characteristic odour of burning sulphur is felt. 2FeSO_(4)(s)overset("Heat")(to)Fe_(2)O_(3)(s)+SO_(2)(g)+SO_(3)(g) In this reaction, you can observe that a single reactant breaks down to give simpler products. This is a decomposition reaction. Ferrous sulphate crystals (FeSO_(4).7H_(2)O) lose water when heated and the colour of the crystals changes. It then decomposes to ferric oxide (Fe_(2)O_(3)) , sulphur dioxide (SO_(2)) and sulphur trioxide (SO_(3)) . Ferric oxide is a solid, while SO_(2) and SO_(3) are gases. Decomposition of calcium carbonate to calcium oxide and carbon dioxide on heating is an important decomposition reaction used in various industries. Calcium oxide is called lime or quick lime. It has many uses -one is in the manufacture of cement. When a decomposition reaction is carried out by heating, it is called thermal decomposition. underset("(Limestone)")(CaCO_(3))(s)overset("Heat")(to)underset("(Quick lime)")(CaO(s))+CO_(2)(g) Give an important household application of quick lime other than in the manufacture of cement.

    Calcium carbonate decomposes on heating to give calcium oxide and carbon dioxide. How much volume of CO_2 will be obtained by thermal decomposition of 50g CaCO_3 ?

    Calcium carbonate, CaCO_(3) decomposes upon heating to calcium oxide and carbon dioxide. What mass of solid calcium carbonate is required to produce 2.40 liters of carbon dioxide measured at STP?

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