3. Which postulate of Dalton s atomic theory is the result of the law of conservation of mass?
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1 1 1. In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium ethanoate. Show that these observations are in agreement with the law of conservation of mass. sodium carbonate + ethanoic acid sodium ethanoate + carbon dioxide + water Mass of the reactants = Mass of sodium carbonate + Mass of ethanoic acid = =11.3 g Mass of products = Mass of carbon dioxide + Mass of water + Mass of sodium ethonate = = 11.3 g Since the mass of products is equal to the mass of reactants, mass is neither created nor lost during the given chemical change and the observation made is in agreement with the law of conservation of mass. 2. Hydrogen and oxygen combine in the ratio of 1:8 by mass to form water. What mass of oxygen gas would be required to react completely with 3 g of hydrogen gas? X grams of hydrogen 8 x gram of oxygen will be required to form water. Oxygen required to react with 3 g hydrogen to form water = 3 8 = 24 g. 3. Which postulate of Dalton s atomic theory is the result of the law of conservation of mass? Atoms are indivisible particles, which cannot be created nor destroyed in a chemical reaction. 4. Which postulate of Dalton s atomic theory can explain the law of definite proportions? The relative number and kinds of atoms are constant in a given compound. 5. Define the atomic mass unit. One atomic unit is a mass unit equal to exactly one twelfth (1/12 th ) the mass of one atom of carbon Why is not possible to see an atom with naked eye? The size of an atom is very small. So it is impossible to see an atom with naked eye. 7. Write down the formulae of (i) sodium oxide 1
2 2 (ii) aluminium chloride (iii) sodium suphide (iv) magnesium hydroxide The formulae are: i) sodium oxide- Na 2 O (ii) aluminium chloride-alcl 3 (iii) sodium suphide-na 2 SO 3 (iv) Magnesium hydroxide - Mg(OH) 2 8. Write down the names of compounds represented by the following formulae: (i) Al 2 (SO4) 3 (ii) CaCl 2 (iii) K 2 SO 4 (iv) KNO 3 (v) CaCO 3. The names of compounds are as follows: (i) Al 2 (SO4) 3 aluminium sulphate (ii) CaCl 2 Calcium chloride (iii) K 2 SO 4 potassium sulphate (iv) KNO 3 potassium nitrate (v) CaCO 3 - calcium carbonate 9. What is meant by the term chemical formula? The chemical formula of a compound is a symbolic representation of its composition. 10. Calculate the molecular masses of H 2, O 2, Cl 2, CO 2, CH 4, C 2 H 6,C 2 H 4, NH 3, CH 3 OH. Molecular mass of H 2 = 1+ 1 = 2u Molecular mass of O 2 = = 32 u Molecular mass of Cl 2 = = 71 u Molecular mass of CO 2 = = 44u Molecular mass of CH 4 = = 16 u Molecular mass of C 2 H 4 = = 28 u Molecular mass of C 2 H6 = = 30 u Molecular mass of NH 3 = = 17u Molecular mass of CH 3 OH. = = 32 u 11. Calculate the formula unit masses of ZnO, Na 2 O, K 2 CO 3, given atomic masses of Zn = 65 u, Na = 23 u, K = 39 u, C = 12 u, and O = 16 u. Formula unit mass of ZnO = = 81 u Formula unit mass of Na 2 O = = 62 u Formula unit mass of K 2 CO 3 = = 138 u. 2
