[5]<\/strong><\/li>\n<\/ol>\n(c)<\/strong> Complete the following calculations. Show working for complete credit:
\n(i)<\/strong> Calculate the mass of Calcium that will contain the same number of atoms as are present in 3.2 gm of Sulphur.
\n[Atomic masses: S = 32, Ca = 40] [2]<\/strong>
\n(ii)<\/strong> If 6 litres of hydrogen and 4 litres of chlorine are mixed and exploded and if water is added to the gases formed, find the volume of the residual gas. [2]<\/strong>
\n(iii)<\/strong> If the empirical formula of a compound is CH and it has a vapour density of 13, find the molecular formula of the compound. [1]<\/strong>
\n(d)<\/strong> State one relevant observation for each of the following:<\/p>\n\n- When crystals of copper nitrate are heated in a test tube.<\/li>\n
- When the gaseous product obtained by dehydration of ethyl alcohol is passed through bromine water.<\/li>\n
- When hydrogen sulphide gas is passed through lead acetate solution.<\/li>\n
- When ammonia gas is burnt in an atmosphere of excess oxygen.<\/li>\n
- At the Anode when aqueous copper sulphate solution is electrolysed using copper electrodes. [5]<\/strong><\/li>\n<\/ol>\n
(e)<\/strong> Identify the acid<\/strong> which matches the following description (i) to (v):<\/p>\n\n- The acid which is used in the preparation of a non-volatile acid.<\/li>\n
- The acid which produces sugar charcoal from sugar.<\/li>\n
- The acid which is prepared by catalytic oxidation of ammonia.<\/li>\n
- The acid on mixing with lead nitrate solution produces a white precipitate which is insoluble even on heating.<\/li>\n
- The acid on mixing with silver nitrate solution produces a white precipitate which is soluble in excess ammonium hydroxide. [5]<\/strong><\/li>\n<\/ol>\n
(f)<\/strong> Give appropriate scientific reasons<\/strong> for the following statements:<\/p>\n\n- Zinc oxide can be reduced to zinc by using carbon monoxide, but aluminium oxide cannot be reduced by a reducing agent.<\/li>\n
- Carbon tetrachloride does not conduct electricity.<\/li>\n
- During electrolysis of molten lead bromide graphite anode is preferred to other electrodes.<\/li>\n
- The electrical conductivity of acetic acid is less in comparison to the electrical conductivity of dilute sulphuric acid at a given concentration.<\/li>\n
- Electrolysis of molten lead bromide is considered to be a redox reaction. [5]<\/strong><\/li>\n<\/ol>\n
(g) (i)<\/strong> Give balanced chemical equations<\/strong> for the following conversions A, B and C: [3]<\/strong>
\n
\n(ii)<\/strong> Differentiate between the terms strong electrolyte<\/strong> and weak electrolyte.<\/strong>\u00a0(stating any two differences) [2]<\/strong><\/p>\n(h)<\/strong> Answer the following questions:
\n(i)<\/strong> Explain the bonding in methane molecule using electron dot structure. [2]<\/strong>
\n(ii)<\/strong> The metals of Group 2 from top to bottom are Be, Mg, Ca, Sr and Ba.<\/p>\n\n- Which one of these elements will form ions most readily and why?<\/li>\n
- State the common feature in the electronic configuration of all these elements. [3]<\/strong><\/li>\n<\/ol>\n
Answer:<\/strong>
\n (a)<\/strong><\/p>\n\n- Ammonia<\/li>\n
- Hydrogen Chloride<\/li>\n
- Ethyne<\/li>\n
- Ethane<\/li>\n
- Hydrogen Sulphide<\/li>\n<\/ol>\n
(b)<\/strong><\/p>\n\n- (A) Lithium<\/li>\n
- (C) They can undergo addition as well as substitution<\/li>\n
- (C) Solder<\/li>\n
- (D) Ammonium chloride<\/li>\n
- (D) 6.02 x 1023<\/sup> atoms of carbon<\/li>\n<\/ol>\n
(c)<\/strong>
\n
\n (d)<\/strong><\/p>\n\n- Release reddish brown gas NO2<\/sub> (Nitrogen-di-oxide) which turns freshly prepared Ferrous Sulphate solution brown.
