(c) H2SO4 20 = Atomic number = Number of protons (or) Number of electrons Reason (R): The ratio of atoms in a molecule may be fixed and integral but may not be simple. Analyse the table and fill in the blanks. Question 13. Answer: Solution: Answer: Molar mass of CaCO3 = 40 + 12 + (16 × 3) = 100 g of moles (n) × (Gram molecular mass), (i) 2 moles of hydrogen molecule, H2 Which of the following contains the largest number of molecules? (d) 1 g of CH4 = 2 × 23 + 1 × 12 + 3 × 16 + 10 [(2 × 1) + (1 × 16)] (d) 1 g of C – 12 Answer: (i) Ion Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{32}{32}\) = 1 mole of sulphur. Solution: 6.23 × 1023 molecules of water = 1 mole = 445.6 × 1022 electrons ⇒ 11 – x = 10.804 amu (OR) (a) CaCO3 CH3Cl, CaCl2, NH3, PCl3, P2O5, H2O, C2H5OH [NCERT Exemplar] ____ and ____ are polyatomic molecules. Question 3. Compute the volume of water so consumed assuming the density of water to be lg cm-3. Calculation based on number of moles from mass and volume: Question 1. Number of atoms which a molecule to sulphur contains is _____. (b) C12H22O11 One molecule of an element contains 6.023 × 1023 atoms and it is equal to its gram atomic mass. (a) 1 g of CO2 How would you identify it without tasting? Give three significance of mole. (iii) 1 gram of carbon Question 2. It is also defined as the amount of substance which contains Avogadro number (6.023 × 1023) of particles. (b) Mass of a hydrogen atom (c) 2 g of He Answer: The stable isotope of carbon (C – 12) with atomic mass 12 is used as the standard for measuring the relative atomic mass of an element. Number of moles in 240 g of Mg metal = \(\frac{240}{40}\) = 10 Answer: (ii) 44.8 litres of sulphur dioxide at N.T.P. (v) 32 g of sulphur. = 62 u Answer: (b) Both (A) and(R) are wrong An ion is a charged particle and can be negatively or positively charged. Question 7. Let the fraction of relative abundance of B – 10 = x Calculate the ratio between the mass of one atom of hydrogen and mass of one atom of silver. Calculate the number of moles present in: II. (d) 100 g 1 gm atom of nitrogen represents: [NCERT Exemplar] (b) Cl– Na+ Question 26. ⇒ -x = 10.804 – 11 Carbon C – 12. Atomic mass of 1(O) = 1 × 16 = 16 = 4 × 10-1 (a) No. Answer: (Atomic mass: Al – 12, O – 16, S – 32) The gram atomic mass of oxygen is 16 g. Answer: Answer: Atomic mass of the element = \(\frac{\text { Molecular mass }}{\text { Atomicity }}=\frac{160}{3}\) = 53.33 u. 1 mole of Mg = 24 g = 6.023 × 1023 atoms (b) (A) is correct but (R) is wrong (a) 1 litre of N2 Which one of the following element is used as the standard for measuring the relative atomic mass of an element in now a days? (a) Molecular mass of H2CO3 = 2 × 1 + 1 × 12 + 3 × 16 True. Answer: (g) P4O10 ∵ Equal moles contains equal number of molecules. 1 mole of H atoms = 1 g Calcium carbonate: CaCO3 (d) C2H6 Question 18. Assertion (A): 18 g water contains Avogadro number (6.023 × 1023) of particles. (a) Both (A) and (R) are correct (a) He ∴ 5.49 × 10-4 mol of Al2O3 contains 2 × 5.49 × 10-4 mol of Al3+ ions (c) 98 g, Question 12. of moles = \(\frac{\text { Mass }}{\text { Atomic mass }}=\frac{46}{23}\) = 2. (b) 0.125 mole (a) 0.2 mole of H2 Answer: 56 × 2 = 112 g. Question 27. Distinguish between isotopes and isobars. = 120 u. Answer: Question 21. (b) 3.011 × 1012 