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Riyesh Rahate
Abhinav Vidyalay, Dombivli, Thane
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MAHESH TUTORIALS I.C.S.E. ICSE X SUBJECT : CHEMISTRY Last Minute Revision Chapter : Periodic Table Q.1. Answer the following : (i) Group No. 1 - IA 2 - IIA 13 - IIIA 14 - IVA 15 - VA 2nd period Li D 3rd period A Mg E 4th period R T I Si Q 16 - VIA 17 - VIIA 18 - 0 O J H M u Ne y In the above table H does not represent hydrogen. Some elements are in their own symbol and position in the periodic table while others are shown with a letter. Identify 1. The most electronegative element. 2. The most reactive element of group I. 3. The element from period 3 with least atomic size. 4. The noble gas of the fourth period. 5. How many valence electrons are present in Q. 6. Which element from group 2 would have the least ionization energy. 7. In the compound between A and H what type of bond is formed and give its molecular formula. (ii) Name or state the following with reference to the elements of the modern periodic table. 1. The more non-metallic element from the elements S, P, CI and Ar. 2. A light element in period-3 with a neutron/proton ratio around 1. 3. The element with the highest ionisation potential from the elements of period 1, 2 and 3. (iii) Arrange the following elements as per the guidelines in brackets. 1. Na, Cl, Mg, P [in decreasing order of atomic size] 2. C, Li, F, N [in increasing order of electronegativity] 3. CI, Al, Na, S [in increasing order of ionisation potential] 4. Li, F, C, O [in increasing order of electron affinity] 5. Ar, He, Ne [in increasing order of number of electron shells] .. 2 .. Chapter : Chemical Bonding Q.2. Answer the following : (i) Explain with the help of 1. an ionic equation 2. electron dot structural diagram 3. atomic or orbit structural diagram the formation of the following : a) Sodium chloride b) Calcium oxide c) Magnesium chloride. [atomic numbers. Na = 11, Cl = 17, Ca = 20, O = 8, Mg = 12]. (ii) Compound X consists of molecules. 1. Bonding in X will be :- A : ionic. B : electrovalent. C : covalent. D : molecular. Chapter : Acids, Bases and Salts Q.3. Answer the following : (i) State which of the following methods is generally used for preparing the salts 1 to 5 given below : A : Neutralisation - insoluble base and dil. acid B : Neutralisation - alkali and dil. acid C : Simple displacement - active metal and dil.acid D : Direct combination E : Precipitation [double decomposition] (ii) 1. PbCO3 5. FeS 2. Zn(NO 3) 2 3. NaCl 4. Cu(NO 3) 2 State the method only, generally used for the preparation of the following salts. 1. Zn(NO 3) 2 4. ZnS 7. PbCl2 2. NH 4Cl 5. CaCO 3 8. Pb(NO3)2 3. ZnSO 4 6. FeCl 3 (iii) State what will be the effect of each of the following solutions on blue litmus 1. (iv) K2CO3 soln. 2. KCl soln 3. NH4NO3 soln. Define : 1. Water of crystallisation 2. Deliquescent salts 3. Efflorescent salts, with four examples each. .. 3 .. Chapter : Analytical Chemistry Q.4. (i) The salt which in soln. gives a pale green precipitate with NaOH soln. and a white ppt. with BaCl2 soln. (ii) 1. Iron [III) sulphate 2. Iron [II] sulphate 3. Iron [II] chloride 4. Iron [III] chloride State two relevant observations for the reaction: Ammonium hydroxide solution is added to copper (II) nitrate solutionin small quantities and then in excess. Chapter : Mole Concept and Stoichiometry Q.5. (i) Calculate the no. of moles and the no. of molecules present in 1.4g of ethylene gas [C 2H4]. What is the vol.occupied by the same amount of C2H4. State the vapour density of C2H4. [Avog. No. = 6 1023; C = 12, H = 1] [0.05. moles; 3 1022 molecules; 1.12 lit. ; 14] (ii) Dil. HCl is reacted with 4.5 moles of calcium carbonate. Calculate 1. The mass of 4.5 moles of CaCO3. 2. The volume of CO2 liberated at stp. 3. The mass of CaCl2 formed. 4. The number of moles of the acid HCl used in the reaction [relative molecular mass of CaCO3 is 100 and of CaCl2 is 111]. (iii) 10 litres of a mixture of propane [C3H8] [60%] and butane [C4H10][40%] is burnt. Calculate the total volume of carbon dioxide formed. Combustion reactions of the mixture are represented as C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g); 2C4H10(g) + 13O2(g) 8CO2(g) + 10H2O(g) [34 lits.] (iv) Ammonia may be oxidised to nitrogen monoxide in the presence of a catalyst according to the following equation: 4NH3 + 5O2 4NO + 6H2O If 27 litres of reactants are consumed, what volume of nitrogen monoxide is produced at the same temperature & pressure? .. 4 .. (v) Samples of O2, N2, CO and CO2 under the same conditions of temp. and press. contain the same number of molecules represented by X. The molecules of oxygen occupy V litres and have a mass of 8g. Under the same conditions of temp. and press., what is the volume occupied by : 1. X molecules of N2. 2. 3X molecules of CO. 3. What is the mass of CO2 in grams? [V litres] ; [3V litres] [11g.] 4. In answering the above questions, whose law has been used. [C = 12, N = 14, O = 16] (vi) If a crop of wheat removes 20 kg of nitrogen per hectare of soil what mass in kg. of the fertilizer calcium nitrate would be required to replace the nitrogen in a 10 hectare field. [N = 14; O = 16; Ca = 40] (vii) Calculate the % of boron [B] in borax Na2B4O7. 