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    CBSE Class 10 Chemistry Worksheet - Chemical Reactions and Equations PDF

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    Malancha high school HS
    This chemistry assignment contains questions about chemical reactions and equations. It asks students to: 1) Define reactants, products, and a balanced chemical equation. 2) Balance a series of chemical equations and identify reactants and products. 3) Indicate the type of chemical reaction being represented in various equations, including combination, decomposition, displacement and combustion reactions. 4) Differentiate between types of chemical reactions and corrosion processes. The assignment covers concepts like oxidation, reduction, balancing equations, and examples of precipitation, thermal decomposition, natural oxidation and exothermic reactions.

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    CBSE Class 10 Chemistry Worksheet - Chemical Reactions and Equations PDF

    Uploaded by

    Malancha high school HS
    696 views4 pages
    This chemistry assignment contains questions about chemical reactions and equations. It asks students to: 1) Define reactants, products, and a balanced chemical equation. 2) Balance a series of chemical equations and identify reactants and products. 3) Indicate the type of chemical reaction being represented in various equations, including combination, decomposition, displacement and combustion reactions. 4) Differentiate between types of chemical reactions and corrosion processes. The assignment covers concepts like oxidation, reduction, balancing equations, and examples of precipitation, thermal decomposition, natural oxidation and exothermic reactions.

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    CBSE Class 10 Chemistry Worksheet - Chemical Reactions And Equations.pdf

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    This chemistry assignment contains questions about chemical reactions and equations. It asks students to: 1) Define reactants, products, and a balanced chemical equation. 2) Balance a series of chemical equations and identify reactants and products. 3) Indicate the type of chemical reaction being represented in various equations, including combination, decomposition, displacement and combustion reactions. 4) Differentiate between types of chemical reactions and corrosion processes. The assignment covers concepts like oxidation, reduction, balancing equations, and examples of precipitation, thermal decomposition, natural oxidation and exothermic reactions.

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    © All Rights Reserved
    Download as PDF, TXT or read online from Scribd
    Download as pdf or txt
    696 views4 pages

    CBSE Class 10 Chemistry Worksheet - Chemical Reactions and Equations PDF

    Uploaded by

    Malancha high school HS
    This chemistry assignment contains questions about chemical reactions and equations. It asks students to: 1) Define reactants, products, and a balanced chemical equation. 2) Balance a series of chemical equations and identify reactants and products. 3) Indicate the type of chemical reaction being represented in various equations, including combination, decomposition, displacement and combustion reactions. 4) Differentiate between types of chemical reactions and corrosion processes. The assignment covers concepts like oxidation, reduction, balancing equations, and examples of precipitation, thermal decomposition, natural oxidation and exothermic reactions.

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    © All Rights Reserved
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    of 4

    CLASS X CHEMISTRY ASSIGNMENT

    CHEMICAL REACTIONS AND EQUATIONS

    Q1Define:

     Reactants
     Products
     Balanced chemical equation.

    Q2 Balance the following chemical equation and identify the reactants and products.

    a. _____ Zn (s) + _____ AgNO3 (aq) → _____ Zn(NO3)2 (aq) + _____ Ag (s)

    b. _____ N2 (g) + _____ H2 (g) → _____ NH3 (g)

    c. _____ Mg(OH)2 (aq) + _____ H3PO4 (aq) → _____ H2O (l) + _____ Mg 3(PO4)2(aq)

    d. _____ HNO3 (aq) + _____ Ni (s) → _____ Ni(NO3)2 (aq) + _____ H2 (g)

    e. _____ Ba(HCO3)2 (s) → _____ BaCO3 (s) + _____ H2O (g) + _____ CO2 (g)

    f. _____ BaCl2 (aq) + _____ Na2SO4 (aq) → _____ NaCl (aq) + _____ BaSO4 (s)

    g. _____ Al2(CO3)3 (s) → _____ Al2O3 (s) + _____ CO2 (g)

    h. _____ Ca (s) + _____ H2O (l) → _____ Ca(OH)2 (aq) + _____ H2 (g)

    i. _____ LiHCO3 (s) → _____ Li2CO3 (s) + _____ H2O (g) + _____ CO2 (g)

    j. _____ N2 (g) + _____ O2 (g) → _____ N 2O5 (g)

