Home Assignment - Chemical reactions and Equations

 Home Assignment - Chemical reactions and Equations

1.       What are the characteristics of chemical reactions? Write one example of each.

2.       Balance the below chemical reactions:

               i.                        Fe + H2O           -------      Fe3O4 + H2

             ii.                        C2H6 + O2           -------               CO2 + H2O

           iii.                        BaCl2 + Al2(SO4)3     -------             BaSO4 + AlCl3

           iv.                        Na + H2O     -------           NaOH + H2

             v.                        NaOH + Al2O3            -------                         NaAlO2 + H2O

           vi.                        KI + Pb (NO3)2          -------            PbI2 + KNO3

          vii.                         HNO3 + Ca(OH)2 → Ca(NO3)2 + H2O

        viii.                        NaOH + H2SO4 → Na2SO4 + H2O

           ix.                        NaCl+AgNOa → AgCl + NaNO3

             x.                        BaCl2 + H2SO4 → BaSO4 + HCl

3.       What are the names given for the substances that react and get formed in a chemical reaction?

4.       Why should a magnesium ribbon be cleaned before burning in air?

5.       What is the colour of the product formed after burning of magnesium?

6.       A solution of a substance ‘X’ is used for white washing.

i.                     Name the substance ‘X’ and write its formula.

ii.                   Write the reaction of the substance ‘X’ name in (i) above with water.

7.       Why is the amount of gas collected in one of the test tubes during electrolysis of water double of the amount collected in the other? Name this gas.

8.       Why does the colour of copper sulphate solution change when an iron nail is dipped in it?

9.       Give an example of a double displacement reaction other than the reaction of barium chloride with sodium sulphate.

10.   Identify the substances that are oxidised 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)

11.   Identify the substances that is getting oxidised and reduced.

2PbO (s) + C (s)                    2Pb(s) + CO2 (g)

12.   What happens when dilute hydrochloric acid is added to iron fillings?

13.   What is a balanced chemical equation? Why should chemical equations be balanced?

14.   Write the balanced chemical equation for the following and identify the type of reaction in each case:-

(a) Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s)
(b) Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g)
(c) Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g)
(d) Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g)

15.   Translate the following statements into chemical equations and then balance them.
(a) Hydrogen gas combines with nitrogen to form ammonia.
(b) Hydrogen sulphide gas burns in air to give water and sulphur dioxide.
(c) Barium chloride reacts with aluminium sulphate to give aluminium chloride and a precipitate of barium sulphate.
(d) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas.

16.    Write the balanced chemical equations for the following reactions.
(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water
(b) Zinc + Silver nitrate → Zinc nitrate + Silver
(c) Aluminium + Copper chloride → Aluminium chloride + Copper
(d) Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride

17.    What does one mean by exothermic and endothermic reactions? Give examples?

18.   Why is respiration considered an exothermic reaction? Explain?

19.   Why are decomposition reactions called the opposite of combination reactions? Write equations for these reactions?

20.   Write one equation each for decomposition reactions where energy is supplied in the form of heat, light or electricity.

21.    What is the difference between displacement and double displacement reactions? Write equations for these reactions?

22.   In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal.
Write down the reaction involved?

23.    What do you mean by a precipitation reaction? Explain by giving examples.

24.    Explain the following in terms of gain or loss of oxygen with two examples each.
(a) Oxidation
(b) Reduction

25.   A shiny brown coloured element ‘X’ on heating in air becomes black in colour. Name the element ‘X’ and the black coloured compound formed.

26.   Why do we apply paint on iron articles?

27.   Which of the following are chemical /physical changes?

a.       Formation of curd from milk

b.      Ripening of fruits

c.       Getting salt from sea water

d.      Burning of wood

28.   What is the value of x, y and z to balance the below chemical reactions?

i.                     2NaoH + xAl2O3                              yNaAlO2 + H2O

ii.                   MnO2 + xHCl                     MnCl2 + yH2O + zCl2

29.   What is the value of x, y and z to balance the below chemical reactions?

aAl2O3 + bHCl                   cAlCl3 + dH2O

30.   When aqueous solutions of potassium iodide and lead nitrate are mixed, an insoluble substance separates out. What is the insoluble substance? What is its colour?

31.  A metal ribbon ' X ' burns in oxygen with a dazzling white flame forming a white ash ' Y '. What is X, Y and the type of reaction.

32.   What happens when lead nitrate is heated in a dry test tube? What type of reaction it is? Name the gas produced and its colour?

 

33.   A magnesium is ribbon is burn in presence of air with a tong over a burner. The ashes are kept on a watch glass.

a.       What do you observe?

b.      What is the colour of powder formed after burning it?

c.       What is the powdered substance formed? Name the substance along with its chemical formula.

d.      Write its reaction.

e.       Why magnesium ribbon should be cleaned before burning?

34.   A test tube is taken in which lead nitrate and potassium iodide solution is mixed together.

a.       List the observations.

b.      What products are formed?

c.       What is the colour of the precipitate formed? Name the substance.

d.      Define precipitation reaction.

35.   Zinc liberates a gas when reacted with dilute hydrochloric acid.

a.       Name the gas liberated. How can you test for it?

b.      What is the colour of the gas?

c.       Write its reaction. What type of reaction it is?

36.   A magnesium ribbon is burnt in oxygen to give a white compound X accompanied by emission of light. If the burning ribbon is now placed in an atmosphere of nitrogen, it continues to burn and forms a compound Y.

a.       Write the chemical formula of X and Y.

b.      Write the balanced chemical equation, when X is dissolved in water.

37.   A substance X, which is used intensively in cement industry. This is present in bones also. On treatment with water it forms a solution which turns red litmus blue. Identify X and also write the chemical reactions involved.

38.   A solution of a substance X is used for white washing.

a.       Name the substance X and write its formula.

b.      Write the reaction of the substance X with water.

c.       Why white washing with this solution forms a shinny finish layer on the wall after two to three days? Show the reaction formed.

39.    Calcium oxide + water -------- X

a.     Name the product X formed when calcium oxide reacts with water? Write its chemical formula.

b.     Which type of reaction between calcium oxide and water?

c.     What change in the temperature during the reaction you notice?

d.     What type of reaction takes place during activity on the basis of change in the temperature?

 

40.   When 2 g of ferrous sulphate crystals are heated in a dry boiling test tube, it gives gas with a strong pungent smell.

e.       Name the gases produced.

f.        Name the type of reaction.

g.       Write its reaction.

41.   A 2 g lead nitrate powder boiled in a test tube with the evolution of fumes

a. Name the fumes evolved. What is the colour of the fumes?

b. Write its reaction.

c. What is the type of reaction?

 

42.   Identify the reducing agent in the following reactions:-                                            

a.       4NH3 + 5O2                         4NO + 6H2O

b.      H2O + F2                            HF + HOF

c.       Fe2O3 + 3CO                                    2Fe + 3CO2

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