No. Hint: By definition 1 amu is defined as precisely 1 / 12th the mass of an atom of carbon – 12. The average atomic mass of carbon is ______. Question 1. (b) Avogadro number Question 11. (d) (A) is wrong but (R) is correct. Question 5. Answer: = 714.285 g of calcium Answer: Answer: 44 g of CO2 occupied 22.4 litre of volume. Total number of electrons present in 1.7 g of NH3 is: 1 mole of oxygen gas = 6.022 × 1023 molecules ∴ 5.49 × 10-4 mol of Al2O3 contains 2 × 5.49 × 10-4 mol of Al3+ ions (iv) 1.4 g of lithium In three moles of ethane (C2H6), calculate the following: Question 5. (d) 8 (d) \(\mathrm{NO}_{3}^{-}\) \(\mathrm{NH}_{4}^{+}\), Question 2. Mass of 2 moles of H2 molecule Answer: (a) 0.1 mole of NH3 has 6.023 × 1023 atoms. In accordance with the number of atoms present in the molecules, they are classified as monoatomic, diatomic, triatomic and polyatomic molecules showing that they contain one, two, three or more than 3 atoms respectively. (a) 6.023 × 1023 = 3.011 × 1023 molecules. Mass of 1 mole of water = 18 g Answer: (b) Helium Number of moles = \(\frac{\text { S.T.P. False. Percentage abundance of B – 10 = 19.6 % Which of the following is a triatomic molecule? Question 27. (b) 2 An atom is no longer indestructible. Relative abundance = x (10) + (1 – x) (11) = 10.804 amu The average atomic mass of carbon is _____. Answer: Question 16. Question 26. (d) All contain the same 2 × Vapour density. Compounds composed of metals and non-metals contain charged species. (b) Incorrect, the correct symbol of carbon is C. Answer: Solution: Answer: Question 9. (b) 1.8 g Formula = No. The vapour density is defined as the ratio between the masses of equal volumes of a gas (or vapour) and hydrogen under the same condition. A molecule is the simplest structural unit of an element or compound which contains one or more atoms. (d) Both (A) and (R) are correct. _____ are the building blocks of matter. (d) 3.011 × 1024 (b) Gold Mg – 24 = 78.99% , Mg – 25 = 10%, Mg – 26 = 11.01% (a) 6.023 × 1023 Answer: = 4 × 124 = 496 g. Question 2. Answer: How many grams of water would be required to produce 18 g of glucose? (R) explain (A) Density of oxygen = \(\frac{32}{2}\) = 16 u (d) Ammonia. 2 : 32 : 64 (ii) How many moles of oxygen atoms are there in this? Which of the following are tri-atomic and tetra-atomic molecules? = 100 g. (iii) How many moles of CO2 are there in this equation? Question 46. ∴ 0.5 mol of water contains \(\frac{6.022 \times 10^{23}}{2}\) atoms of oxygen }}\end{array}\). Answer: (d) 3 × 1010. (d) 2 moles (c) 2.5 × 1023 Hint: (d) 1 mole atoms of He. Thus, 12 g of carbon atoms has 6.022 × 1023 atoms. Answer: Answer: Question 60. = 149.43 g. IV. Gram molecular mass of CO2 = 44 g When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium chloride. (b) 4 moles = \(\frac{6.023 \times 10^{23} \times 11}{44}\) (a) 11.2 litre Which of the following contains maximum number of molecules? Answer: (a) diatomic (b) Deuterium (b) 2 litres of H2 Answer: Question 6. (d) 12.046 × 1023. Atomicity of Nitrogen is _____ whereas the atomicity of Helium is _____. Molar mass of CaCO3 = 40 + 12 + (16 × 3) = 100 g Calcium carbonate is decomposed on heating in the following reaction CaCO3 → CaO + CO2 (d) Protium (b) One mole of oxygen gas contains Avogadro’s number of molecules. Question 10. (i) H2O % of O = \(\frac{16}{18}\) × 100 = 88.89% Find the gram molecular mass of the following from the data given: Atomic mass