\nThe residue left is black copper oxide.<\/li>\n- Ethyl alcohol on dehydration forms ethene which when passed through bromine water makes it colourless.<\/li>\n
- The yellow lead acetate paper turns greyish black with hydrogen sulphide gas due to formation of lead (II) Sulphide.<\/li>\n
- Ammonia bums with a green flame.<\/li>\n
- Nothing is left at anode as copper atoms form copper ions and migrate towards cathode.<\/li>\n<\/ol>\n
(e)<\/strong><\/p>\n\n- Conc. Sulphuric acid<\/li>\n
- Conc. Sulphuric acid<\/li>\n
- Nitric acid<\/li>\n
- Sulphuric acid<\/li>\n
- Hydrochloric acid<\/li>\n<\/ol>\n
(f)<\/strong><\/p>\n\n- Zinc is comparatively less reactive. So its oxideis less stable and hence it can be reduced by reducing agent whereas Aluminium is very reactive due to which its oxide is quite stable and it can not be reduced by a reducing agent it can be reduced only by electrolytic reduction.<\/li>\n
- Carbon tetrachloride is a non polar covalent compound and so do not have free ions therefore they do not conduct electricity.<\/li>\n
- Graphite is an inert electrode which is preferred in electrolysis of molten lead bromide because if other active electrodes are used then bromine will react with them.<\/li>\n
- Acetic acid is a weak acid and has less number ions so conductivity is less whereas dil. sulphuric acid is a strong acid, has more number of ions and thererfore its electrical conductivity is more.<\/li>\n
- During electrolysis of molten lead bromide lead gets oxidised and bromine gets reduced. Thus both oxidation and reduction occur simultaneously. So it is a redox reaction.<\/li>\n<\/ol>\n
(g)<\/strong>
\n
\n (h)<\/strong>
\n(i)<\/strong> Methane: CH4<\/sub>
\nC = 6 = 2, 4
\nH = 1
\nIn bonding of methane molecule, one atom of carbon shares four electron pairs, one with each of the four atoms of hydrogen.
\n
\n(ii)<\/strong><\/p>\n\n- Barium will form ions most readily because it is most metallic and lose electrons readily and form positive ion.<\/li>\n
- All these elements have 2 valence electrons.<\/li>\n<\/ol>\n
SECTION-II \u00a0(40 Marks)<\/strong><\/span>
\n(Answer any four<\/strong> questions from this section)<\/em><\/p>\nQuestion 2:<\/strong>
\n (a)<\/strong> Arrange the following as per the instructions<\/strong> given in the brackets:<\/p>\n\n- Cs, Na, Li, K, Rb (increasing order of metallic character)<\/li>\n
- Mg, Cl, Na, S, Si (decreasing order of atomic size)<\/li>\n
- Na, K, Cl, S, Si (increasing order of ionization energy)<\/li>\n
- Cl, F, Br, I (increasing order of electron affinity) \u00a0 \u00a0 \u00a0 \u00a0 [4]<\/strong><\/li>\n<\/ol>\n
(b)<\/strong> Choose the most appropriate answer from the following list of oxides which fit the description<\/strong>. Each answer may he used only once:
\n[SO2<\/sub>, SiO2<\/sub> Al2<\/sub>O3<\/sub>, MgO, CO, Na2<\/sub>O]<\/p>\n\n- A basic oxide.<\/li>\n
- An oxide which dissolves in water forming an acid.<\/li>\n
- An amphoteric oxide<\/li>\n
- A covalent oxide of a metalloid. \u00a0 \u00a0 \u00a0 \u00a0\u00a0[4]<\/strong><\/li>\n<\/ol>\n
(c)<\/strong> Element X is a metal with a valency 2, Y is a non-metal with a valency 3.<\/p>\n\n- Write an equation to show how Y forms an ion.<\/li>\n
- If Y is a diatomic gas, write an equation for the direct combination of X and Y to form a compound. [2]<\/strong><\/li>\n<\/ol>\n
Answer:<\/strong>
\n (a)<\/strong><\/p>\n\n- Li < Na < K < Rb < Cs<\/li>\n
- Na > Mg > Si > S > Cl<\/li>\n
- K < Na < Si < S < Cl<\/li>\n
- I < Br < F < Cl<\/li>\n<\/ol>\n
(b)<\/strong><\/p>\n\n- MgO<\/li>\n
- SO2<\/sub><\/li>\n
- Al2<\/sub>O3<\/sub><\/li>\n
- CO<\/li>\n<\/ol>\n
(c)<\/strong><\/p>\n\n- Y + 3e–<\/sup>\u00a0\u00a0\u2192 \u00a0\u00a0Y– – –<\/sup><\/li>\n
- 3X + Y2<\/sub>\u00a0 \u00a0\u2192 \u00a0 X3<\/sub>Y2<\/sub><\/li>\n<\/ol>\n
Question 3:<\/strong>
\n(a)<\/strong> Give balanced chemical equations<\/strong> for the following conversions<\/strong>:
\n(i)<\/strong> Ethanoic acid to ethyl ethanoate.