    k. _____ MgBr2 (aq) + _____ KOH (aq) → _____ KBr (aq) + _____ Mg(OH)2 (s)

    l. _____ Mn (s) + _____ CuCl (aq) → _____ Cu (s) + _____ MnCl2 (s)

    m. _____ Zn (s) + _____ S8 (s) → _____ ZnS (s)


    n. _____ NaOH (aq) + _____ H2SO4 (aq) → _____ H2O (l) + _____ Na2SO4 (aq)

    o_____ K (s) + _____ H2O (l) → _____ KOH (aq) + _____ H2 (g)

    p. _____ C5H12 (l) + _____ O2 (g) → _____ H2O (g) + _____ CO2 (g)

    q. _____ KOH (aq) + _____ H2CO3 (aq) → _____ H2O (l) + _____ K 2CO3 (aq)

    r. _____ C4H8O 2 (l) + _____ O2 (g) → _____ H2O (g) + _____ CO2 (g)

    Q2 Write the skeleton equation for each of the following reactions. Then balance each of the
    following chemical equations.

    1. hydrogen + oxygen water


    2.iron(III) oxide + hydrogen water + iron
    3. sodium + water sodium hydroxide + hydrogen
    4. copper + Oxygen Copper(II) Oxide
    5. potassium iodide + chlorine potassium chloride + iodine
    6. chromium + tin(IV) chloride chromium(III) chloride + tin
    7. magnesium + copper(II) sulphate magnesium sulphate + copper
    8. zinc sulphate + strontium chloride zinc chloride + strontium sulphate
    9. ammonium chloride + lead(III) nitrate ammonium nitrate + lead(III) chloride
    10. iron(III) nitrate + magnesium sulphide iron(III) sulphide + magnesium
    nitrate
    11. aluminum chloride + sodium carbonate aluminum carbonate + sodium
    chloride
    12 sodium phosphate + calcium hydroxide sodium hydroxide +calcium
    phosphate

    Q3 Indicate which type of chemical reaction (Combination, decomposition, single-


    displacement, double-displacement or combustion) is being represented in the following
    reactions:
    1. Na3PO4 + 3 KOH  3 NaOH + K3PO4
    2. MgCl2 + Li2CO3  MgCO3 + 2 LiCl
    3. C6H12 + 9 O2  6 CO2 + 6 H2O
    4. 2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag
    5. C3H6O + 4 O2  3 CO2 + 3 H2O
    6. 2 C5H5 + Fe  Fe(C5H5)2
    7. SeCl6 + O2  SeO2 + 3Cl2
    8. 2 MgI2 + Mn(SO3)2  2 MgSO3 + MnI4
    9. O3  O. + O2
    10. 2 NO2  2 O2 + N2

    Q4 Differentiate between:
     Combination and Decomposition reaction.
     Displacement and Double displacement reaction.
     Oxidation and Reduction reaction.
     Balanced and unbalanced chemical equation.
     Corrosion of iron and Copper.

    Q5 Identify the substances that are oxidized and the substances that are reduced in the following
    reactions.

    (i) 4Na(s) + O2(g) → 2Na2O(s)

    (ii) CuO(s) + H2(g) → Cu(s) + H2O(l)

    Q6. Fe2O3 + 3CO 2Fe + 3CO2

    Study the above reaction and name the following:

     Substance getting reduced


     Substance getting oxidized
     Oxidizing agent
     Reducing agent.

    Q7.Give reasons for the following:

     Silver Nitrate solution cannot be stored in Copper containers.


     Gold and Silver do not corrode in air
     Blue colour of copper sulphate solution starts fading when a zinc rod is dipped in it.
     Respiration is an endothermic reaction.
     Photo chemical decomposition reaction finds application in photography.

    Q8.why does stale food gives a bad smell and bad taste? How can this be prevented?

    Q9Foreachof the following experiments, decide whether a reaction will occur. If you think there will be
    no reaction, write down why you think this.

    If you think a reaction will happen:


    write down why you think it will happen,what you expect to see, andthe word equation to go with it.

    a) iron heated with copper(II) oxide


    b) aluminium heated with iron oxide
    c) copper heated with iron oxide
    d) magnesium heated with zinc oxide

    Q10. Give examples for the following:

     Precipitation reaction.
     Thermal decomposition.
     Natural oxidation.
     Exothermic reaction.

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