If the atomic mass of sodium is 23 amu, then the mass of 3.011 × 1023 sodium atoms is _____. Question 6. Homo. 1000 g of calcium oxide give = \(\frac{40}{56} \times 1000\) (a) 1 litre of N2 of moles of Water = \(\frac { 90 }{ 18 }\) = 5 moles of water, No. One mole of water weighs 18 g. In three moles of ethane (C2H6), calculate the following: Question 5. Question 5. Atomic masses of Ca = 40, P = 30, O = 16. Gram molecular mass of 4 moles of P2 Solution: The percentage by weight of O2 in CaSO4. Solution: 0.3 mole of aluminium (Atomic mass of Al = 27). 2 × Vapour density is equal to _____. _____ determines the relation between molecular mass and vapour density. Chemical bonds. (j)5 (c) Noble gases, Question 14. A compound made up of two elements A and B has A = 70%, B = 30%. (a) 5 moles of CO2 and 5 moles of H20 do not have the same mass. (d) (A) is wrong but (R) is correct. (a) 18 g Answer: Calculate the number of moles in 12.046 × 1022 atoms of copper. x = % abundance of B – 10 = 0.196 × 100 = 19.6 % Volume occupied by NH3 = number of moles × molar volume (a) 0.5 mole (c) (A) is correct but (R) is wrong Answer: (b) One mole of oxygen gas contains Avogadro’s number of molecules. 40 g of calcium was extracted from 56 g of calcium oxide (Atomic mass of Ca = 40, O = 16) Question 8. e.g., \(_{1} \mathrm{H}^{1},_{1} \mathrm{H}^{2},_{1} \mathrm{H}^{3}\). = 1.51 × 1023 molecules, (c) 1 mole of carbon atoms contains 6.022 × 1023 atoms Correct Statement: Noble gases are monoatomic. Question 2. 1 molecule of methane contains electrons = 6 + 4 = 10 Solution: = 3.764 × 1022 molecules of CH4 Assertion (A): \(_{18} \mathrm{Ar}^{40}\) and \(_{20} \mathrm{Ca}^{40}\) are isobars. HCl, H2O, Question 10. (c) (ii) and (iii) Gram molecular mass of H2SO4 is: The atomic number of three elements A, B and C are 9, 10 and 13 respectively. Question 8. We know that one mol of alumina contains 2 mol of Al3+ ions. Answer: Let the fraction of relative abundance of B – 11 = y = \(\frac{1 \mathrm{mol}}{(22.4 \mathrm{L})} \times(44.8 \mathrm{L})\) = 2.0 mol. (e) CO The volume occupied by one mole of any gas at STP is called molar volume. Heterodiatomic molecules. (b) Whose container has more number of atoms? Answer: Question 27. Answer: Give any two examples for heteroatomic molecules. Answer: (a) 46 g of Na atom Answer: Number of molecules = \(\frac{6.023 \times 10^{23} \times 360}{180}\) Mass % of Nitrogen = \(\frac{14}{17} \times 100\) = 82.35%. = 3.34 × 1022 molecules, Question 3. Ca : O × 2 : H × 2 Antoine L. Lavoiser and Joseph L. Proust. = 180 g Reason (R): They have the same atomic mass but a different atomic number. Thus, Krish’s container is heavier. (a) Ozone Answer: Empirical formula, molecular formula. (b) 1 atom of He 2013–2015 Morrill Professor, Iowa State University. (a) \(_{17} \mathrm{Cl}^{35},_{17} \mathrm{Cl}^{37}\), Question 2. 5 × 1023 molecules of glucose? The Earth is 2400 times heavier than one mole of screws. 