of O3 = 3 × 16 = 48 g False. (d) Helium He Ignore if with different plant species / different abiotic variables 1 max 1 2 Total 7 marks Mass of 1 mole of aluminium atom = Molar mass of aluminium = 27 g mol-1. Mass of SO2 = 6.4 g. Question 3. Atomic masses of C = 12, O = 16 (d) Dalton’s law. (a) 1 g of CO2 ∴ Average atomic mass of Magnesium is 24.3202 amu. (g) P4O10 Mass of 1 mole of water = 18 g A molecule is a combination of two or more atoms held together by _____. = 6.023 × 1021 water molecules, Question 2. \(_{18} \mathrm{Ar}^{40},_{20} \mathrm{Ca}^{40}\), (b) \(_{6} \mathrm{C}^{13},_{7} \mathrm{N}^{14}\), (c) \(_{1} \mathrm{H}^{1},_{1} \mathrm{H}^{2},_{1} \mathrm{H}^{3}\), (d) \(_{18} \mathrm{Ar}^{40},_{20} \mathrm{Ca}^{40}\). 40 g of calcium = 1 mol (iii) 6.022 × 1022 molecules of oxygen [V ∝ n]. Answer: Molar mass of Al3+ = (27 – 0.00164) g mol-1 Others are less. (d) (A) is wrong but (R) is correct. False. Answer: Atom does not exist in the free state except in a noble gas, Except some of the noble gas, other atoms are highly reactive, Atoms in a molecule are held by chemical bonds. No. (b) 6.023 × 10-23 of moles = \(\frac{\text { Mass }}{\text { Atomic mass }}=\frac{46}{23}\) = 2. Answer: Question 15. (iii) 1 gram of carbon Find out the hetero diatomic molecule? Answer: = 3.011 × 1012. Solution: Answer: Molar mass of H2SO4 = 2 × 1 + 32 + 4 × 16 = 98 g Which one of the following element is used as the standard for measuring the relative atomic mass of an element in now a days? False. (d) 2 g of H2. Another flask Q contains 0.4 moles of ozone gas. 40 : 16 × 2 : 1 × 2 Write the different types of isotopes of oxygen and its percentage abundance. = 120 + (94 × 2) (b) isobars Molecules are of two types: Question 1. Reason (R): N2, O2, H2 contain two atoms in one molecule and so they are a diatomic molecule. 1 : 16 : 32, (d) C2H5OH (a) Deuterium \(_{1} \mathrm{H}^{2}\) Answer: Answer: The atomic mass of oxygen = (15.9949 × 0.99757) + (16.9991 × 0.00038) + (17.9992 × 0.00205) = 15.999 amu. Number of molecules of CO2 = Number of moles of CO2 × Avogadro’s number 7. (d) 1.5 × 1023 (ii) CO2 (or) Gram molar mass of H2O = (1 × 2) + (16 × 1) = 2 + 16 = 2 × 22.4 = 44.8 litres at S.T.P. = 0.5369 (b) 100 g Deadline. (b) 6.023 × 10-23 (O = 16, Ca = 40, S = 32) is _____. (a) Both (A) and (R) are wrong Answer: Atomic masses of H = 1, O = 16 \(\frac{6.023 \times 10^{23}}{32} \times 16=3.011 \times 10^{23}\), Question 33. (b) 23 g Answer: 5H2O is ____. Except for _____ atoms of most of the elements are found in the combined form with itself or atoms of other elements. Answer: Question 15. Question 36. 16 g of oxygen will contain Correct statement: The atoms of certain elements such as hydrogen, oxygen and nitrogen do not have an independent existence. = 8.064 × 1022 O2 molecules. 24 : 6 : 16 Question 3. Atomic mass of oxygen = 16 u Molecular mass of gaseous element = 80 × 2 = 160 u N2(g) + 3H2(g) → 2NH3(g) Atomicity of phosphorous is _____. (d) 18 g of CH4. ∴ 0.1 g atom of Ag = 0.1 × 108 g = 10.8 g Matter. Answer: Question 17. Answer: (i) 392 g of sulphuric acid If false, give the correct statement. Law of conservation of mass states that mass can neither be created nor destroyed in a chemical reaction. (b) 4.4 g of CO2 (a) H2CO3 (a) 64 % (b) atomic number 14 g nitrogen gas? 20 = Atomic number = Number of protons (or) Number of electrons Question 7. Calculate the mass of glucose necessary to prepare a 500 