No. [NCERT Exemplar] (b) Hydrogen chloride, Question 19. Question 5. (a) Atomic number (a) 6.023 × 10-23 (b) 2 (i) A group of atoms carrying a charge 1.008 amu. (ii) Mass of sodium bicarbonate in this equation is mass of 2 moles of NaHCO3. Atomic mass of sulphur = 32 One mole of screw weighs = 2.475 × 1024 g = 2.475 × 1021 kg The statement does not clarify whether we are talking about atoms or molecules of nitrogen. (d) 1.5 × 1023 (d) 100 g (a) 0.5 mole Atoms of different elements join together in definite proportions to form molecules of compounds. Answer: Atomicity of Nitrogen is _____ whereas the atomicity of Helium is _____. Number of molecules = \(\frac{(\text { Avogadro number } \times \text { Given mass })}{\text { Gram molecular mass }}\) (b) 1.8 g (c) Avogadro’s law. = 12.046 × 1023 molecules. i.e. Answer: Mass of CaO = \(\frac{56 \times 12.046 \times 10^{23}}{6.023 \times 10^{23}}\) Solution: (b) 2 litres of oxygen Analysis What are the types of molecules? Hint. = 7.23 × 1022 atoms An ion is a charged particle and can be negatively or positively charged. ⇒ Total moles of ions = 0.1 × 2 = 0.2 moles (g) P4O10 No. Give the salient features of ‘Modern atomic theory’. What are isotones? 5.6 litre of Oxygen at S.T.P? Find the mass of 2.5 moles of oxygen atoms. of molecules = \(\frac{6.023 \times 10^{23} \times 1}{16}\) One gram of which of the following contains the largest number of oxygen atoms? (b) 11.2 Which of the following will have maximum mass? Question 8. How many moles are present in 4 g of sodium hydroxide? A sample of ammonia weighs 3.00 g. What mass of sulphur trioxide contains the same number of molecules as are in 3.00 g ammonia? 2.24 litre of SO2 gas at S.T.P? Hint: Molar mass = 12 + (16 × 2) = 44 g. Question 30. Question 6. Answer: Answer: Question 1. Question 6. Total number of electrons present in 1.7 g of NH3 is: V.D = \(\frac{\text { Mass of } 1 \text { molecule of a gas or vapour at S.T.P. (i) It explains Gay-Lussac’s law. Answer: 6.23 × 1023 molecules of water = 1 mole 1 mole of SO3 weighs 80 g 5.85 g of NaCl = \(\frac{5.85}{58.5}\) = 0.1 moles Question 2. Question 3. (c) H2—It is a covalent compound True. Ca : C : O × 3 Atomic masses of H = 1, O = 16 Question 14. Answer: (c) Aluminium AL Answer: True. How many molecules are there in a certain mass of a substance? Mass of the substance = \(\frac{\text { Gram molecular mass } \times \text { Number of particles }}{\text { Avogadro number }}\) Molecular mass of H2O = 18 (b) 3.011 × 1023 [Given mass of a dot = 10-18 g] Question 13. 5 moles of CO2 have molar mass = 44 × 5 = 220 g Anions Cations = 0.625 × 44 (a) 16 g \(_{20} \mathrm{Ca}^{40}\) contains 20 protons, 20 electrons and 20 neutrons. (ii) 44.8 litres of sulphur dioxide at N.T.P. Question 21. Deriving the Number of Atoms and Molecules from the Mass of a Compound A packet of an artificial sweetener contains 40.0 mg of saccharin (C 7 H 5 NO 3 S), which has the structural formula: Given that saccharin has a molar mass of 183.18 g/mol, how many saccharin molecules are in a 40.0-mg (0.0400-g) sample of saccharin? True. Question 41. Answer: Answer: Give two examples. Assertion: Atomic mass of aluminium is 27 The number of _____ present in the molecule is called its atomicity. (b) (A) is correct but (R) does not explain (A) ∴ 10-18 g of carbon will have \(\frac{6.022 \times 10^{23}}{12} \times 10^{-18}\) × 10-18 carbon atoms Gram atomic mass of Ca = 40 g (v) 1023 atoms of calcium. (e) CO (b) 240 g of calcium and 240 g of magnesium elements have a mole ratio of 3 : 5. 22.4 litres. (c) 5 Compounds composed of metals and non-metals contain charged species. Number of moles of O2 \(=\frac{\text { Volume at S.T.P }}{\text { Molar volume }}\) \(=\frac{3}{22.4}\) = 0.1339 moles Answer: of moles of Ammonia = \(\frac { 5.1 }{ 17 }\) = 0.3 moles of ammonia, No. Answer: Chemical bonds. Complete the table given below. (iv) 1.4 g of lithium Hint: By definition 1 amu is defined as precisely 1 / 12th the mass of an atom of carbon – 12. (d) 8 Molecular mass of NaCl = (1 × 23 + 1 × 35.5) u = 58.5 u The volume occupied by 4.4 g of CO2 at S.T.P is _____. = 2 + 12 + 48 = 2 × 27 u + 3 × 16 u \(\begin{array}{l}{\text { Number of moles of } \mathrm{CO}_{2}=\frac{\text { Given volume at S.T.P }}{\text { Molar volume at S.T.P }}} \\ {\qquad 2.5 \text { mole of } \mathrm{CO}_{2}=\frac{\text { Volume of } \mathrm{CO}_{2} \text { at } \mathrm{S} . (a) (A) is correct and (R) explains (A) Question 31. The number of atoms present in the molecule is called the Avogadro number. Answer: Question 13. 