24 : 35.5 × 2 Atomic mass of 4(H) = 4 × 1 = 4 g Question 6. (a) 0.5 Question 57. Glucose has a molar mass of 180.16 g/mol. 2013-2014 Visiting Lecturer, University of Oregon. (b) 44 g a – ii, b – iii, c – v, d – i, e – iv. (d) 8. Pages (550 words) Approximate price: $ 22. \(\begin{array}{l}{\% \text { of } \mathrm{S} \text { in } \mathrm{H}_{2} \mathrm{SO}_{4}=\frac{\text { Mass of sulphur }}{\text { Molar mass of } \mathrm{H}_{2} \mathrm{SO}_{4}} \times 100} \\ {\% \text { of } \mathrm{S} \text { in } \mathrm{H}_{2} \mathrm{SO}_{4}=\frac{32}{98} \times 100}\end{array}\) Correct Statement: The gram atomic mass of an element is expressed in the unit grams. Answer: Mass of glucose = \(\frac{180 \times 2 \times 10^{24}}{6.023 \times 10^{23}}\) = 597.7 g. Question 26. (b) 240 g of calcium and 240 g of magnesium elements have a mole ratio of 3 : 5. Atomicity = \(\frac{\text { Molecular mass }}{\text { Atomic mass }}\), Homoatomic molecule: The molecules which are made up of atoms of the same element are called Homoatomic molecule, e.g., N, Heteroatomic molecule: The molecules which are made up of atoms of different elements are called Heteroatomic molecule, e.g., NH. (d) \(_{33} \mathrm{As}^{77},_{34} \mathrm{Se}^{78}\). H2 (g) + O2 (g) → 2H2O (g) (At. Which one of the following is the most abundant element in both the Earth’s crust and in the human body? Hint: % by weight of O2 = \(\frac{64}{136}\) × 100 = 47.05 %. Answer: Question 56. (d) Protium A molecule is the smallest particle of an element or compound. Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{1.4}{7}\) = 0.2 mole of lithium. Mass of oxygen = 16 × 2.5 = 40 g. Question 22. Question 11. Answer: Answer: Question 5. Each NaCl particle is equivalent to 2 ions, i.e., one Na2 and one Cl– where ‘W is the mass of the substance in which number of molecules is to be calculated and ‘M’ is the molecular mass of the substance. (iii) According to Avogadro’s law, equal volumes of all gases contain equal number of molecules. 1 mol of water contains 2 × 6.022 × 1023 atoms of hydrogen No. Correct statement: The number of atoms present in one molecule of an element is called the atomicity of an element. \(=\frac{5}{40}=\frac{1}{8}\) = 0.125 mole. (c) Both (A) and (R) are correct (d) relative atomic mass. True. Atoms of the same element that have same atomic number but different mass number are called isotopes. Answer: A flask P contains 0.5 moles of oxygen gas. A colourless liquid is thought to be a pure compound. = 72 + 12 + 96 Question 10. Number of molecules of water = 6.023 × 1023 × \(\frac { 54 }{ 18 }\) The volume of H2 required to form 6 dm3 of NH3 is: Question 58. Answer: Density of water = 1.0 g/mL = 3.011 × 1023 molecules of CO2. (c) 1022 molecules of CO2 5.6 litre of Oxygen at S.T.P? Answer: Molecular mass of gaseous element = 80 × 2 = 160 u Gram molecular mass of 5 moles of S2 Same, different. One mole of screw weighs = 2.475 × 1024 g = 2.475 × 1021 kg Answer: = 3 × 71 = 213 g, (iii) 5 moles of sulphur molecule, S2 Question 9. 20 : 16 : 1. (b) valency Question 11. (d) (A) is wrong but (R) is correct. Answer: Assertion (A) & Reason (R): Mass of 20 moles of water = 18 × 20 = 360 g. (iii) 6.023 × 1023 molecules of water = 1 mole = 18 g. (iv) 1.2044 × 1025 molecules of water (b) 18 g of O2 (a) Atomic masses of the elements A and B. Answer: Answer: Relative atomic mass is otherwise known as _____. Question 34. 