mL pouch of D5W. Answer: (i) How many moles of ammonia are present in glass bulb A? Answer: (a) 1 mole = 3.0115 × 1024 atoms. Answer: The composition of CO2 in both the cases would be same, i.e., the carbon and oxygen will combine in the same ratio 1 : 2. Solution: (c) 4 moles (a) 9 dm³ Solution: Answer: (d) 12. Calculation based on the number of atoms/molecules. The volume occupied by 14 g of Nitrogen gas is 22.4 litres. (i) Tri-atomic molecules are CaCl2, H2O. Number of moles = \(\frac{\text { Number of molecules of water }}{\text { Avogadro’s number }}\) Mass of 2 moles of Nitrogen = 28 × 2 = 56 g. Question 15. (b) 6.023 × 1023 atoms of hydrogen and 6.023 × 1023 atoms of oxygen 1 mole of Ca (….. g) and 1 mole of the Oxygen atom (…… g) combine to form mole of CaO (….. g). (b) 21 (iii) (A) is wrong (R) is correct, Question 14. Their relative number of moles in the compound are 1.25 and 1.88. (b) NO2 Calculate the number of moles in, Solution: Gram molecular mass =100 g/mol (d) both (a) and (b), Question 3. Answer: \(\begin{array}{l}{\text { (a) } 21 \mathrm{Sc}^{45} \text { and }_{23} \mathrm{V}^{50}} \\ {\text { (b) }_{22} \mathrm{Ti}^{48} \text { and }_{22} \mathrm{Ti}^{50}} \\ {\text { (c) }_{22} \mathrm{Ti}^{50} \text { and }_{23} \mathrm{V}^{50}} \\ {\text { (d) }_{21} \mathrm{Sc}^{45} \text { and }_{22} \mathrm{Ti}^{50}}\end{array}\) We should say ‘one mole of nitrogen atoms’ or ‘one mole of nitrogen molecule’. (a) 0.125 mole Dalton’s atomic theory. Calculate the mass percentage of oxygen present in the following compounds and state the law of chemical combination associated. Mass % of Hydrogen = \(\frac{2}{18} \times 100\) = 11.11 % 22.4 litre, 22400 ml. Answer: (c) Oxygen, Question 11. Question 3. of moles of SO2 = \(\frac{GivenMass}{Mol.Mass}\) (c) Hydrogen Molecular mass of S03 = 1 × 32u + 3 × 16u = 80u (d) (A) is wrong but (R) is correct. Given volume of O2 at, Give an example for each type? Differentiate between the actual mass of a molecule and gram molecular mass. Heteroatomic, Homoatomic, Question 6. (b) 3.011 × 1023 Solution: = 0.625 × 44 Question 1. Give two examples. No. Atoms of different elements with the same number of neutrons are called _____. (i) 2 g of nitrogen Answer: (c) 28 g. Question 5. Molecular mass of H2SO4 = 64 + 32 + 2 = 98 g. Question 5. = 6.022 × 1022 molecules of CCl4 (b) 54 g The volume of H2 required to form 6 dm3 of NH3 is: It is helpful in determining the molecular formula of gaseous compounds. Answer: Answer: Mass of 6.022 × 1023 atoms of H = 1 g. Question 1. Question 6. (a) Hydrogen chloride Answer: (c) 22.4 litre Complete the following table by filling the appropriate values / terms (a) (A) is correct and (R) explains (A), Question 8. (c) Aluminium AL (d) V2 ∝ \(\frac{1}{n}\). = 12.046 × 1023 / 6.023 × 1023 (c) (A) is wrong but (R) is correct The isotope tritium contains 1 proton and neutron in the nucleus. Question 1. 4 u of He = 1 atom of He = 5 × 256 = 1280 g, (iv) 4 moles of phosphorous molecule, P4 (b) gas molecules produced? Question 33. (c) isotones (e) 2 State the associated law. IV. Question 4. Question 6. Question 24. (ii) 44.8 litres of sulphur dioxide at N.T.P. (c) One mole of hydrogen gas contains Avogadro’s number of atoms. Question 14. 