1 mole of Ca (….. g) and 1 mole of the Oxygen atom (…… g) combine to form mole of CaO (….. g). = 24 × \(\frac{78.99}{100}\) + 25 × \(\frac{10}{100}\) + 26 × \(\frac{11.01}{100}\) H2O has molar mass = 18 g mol-1 Calculate. Write the cations and anions present (if any) in the following compounds: Question 3. All noble gases are _____ molecules. [NCERT Exemplar] Question 11. of moles of Sodium = \(\frac { 4.6 }{ 23 }\) = 0.2 moles of sodium, No. ⇒ 11 – x = 10.804 amu 1.2046 × 1024 glucose molecules. Does the solubility of a substance change with temperature? Compute the number of ions present in 5.85 g of sodium chloride. True. (a) Ozone Question 1. (Atomic mass: Al – 12, O – 16, S – 32) (c) (A) is correct but (R) is wrong, Question 3. (d) 18 g of CH4. (b) 8 (S8), Question 44. = 6.613 × 1020 ions of Al3+, Question 3. (c) relative molecular mass. Atomic mass of 2(O) = 2 × 16 = 32 The formula of Calcium oxide is CaO. Solution: ∴ 1.2044 × 1025 molecules (a) (A) is correct and (R) explains (A), Question 8. or, 3 : 5, Question 5. The volume occupied by one mole of any gas at STP is called molar volume. (b) 22.4 litres Same, different. (a) 9 dm³ Answer: Number of moles = \(\frac{\text { Mass of Al }}{\text { Atomic mass of Al }}\) (c) 640 moles Mass of 1 mole of water = 18 g (a) 6.023 × 1023 (i) H2O Answer: Question 38. Answer: No. The molecular formula of gases can be derived using Avogadro’s law. An isotope of hydrogen without neutrons is _____. = 120 u. Mass of 1 mole of NaHCO3 = 84 g Answer: (c) CH4 (c) Molecular mass of MgSO4 =1 × 24 + 1 × 32 + 4 × 16 (ii) How many moles of gas molecules are obtained from 1 mole of nitroglycerine? (b) 21 Answer: = 0.8064 × 1023 Gram molar mass of H2O = 18 g. (ii) CO2 Also, 1 mole of carbon atoms = 6.0 2 2 × 1023 atoms Answer: (b) 6.023 × 1023 atoms of hydrogen and 6.023 × 1023 atoms of oxygen CO2 = molar mass = 44 g (c) Oxygen, Question 11. (b) 10 dm³ In case we need more time to master your paper, we may contact you regarding the deadline extension. (b) 44 g Answer: Answer: (a) 9 (a) 1 litre of N2 You can Download Samacheer Kalvi 10th Science Book Solutions Guide Pdf, Tamilnadu State Board help you to revise the complete Syllabus and score more marks in your examinations. Answer: Which one of the following represent Avogadro’s law? 18 g of water contains = 6.02 2 × 1023 molecules Avogadro number represents the number of atoms in _____. Molecular mass of oxygen = 32 u (ii) 44.8 litres of sulphur dioxide at N.T.P. Question 1. 10 : 3 : 12, (b) MgCl2 (c) Both (A) and (R) are correct. (i) 392 g of sulphuric acid (a) Incorrect, the correct symbol of cobalt is Co. Gram molecular mass of water =18 g/mol Calculate the mass of CO2 which contains the same number of molecules as are contained in 40 g of SO2. % relative abundance of B – 11 = ? Differentiate between the actual mass of a molecule and gram molecular mass. Answer: Samacheer Kalvi 10th Model Question Papers. (c) Both (A) and (R) are correct Reason (R): Atoms of the same element have the same atomic number but a different mass number. Answer: An atom is the smallest particle of an element. Calculate the mass per cent of each element present in the molecule of calcium carbonate. Molecular mass of H2O = 2 × lu + 1 × 16u = 18u Question 3. Answer: (a) 3.011 × 1020 Question 1. False. ∴ 1023 atoms of Ca have mass = \(\frac{40}{6.02 \times 10^{23}}\) × 1023 = 6.64 g Yes, it is a temperature dependent property. Define Mole. The value of gram molar mass of CO2 is _____. (c) 4 moles Question 23. (i) 1 mole of CO2= 44 g = 6.02 × 1023 molecules Molar mass of CaCO3 = 40 + 12 + (16 × 3) = 100 g Dalton’s atomic theory states that atoms of different elements combine together in simple whole number ratio. Mass % of Oxygen = \(\frac{16}{18} \times 100\) = 88.89 %. (b) valency (i) 3.011 × 1023 number of oxygen atoms. False. Question 60. (d) 22400. (d) \(_{33} \mathrm{As}^{77},_{34} \mathrm{Se}^{78}\). The average atomic mass of an element becomes fractional due to the presence of ______. Hetero triatomic. Gram molecular mass of glucose = 180 g Question 23. Answer: Molar volume of CO2 = 22.4 litre. Answer: Question 19. (b) Carbon c (ii) (A) is correct (R) is wrong Answer: Which of the following pair is an example of isotopes? Relative abundance = x (10) + (1 – x) (11) = 10.804 amu (a) Both (A) and (R) are correct How is Average atomic mass calculated? (c) Hydrogen Question 42. The value of Gram molar volume at STP is 11.2 litres. (a) Atomic masses of the elements A and B. In the nucleus of \(_{20} \mathrm{Ca}^{40}\), there are _____. Required fields are marked *. One mole of a gas occupies a volume of 22.4 L. This is derived from _____. Question 34. (c) Methane (c) Atomic mass Which of the following are tri-atomic and tetra-atomic molecules? Gram molar mass of NaOH = 40 g, (b) C12H22O11 (Sucrose) (b) 18 g, Question 23. 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