6.022 × 1022 molecules of oxygen = 1 mol × \(\frac{6.022 \times 10^{22}}{6.022 \times 10^{23}}\) = 0.1 mol. (c) O3. = \(\frac{40}{64}\) = 0.625 moles Answer: Answer: Compute the difference in masses of one mole each of aluminium atoms and one mole of its ions. The weight % of Mg as 2.68 = 6.613 × 1020 ions of Al3+, Question 3. = 2.151 × 1022 molecules of N2. Calculate the number of moles in 46 g of sodium. (c) relative molecular mass Eg: isotopes 17Cl35, 17Cl37. Answer: Answer: Solution: Atomicity of chlorine = \(\frac{48}{16}\) = 3. Carbon dioxide produced by action of dilute hydrochloric acid on potassium hydrogen carbonate is moist whereas that produced by heating potassium hydrogen carbonate is dry. Hint: Molar mass = 12 + (16 × 2) = 44 g. Question 30. Answer: (a) 1 mole 44 g (molar mass) of CO2. Answer: (a) O2 Answer: (a) Both (A) and (R) are correct, Question 10. (b) Nitrogen (a) 2 Question 2. = 0.5 mole. Question 4. Atomic mass of N2 = 2 × 14 = 28 g (i) 8 We know that one mole of sodium contains 6.022 × 1023 atoms. 44.8 litres of sulphur dioxide at N.T.P. 2 : 32 : 64 Molecular mass of NO2 = 14 + 32 = 46 g. (v) H2SO24 Atomic mass of 3(N) = 3 × 14 = 42 Question 34. Question 24. (d) \(\mathrm{NO}_{3}^{-}\) \(\mathrm{NH}_{4}^{+}\), Question 2. (d) 12. \mathrm{TP}}{22.4}}\end{array}\) (a) 22.4 ml 40 g of calcium = 1 mol (iv) It determines the relation between molecular mass and vapour density. Answer: 1 mole of carbon atoms weigh = 12 g (d) 1 mole atoms of He = 4 g = 0.004 kg. (b) 5.6 litre Question 1. It is used to determine the atomicity of gases. Calculate the number of moles of a sample that contains 12.046 × 1023 atoms of iron? (b) \(6^{\mathrm{O}^{12}}\) True. Answer: Molecules are of two types: Question 1. (b) 3.011 × 1023 (c) (A) is wrong but (R) is correct H2 and O2 react according to the equation Number of ions = 0.2 × 6.022 × 1023 ⇒ Total moles of ions = 0.1 × 2 = 0.2 moles Computing Molecular Mass for a Covalent Compound Ibuprofen, C 13 H 18 O 2, is a covalent compound and the active ingredient in several popular nonprescription pain medications, such as Advil and Motrin.What is the molecular mass (amu) for this compound? False. (iv) What mass of calcium will be obtained from 1000 g of calcium oxide? Answer: Solution: Answer: (i) 1 mole of chlorine molecule, Cl2 (ii) How many moles of gas molecules are obtained from 1 mole of nitroglycerine? Volume occupied by N2 at S.T.P = No. 1 molecule of ozone (O3) = 3 atoms of oxygen = \(\frac{\text { Mass of a given volume of gas or vapour at S.T.P }}{\text { Mass of same volume of hydrogen }}\). Give an example of a triatomic molecule of an element. Solution: Number of molecules = Number of moles × Avogadro number Mass = 0.25 × 18 (d) 2 g of H2. 6.022 × 1022 molecules of oxygen = 1 mol = 6.022 × 1023 atoms of hydrogen, (c) 1 molecule of water contains 1 atom of oxygen Molar volume at S.T.P = \(\frac { 46 }{ 23 }\) = 2 moles Atomicity of Nitrogen is _____ whereas the atomicity of Helium is _____. Answer: True. Reason (R): 1 molecule of ozone contains 3 atoms of oxygen. Which has the highest number of molecules? Calculate % of S in H2SO4 (a) 22.4 litre Answer: Solution: Question 2. (c) 11.2 L of N2 at STP Find the gram molecular mass of the following from the data given: (Atomic mass of Na = 23, C = 12, H = 1, O = 16) (iv) Atoms of one element can be transmuted into atoms of other elements. Question 12. One gram of which of the following contains the largest number of oxygen atoms? Define the Avogadro number. (b) Protium \(_{1} \mathrm{H}^{1}\) The volume