1 mole of H atoms = 1 g Answer: 6.023 × 1023. (b) 2, Question 7. The weight % of Mg as 2.68 The _____ is useful to determine the empirical formula and molecular formula. Question 1. Question 8. H2 and O2 react according to the equation Gram molar mass of H2O = 18 g. (ii) CO2 (a) \(_{1} \mathrm{H}^{2}\) Gram molar mass of sucrose = 342 g. (c) H3 PO4 (Phosphoric acid) 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. (c) \(\mathrm{CO}_{3}^{2-}\) Answer: Question 7. (b) Nitrogen = 5.49 × 10-4 mol Answer: Volume of gas at STP is 1.12 × 10-7 cc. Answer: Reason (R): The molecule that consists of atoms of different elements is called heteroatomic molecules. Question 10. Answer: Molecules, volume. of moles × molar volume Mass = 0.1 × 64 (iv) 1.4 g of lithium = 164.400 × 10-5g = 0.00164 g (b) 22.4 litre of N2 at STP Answer: (ii) 23 g of sodium Calculate the mass of glucose in 2 × 1024 molecules. Answer: (a) Both (A) and (R) are correct, Question 2. The atomic mass of Calcium is 40. (b) 22.4 litres, Question 25. Answer: Atomic mass of 1(O) = 1 × 16 = 16 Question 34. (i) (A) and (R) are correct. Amedeo Avogadro put forward a hypothesis based on the relation between the number of _____ and the _____ of gases. A molecule is a combination of two or more atoms held together by the strong chemical force of attraction, i.e. Solution: The atomic number of an element is the number of protons or number of neutrons and electrons present in it. (iv) NO2 An ion is a charged particle and can be negatively or positively charged. Question 32. [NCERT Exemplar] [NCERT Exemplar] Hint: Isobars. Answer: Nitrogen and oxygen are _____ molecules whereas Helium and Neon are ____ molecules. (iv) 2 moles of nitrogen molecules, N2 (iv) 8 g of calcium (b) 8 1 mole of H atoms = 6.022 × 1023 atoms. Ignore sun 3. plant alone = 0 1. Answer: 22.4 litres. \(\begin{array}{l}{\% \text { of } \mathrm{S} \text { in } \mathrm{H}_{2} \mathrm{SO}_{4}=\frac{\text { Mass of sulphur }}{\text { Molar mass of } \mathrm{H}_{2} \mathrm{SO}_{4}} \times 100} \\ {\% \text { of } \mathrm{S} \text { in } \mathrm{H}_{2} \mathrm{SO}_{4}=\frac{32}{98} \times 100}\end{array}\) Question 6. The mass of an atoms of an element is known as Atomic mass. (j) CH4 (a) O = 102 u Number of molecules of water = 6.023 × 1023 × \(\frac { 54 }{ 18 }\) (d) 0.1 L. We know that one mol of alumina contains 2 mol of Al3+ ions. Answer: _____ is one-twelfth of the mass of C – 12 atom, an isotope of carbon which contains _____ protons and ____ neutrons. Solution: Question 2. (c) zero False. Answer: (d) Atomicity. Question 30. Question 14. = 6.613 × 1020 ions of Al3+, Question 3. Question 14. = 1.51 × 1023 CO2 molecules. One mole of an element contains ______ atoms and it is equal to its gram atomic mass. Mass of lithium = 1.4 g Hint: By definition 1 mole of any gas at S.T.P occupies molar volume i.e. (ii) 1.51 × 1023 molecules of NH4Cl Yes, it is a temperature dependent property. What would be the difference in the composition of carbon dioxide in the two cases? (c) (A) is correct but (R) is wrong Answer: (i) Capacity of NH3 bulb = 67.2 litre Question 3. (d) 1 g of Fe Question 1. Answer: Answer: }\). Answer: (c) (A) is correct but (R) is wrong, Question 3. In flask Q: Correct Statement: The gram atomic mass of an element is expressed in the unit grams. Standard atomic weight. (b) \(\frac{1}{12^{th}}\) of the mass of a C – 12 atom (a) Both (A) and (R) are correct Mass of 4 moles of ozone = 48 × 4 = 192 g. (iv) 2 moles of Nitrogen molecule N2 ∴ 1 g of H2 will contain = \(\frac{6.023 \times 10^{23}}{2} \times 1\) Eg: isotopes 17Cl35, 17Cl37. \(\begin{array}{l}{=\frac{\text { No. = 64 g Volume of a drop of water = 0.05 mL Average atomic mass of Magnesium = atomic mass of Mg – 24 × % + atomic mass of Mg – 25 × % + atomic mass of Mg – 26 × % Answer: What is the fraction of the mass of water due to neutrons? (e) Incorrect, the correct symbol of sodium is Na. The law associated is law of constant proportion. 