10H2O. [H = 1, B = 11, O = 16, Na = 23] (viii) Calculate the percentage of nitrogen in a aluminium nitride. [Al = 27, N = 14] (ix) An experiment showed that in a lead chloride solution, 6.21g of lead combined with 4.26 g. of chlorine. What is the empirical formula of this chloride. [Pb = 207; Cl = 35.5] (x) 2KClO 3 1. 2KCl + 3O2 Calculate the mass of KClO3 required to produce 6.72 litre of O2 at STP. [K = 39, CI = 35.5, O = 16]. [24.5g.] 2. Calculate the no. of moles of O 2 in the above volume and also the no. of molecules. [0.3 moles, 6.023 1023 0.3] (xi) 10g. of a mixture of NaCl and anhydrous Na2SO4 is dissolved in water. An excess of BaCl2 soln. is added and 6.99 g. of BaSO 4 is precipitated according to equation : Na2SO4 + BaCl2 BaSO4 + 2NaCl. Calculate the percentage of Na2SO4 in the original mixture. [O = 16; Na = 23; S = 32; Ba = 137] Chapter : Electrolysis Q.6. Answer the following : (i) Select the correct answer from the list in brackets : 1. An aqueous electrolyte consists of the ions mentioned in the list. The ion which could be discharged most readily during electrolysis. [Fe2+, Cu2+, H1+] .. 5 .. 2. The metallic electrode which does not take part in an electrolytic reaction. [Cu, Ag, Pt, Ni] 3. The ion which is discharged at the anode during the electrolysis of copper sulphate solution using copper electrodes as anode and cathode. [ Cu2+, OH1 , SO42 , H1+ ] 4. When dilute sodium chloride is electrolysed using graphite electrodes, the cation which is discharged at the cathode most readily. [Na1+, OH1 , H1+, Cl1 ] 5. During silver plating of an article using potassium argentocyanide as an electrolyte, the anode material should be. [Cu, Ag, Pt, Fe]. (ii) Give reasons : The electrolysis of acidulated water is considered to be an example of catalysis. (iii) Copper sulphate soln. is electrolysed using copper electrodes as seen in diagram. + Copper Copper Copper (a) Using copper electrodes 1. 2. 3. Which electrode to your left or right is known as the oxidising electrode and and why? Write the equation representing the reaction that occurs. State two appropriate observations for the above electrolysis reaction. Chapter : Metallugy Q.7. Answer the following : (i) The following is a sketch of an electrolytic cell used in the extraction of aluminium. 1. 2. 3. 4. What is the substance of which the electrodes A and B are made. At which electrode (A or B) is the aluminium formed. What are the two aluminium compounds in the electrolyte C. Why is it necessary for electrode B to be continuously replaced. + A B C .. 6 .. (ii) 1. Write three balanced equations for purification of bauxite by Hall s process in extraction of Al. 2. Name a chemical used for dissolving Al 2 O 3 . In which state of subdivision is the chemical used. 3. Write an equation for the reaction at the anode during the extraction of aluminium by the electrolytic process. 4. Mention one reason for the use of aluminium in thermite welding. Graphite rods (iii) A Pure aluminium Graphite rods Molten fluorides B Impure aluminium Iron container The sketch illustrates refining of aluminium by Hoope s process. [reference] 1. Which of A and B is the cathode and which one is the anode 2. What is the electrolyte in the tank. 3. What material is used for the cathode. Chapter : Organic Chemistry Q.8 Answer the following : (i) What is esterification? (ii) What is spurious alcohol? (iii) What is glacial acetic acid? (iv) Write balanced chemical equations for the following : 1. Reaction between 1, 2 - dibromoethane and alcoholic potassium hydroxide. 2. Monochloro ethane is hydrolysed with aqueous KOH. 3. A mixture of sodalime and sodium acetate is heated. 4. Ethanol under high pressure and low temperature is treated with acidified potassium dichromate. 5. Water is added to calcium carbide. 6. Ethanol reacts with sodium at room temperature. .. 7 .. (v) Choose the correct answer : 1. 2. 3. The functional group present in acetic acid is (a) Ketonic C = O (b) Hydroxyl - OH (c) Aldehydic - CHO (d) Carboxyl - COOH Unsaturated hydrocarbons undergo (a) a substitution reaction (b) an oxidation reaction (c) an addition reaction (d) none of the above The number of C-H bonds in ethane molecule are (a) Four (b) Six (c) Eight (d) Ten (vi) What is methylated spirit? (vii) What is denaturated alcohol? (viii) Give chemical equations for : 1. The laboratory preparation of methane from sodium acetate. 2. The reaction of one mole of ethene with one mole of chlorine gas 3. The preparation of ethyne from 1, 2 - dibromoethane. (ix) How are the following conversions carried out: 1. Ethyl choloride to Ethyl alcohol. 2. Ethyl chloride to Ethene. 3. Ethene to Ethyl alcohol. 4. Ethyl alcohol to Ethene. Note : 1. Learn all the defination properly word to word. 2. Alkane, Alkene, Alkyne, Alcohol, Acid-Lab preparation. 3. Study of compound [HCl, H2SO4, HNO3, NH3] 4. Study Lab. preparation and Industrial process. All the Best

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