\n(ii)<\/strong> Calcium carbide to ethyne.
\n(iii)<\/strong> Sodium ethanoate to methane.\u00a0 \u00a0 \u00a0 [3]<\/strong><\/p>\n(b)<\/strong> Using their structural formulae identify the functional group by circling them:
\n(i)<\/strong> Dimethyl ether.
\n(ii)<\/strong> Propanone. \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0[2]<\/strong><\/p>\n(c)<\/strong> Name the following:<\/p>\n\n- Process by which ethane is obtained from ethene.<\/li>\n
- A hydrocarbon which contributes towards the greenhouse <\/strong>effect.<\/li>\n
- Distinctive reaction that takes place when ethanol is treated with acetic acid.<\/li>\n
- The property of elements by virtue of which atoms of the element can link to each other in the form of a long chain or ring structure.<\/li>\n
- Reaction when an alkyl halide is treated with alcoholic potassium hydroxide. [5]<\/strong><\/li>\n<\/ol>\n
Answer:
\n<\/strong>
\n
\n(c)<\/strong><\/p>\n\n- Hydrogenation<\/li>\n
- Methane<\/li>\n
- Esterification<\/li>\n
- Catenation<\/li>\n
- Dehydrohalogenation<\/li>\n<\/ol>\n
Question 4:<\/strong>
\n(a)<\/strong> Identify the anion<\/strong> present in each of the following compounds:<\/p>\n\n- A salt M<\/strong> on treatment with concentrated sulphuric acid produces a gas which fumes in moist air and gives dense fumes with ammonia.<\/li>\n
- A salt D<\/strong> on treatment with dilute sulphuric acid produces a gas which turns lime water milky but has no effect on acidified potassium dichromate solution.<\/li>\n
- When barium chloride solution is added to salt solution E<\/strong> a white precipitate insoluble in dilute hydrochloric acid is obtained. \u00a0 \u00a0[3]<\/strong><\/li>\n<\/ol>\n
(b)<\/strong> The following table shows the tests a student performed on four different aqueous solution which are X, Y, Z and W. Based on the observations provided, identify the cation present: \u00a0\u00a0\u00a0[4]<\/strong><\/p>\n\n\n\nChemical test<\/strong><\/td>\nObservation<\/strong><\/td>\nConclusion<\/strong><\/td>\n<\/tr>\n\nTo solution X<\/strong>, ammonium hydroxide is added in minimum quantity first and then in excesss.<\/td>\nA dirty white precipitate is formed which dissolves in excess to form a clear solution.<\/td>\n | (i)<\/td>\n<\/tr>\n | \nTo solution Y,<\/strong> ammonium hydroxide is added in minimum quantity first and then in excess.<\/td>\nA pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution.<\/td>\n | (ii)<\/td>\n<\/tr>\n | \nTo solution W,<\/strong> a small quantity of sodium hydroxide solution is added and then in excess.<\/td>\nA white precipitate is formed which remains insoluble.<\/td>\n | (iii)<\/td>\n<\/tr>\n | \nTo a salt Z,<\/strong> calcium hydroxide solution is added and then heated.<\/td>\nA pungent smelling gas turning moist red litmus paper blue is obtained.<\/td>\n | (iv)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n (c)<\/strong> Give balanced chemical equations for each of the following:<\/p>\n\n- Lab preparation of ammonia using an ammonium salt.<\/li>\n
- Reaction of ammonia with excess chlorine.<\/li>\n
- Reaction of ammonia with sulphuric acid. \u00a0 \u00a0 \u00a0\u00a0\u00a0[3]<\/strong><\/li>\n<\/ol>\n
Answer:<\/strong> \n(a)<\/strong><\/p>\n\n- M = Chloride (Cl–<\/sup>)<\/li>\n
- D = Carbonate (CO3<\/sub>– –<\/sup> )<\/li>\n
- E = Sulphate (SO4<\/sub>– –<\/sup>)<\/li>\n<\/ol>\n
(b)<\/strong><\/p>\n\n- Zn++<\/sup> = Zinc ion.<\/li>\n
- Cu
| | | | | | | |