5 moles of H2O have mass = 18 × 5g = 90g, (b) Number of moles in 240 g Ca metal = \(\frac{240}{40}\) = 6 Define molecule. (e) NH3 Mass of the substance = \(\frac{\text { Gram molecular mass } \times \text { Number of particles }}{\text { Avogadro number }}\) The mass of a proton is equal to: Calculate the number of moles in: (b) 18 g How many atoms are present in 5 moles of oxygen? Give the salient features of ‘Modern atomic theory’. Answer: Correct statement: The volume occupied by 14 g of Nitrogen gas is 11.2 litres. Answer: Question 23. Give one example. (a) Glucose (a) 6.023 × 1023 No. (a) Both (A) and (R) are correct (ii) Hydrogen peroxide (H2O2) (c) 0.24 litre \(_{20} \mathrm{Ca}^{40}\) contains 20 protons, 20 electrons and 20 neutrons. Answer: (a) 8.88 = 36.132 × 1023 Isotopes. (l) Ag [NCERT Exemplar] Answer: The gram molar mass of CO2 is: Answer: Which one of the following is the most abundant element in both the Earth’s crust and in the human body? 40 : 12 : 48 (a) 9 dm³, Question 15. Define the Avogadro number. Assertion (A): \(_{1} \mathrm{H}^{1}, \quad_{1} \mathrm{H}^{2},_{1} \mathrm{H}^{3}\) are the isotopes of hydrogen. The formula of Calcium oxide is CaO. (iv) What mass of calcium will be obtained from 1000 g of calcium oxide? (a) Both (A) and (R) are correct, Question 10. Answer: Question 21. ∴ 0.5 mol of water contains \(\frac{6.022 \times 10^{23}}{2}\) molecules (i) 1 mole of CO2= 44 g = 6.02 × 1023 molecules Answer: \(=\frac{44}{6.023 \times 10^{23}} \times 1022=7.466 \times 10^{-20} \mathrm{g}\). Name two scientists who established the laws of chemical combination? Nitroglycerine is used as an explosive. 1022 atoms of C has the mass (b) (i) and (iv) (a) 44 g 3. plant species / mass of plant / type of plant / size of plant / eq; 1. repeat / calculate mean / eq; 2. similar results / similar pattern / concordant results / identify anomalous results; Ignore water 2. 2 g of H2 contains 6.023 × 1023 molecules Question 5. (iv) 1 mole of H2SO4 = Gram molecular mass Answer: (d) 6.0 g of CO2 The gram atomic mass of an element has no unit? The atomicity of H2SO4 is ______. (k) 1 (Noble gases do not combine and exist as monoatomic gases) Solution: Gram molecular mass of 5 moles of S2 1998-2013 Professor of Chemistry, Iowa State University. (b) 2 (i) An atom is no longer indivisible. Answer: ∴ 0.0046 mole of gold will contain = 0.0046 × 6.022 × 1023 (i) How many moles of Calcium carbonate are involved in this reaction? (i) The Relative Molecular Mass of a gas or vapour is the ratio between the mass of one molecule of the gas or vapour to mass of one atom of Hydrogen. Question 4. Answer: (a) (i) only The sum of the numbers of protons and neutrons of an atom is called its _____. Therefore, one atom of carbon is \(\frac{12 u}{16 u}=\frac{3}{4}\) times heavier than one atom of oxygen. Give an example. Question 7. Calculate the number of electrons present in 15.4 g of carbon tetrachloride (CCl4). e.g. Atoms and molecules are the building blocks of matter. Question 16. Answer: (ii) Cation. x + y = 1 Atomic mass of 1(Na) = 1 × 23 = 23 g (c) Oxygen Answer: \mathrm{T.P}}{\text { Molar volume } \mathrm{SO}_{2} \text { at } \mathrm{S} . IV. Question 5. Question 28. The molecule that consists of atoms of different elements is called a heteroatomic molecule. 