occupied by 4.4 g of CO2 at S.T.P is _____. Atoms of one element can be transmuted into atoms of other elements by _____. Volume of gas at STP is 1.12 × 10-7 cc. Which of the following pair indicates isotopes? Assertion (A): The atomicity of ozone is three. (d) none Question 36. (i) H2O (b) Glucose Correct statement: Equal volume of all gases under similar conditions of temperature and pressure contain the same number of molecules. Correct statement: The number of atoms present in the molecule is called its Atomicity. Mass of one atom = \(\frac{1}{6.022 \times 10^{23}}\)g 16 g of methane contain molecules = 6.022 × 1023 Question 4. Which one is heavier? [NCERTExemplar] Give the salient features of ‘Modern atomic theory’. Gram molar mass of H2O = (1 × 2) + (16 × 1) = 2 + 16 Calculate the formula mass of sodium carbonate (Na 2 CO 3.10H 2 O). The number of molecules in 16.0 g of oxygen is _____. 3.011 × 1023 of ammonia gas molecules? (d) isomers. Answer: Answer: Assertion (A): \(_{1} \mathrm{H}^{1}, \quad_{1} \mathrm{H}^{2},_{1} \mathrm{H}^{3}\) are the isotopes of hydrogen. Mole is defined as the amount of substance that contains as many specified elementary particles as the number of atoms in 12 g of C-12 isotope. Ozone (O3). (g) 14 Answer: Answer: ∴ 2 g of chlorophyll will contain Mg Answer: Question 18. Hetero atomic molecule. Answer: Modem methods of determination of atomic mass by _____ use C – 12 as standard. True. ∴ 0.0046 mole of gold will contain = 0.0046 × 6.022 × 1023 (a) nucleus Question 9. Samacheer Kalvi 10th Science Book Solutions, Samacheer Kalvi 11th Bio Botany Solutions Chapter 12 Mineral Nutrition, Samacheer Kalvi 11th Bio Botany Solutions Chapter 10 Secondary Growth, Samacheer Kalvi 11th Bio Botany Solutions Chapter 7 Cell Cycle, Samacheer Kalvi 11th Bio Botany Solutions Chapter 8 Biomolecules, Samacheer Kalvi 11th Bio Botany Solutions Chapter 11 Transport in Plants, Samacheer Kalvi 11th Bio Botany Solutions Chapter 13 Photosynthesis, Samacheer Kalvi 11th Bio Botany Solutions Chapter 9 Tissue and Tissue System, Samacheer Kalvi 11th Bio Botany Solutions Chapter 4 Reproductive Morphology, Samacheer Kalvi 11th Bio Botany Solutions Chapter 14 Respiration, Samacheer Kalvi 11th Bio Botany Solutions Chapter 15 Plant Growth and Development, Samacheer Kalvi 12th Accountancy Solutions Chapter 6 Retirement and Death of a Partner, i. Isobars. 1 mole of any substance contains ______ molecules. ‘Dalton’s atomic theory is contradicted by the formula of sucrose (C12H22O11).’ Justify the statement. ∴ 0.1 mole of CCl4 = 0.1 × 6.022 × 1023 molecules of CCl4 Answer: 5 moles of H2O = 5 × 18 = 90 g, (ii) 1 mole of Glucose (C6H12O6) The metals Cu, Ag, Au are _____ elements. (c) 1.25 mole The volume occupied by NH3 in glass bulb A is three times more than the volume occupied by HCl in glass bulb B at STP. Correct statement: O2, N2, H2, Cl2, Br2, F2, I2 are homo diatomic molecules. The statement does not clarify whether we are talking about atoms or molecules of nitrogen. (c) 28 g (d) 1 g of Fe Question 8. Answer: ∴ 8 g of O2 contains = \(\frac{6.022 \times 10^{23}}{32}\) × 8 molecules (c) 18 u (a) \(_{1} \mathrm{H}^{2}\) How many (a) molecules (b) hydrogen atoms (c) oxygen atoms are there in 0.5 mol of water? 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