3 3 12. If one mole of carbon atom weighs 12 gram, what is the mass (in gram) of 1 atom of carbon? 1 mole of carbon atom = atoms Now atoms of carbon weigh 12 grams one atom of carbon weighs = = g g sample of compound of oxygen and boron was found to contain g of boron and g of oxygen on analysis. Calculate the percentage composition of the compound by weight. % of boron in the sample = 100 = 40% % of oxygen in the sample = 100 = 60% The sample of compound contains 40% boron and 60% oxygen by weight. 14. When 3.0 g of carbon is burnt in 8.00 g of oxygen, g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in g of oxygen? Which law of chemical combination will govern your answer? The mass of the carbon dioxide formed will be only 11 grams. The remaining oxygen is not used up. This indicates the law of definite proportions which says that in compounds, the combining elements are present in definite proportions by mass. 15. What are polyatomic ions? Give examples. When two or more atoms combine together and behave like one entity with a net charge, then it is called polyatomic ion. For example oxygen atom and hydrogen atom combine to form hydroxide ion (OH - ). One carbon atom and three oxygen atoms act as carbonate ion (CO 3-2 ). 16. Write the chemical formulae of the following. (a) Magnesium chloride (b) Calcium oxide (c) Copper nitrate (d) Aluminium chloride (e) Calcium carbonate. The chemical formulae for the following are (a) Magnesium chloride MgCl 2 (b) Calcium oxide -CaO (c) Copper nitrate Cu(NO 3 ) 2 3
4 4 (d) Aluminium chloride AlCl 3 (e) Calcium carbonate. CaCO Give the names of the elements present in the following compounds. (a) Quick lime (b) Hydrogen bromide (c) Baking powder (d) Potassium sulphate. The names of the elements present in in the following compounds are (a) Quick lime calcium and oxygen (b) Hydrogen bromide-hydrogen and bromide (c) Baking powder Sodium, hydrogen, carbon and oxygen (d) Potassium sulphate- Potassium, sulphur and oxygen. 18. Calculate the molar mass of the following substances. (a) Ethyne, C 2 H 2 (b) Sulphur molecule, S8 (c) Phosphorus molecule, P4 (Atomic mass of phosphorus = 31) (d) Hydrochloric acid, HCl (e) Nitric acid, HNO 3 The molar mass of the following substances are (a) Ethyne, C 2 H = 26 u (b) Sulphur molecule, S = 256 u (c) Phosphorus molecule, P = 124 u (d) Hydrochloric acid, HCl = 36.5 u (e) Nitric acid, HNO = 63 u 19. What is the mass of (a) 1 mole of nitrogen atom (b) 4 moles of aluminium atoms (Atomic mass of aluminium = 27)? (c) 10 moles of sodium sulphite (Na 2 SO 3 )? a) 1 mole of nitrogen atom =14 u = 14 gm (b) 4 moles of aluminium atoms = 4 27 = 108 u = 108 gram (c) 10 moles of sodium sulphite = 10 (126 gram) = 1260 grams 20. Convert into mole. (a) 12 g of oxygen gas (b) 20 g of water (c) 22 g of carbon dioxide. a)32 gram of oxygen gas = 1 mole 12 grams of oxygen gas = = mole b) 18 grams of water = 1 mole 20 grams of water = = 1.1 mole 4
5 5 c) 44 grams of carbon dioxide = 1 mole 22 grams of carbon dioxide = 0.5 mole 21. What is the mass of: (a) 0.2 mole of oxygen atoms? (b) 0.5 mole of water molecules? 1 mole of oxygen atoms = 16 grams 0.2 moles of oxygen atoms = = 3.2 grams b. 1 mole of water molecules = 18 grams 0.5 mole of water molecules = = 9 grams 22. Calculate the number of molecules of sulphur (S 8 ) present in 16 g of solid sulphur. 1 mole of S 8 = 32 8 = 256 grams 1 mole of S 8 = molecules 256 grams S 8 has = grams S 8 has = 16 = molecules. 23. Calculate the number of aluminium ions present in g of aluminium oxide. (Hint: The mass of an ion is the same as that of an atom of the same element. Atomic mass of Al = 27 u) 1 mole of aluminium oxide = = 102 grams 102 grams aluminium oxide has = aluminium oxide molecules 0.56 gram of aluminium oxide has = = aluminium oxide molecules 1 molecule of aluminium oxide gives = 2 Al +++ ions Hence 0.56 grams aluminium oxide gives = Al +++ ions. = aluminium ions 5
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