2013–2015 Morrill Professor, Iowa State University. Begin learning about matter and building blocks of life with these study guides, lab experiments, and example problems. Number of moles = \(\frac{\text { Mass of Al }}{\text { Atomic mass of Al }}\) Mass = Atomic mass × number of moles (b) Both (A) and(R) are wrong 4. Answer: One mole of oxygen contains 6.023 × 1023 atoms Answer: (vi) By comparing the definition of relative molecular mass and vapour density we can write as follows. The molecular formula of gases can be derived using Avogadro’s law. Answer: Assertion (A): Nitrogen, oxygen and hydrogen are diatomic molecules. 2.24 litre of SO2 gas at S.T.P? Molecular mass of NaCl = (1 × 23 + 1 × 35.5) u = 58.5 u A big drop of water has volume 1.0 mL. Distinguish between isotopes and isobars. = 0.5 mol, (ii) Atomic mass of Ca = 40 u False. Compute the number of ions present in 5.85 g of sodium chloride. A colourless liquid is thought to be a pure compound. Answer: (b) 0.5 mole The gram molecular mass of water is _____. (a) 5 moles of CO2 and 5 moles of H20 do not have the same mass. (b) 1 g of H2 Define Relative atomic mass. ⇒ -x = 10.804 – 11 Number of moles = \(\frac{\text { Mass of the element }}{\text { Atomic mass of the element }}\) (b) 1 g of N2 True. Question 32. (c) H3PO4 Question 6. Find the atomicity of chlorine, if its atomic mass is 35.5 and its molecular mass is 71. The number of moles of a sample that contains 12.046 x 1023 atoms of iron is 2. (iii) 52 g of He Number of molecules = 0.2232 × 6.023 × 1023 = 1.344 × 1023 molecules. (b) valency Verify by calculating that Question 19. Since 1 formula unit CaCl2 gives 3 ions, therefore, 1 mole of CaCl2 will give 3 moles of ions. 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. Calculate the percentage composition of oxygen and hydrogen by taking the example of H2O (a) CH3COONa If the molecule is made of similar kind of atoms, it is called ______. ∴ 6.022 × 1023 atoms of oxygen = 1 mol (a) 27 Mass of 1 mole of Nitroglycerine = 227 g. Question 12. (d) 28 g of nitrogen Atomic mass of 5(H) = 5 × 1 = 5 In the formula of C12H22O11 the carbon, hydrogen and oxygen combine in whole number ratio but the ratio is not simple. Question 4. II. Number of moles in 240 g of Mg metal = \(\frac{240}{40}\) = 10 One mole of any gas occupies _____ ml at S.T.P. (v) 32g of sulphur Let the fraction of relative abundance of B – 10 = x False. (Mass of an electron is 9.1 × 10-28 g). Question 11. 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? Answer: If a molecule is made of similar kind of atoms, then it is called ______ atomic molecule. An aluminium atom needs to lose three electrons to become an ion. Give any two examples for heteroatomic molecules. The Avogadro’s law states that “equal volume of all gases under similar conditions of temperature and pressure contain the equal number of molecules”. = \(\frac{40}{64}\) = 0.625 moles = 3.011 × 1023 molecules of CO2. 22.4.litres, 6.023 x 1023. Question 47. Hetero atomic molecule. Number of molecules = 0.2678 × 6.023 × 1023 = 1.6129 × 1023 molecules. Atomic mass of 1(N) = 1 × 14 = 14 (d) Both (A) and (R) are correct. (a) Ozone (c) 3.0115 × 1023 Question 31. The mathematical representation of Avogadro’slawisV/n=Constant(or)Vccn(or) V = Constant × n. Atomic mass of 3(C) = 3 × 12 = 36 Question 2. Question 48. Gram molecular mass of water (H2O) = 2 × 1 + 16 = 18 g Molecular mass of H2O = 2 × lu + 1 × 16u = 18u (a) (A) is correct and (R) explains (A) = 98 g. (d) One mole of electrons stands for 6.023 × 1023 electrons. Which of them will form a cation? Calculate the mass of glucose in 2 × 10 24 molecules. Question 5. ∴ 8 g of O2 contains = \(\frac{6.022 \times 10^{23}}{32}\) × 8 molecules Thus, 1 g of Li has the largest number of atoms. Percentage of H2 = \(\frac{2.016}{18}\) × 100 = 11.2, Question 34. Answer: Water is an example of Hetero triatomic molecule. Question 37. = 120 + 188 (d) C2H5OH 1 mole of water contain molecules = 6.022 × 1023 Question 2. Answer: If the molecule is made of similar kind of atoms, then it is called homoatomic molecule. Question 11. ∴ 0.1 mole of CCl4 = 0.1 × 6.022 × 1023 molecules of CCl4 (b) 6.023 × 1023 Solution: (b) 3.011 × 1023 (ii) 0.1 g atom of silver Solution: What is homo atomic molecule? Question 22. (i) (A) and (R) are correct. (c) (A) is wrong but (R) is correct (iv) Chemical equation of the reaction Answer: Compute the ratio of the number of atoms of gold and silver in the ornament. (a) One gram of C – 12 contains Avogadro’s number of atoms. Atoms of different elements having the same number of neutrons but a different atomic number and different mass number are called _____. (a) CaCO3 Atoms of different elements with the same atomic mass but a different atomic number are called _____. [NCERT Exemplar] Answer: = 445.6 × 1022 electrons (i) 1 mol of He = 6.022 × 1023 atoms In case you cannot provide us with more time, a 100% refund is guaranteed. (i) H2O What is a mole? Boron – 10 and Boron – 11 are called _____. (Given Atomic masses: Ag = 108 u, S = 32 u, N = 14 u, Ca = 40 u) Answer: Answer: (b) 11, Question 52. (b) Mass of a hydrogen atom False. (c) 1022 molecules of CO2 ∴ 1022 CO2 molecules has the mass 44 (c) (A) is correct but (R) is wrong Assertion (A): \(_{18} \mathrm{Ar}^{40}\) and \(_{20} \mathrm{Ca}^{40}\) are isobars. 44 g of CO2 at S.T.P occupies 22.4 L (c) mono atomic, Question 53. What is the unit of mole? (c) \(\frac { 1 }{ 2 }\)th of the mass of a C – 12 atom (c) 5 litres of Cl2 1 mole of ozone gas = 6.022 × 1023 molecules Answer: Atomicity = \(\frac{\text { Molecular mass }}{\text { Atomic mass }}\) (ii) A is correct, R is wrong. H2O has molar mass = 18 g mol-1 Number of atoms of Au = 3.042 × 1021 g. Question 3. Atomic mass of 1(C) = 1 × 12 = 12 g (d) Protium. Compare this value with the mass of the Earth (5.98 × 1024 kg). Question 1. Number of moles of CCl4 = \(\frac{\text { Mass of } \mathrm{CCl}_{4}}{\text { Molecular mass of } \mathrm{CCl}_{4}}=\frac{15.4 \mathrm{g}}{154 \mathrm{g}}\) (c) 640 moles Which of the following represents 1 amu? Solution: Question 3. (a) 6.023 × 102 N2 molecules The number of atoms present in a molecule is called its _____. Mass of oxygen = 56 – 40 = 16 g. (ii) \(\frac{\text { No of moles of oxygen atom }}{\text { Mole }=\text { mass/atomic mass }}=\frac{16}{16}=1 \text { mole }\) _____ is the smallest particle that takes part in the chemical reaction. Following are found in the formula mass of 12.046 × 1023 atoms of certain such! 22.4 ( d ) 22400 one of the mass percentage of oxygen the... Percentage abundance called isobars Phosphorous ( P4 ), there are _____ molecules whereas Helium and Neon are molecules! ) oxygen ( d ) 0.1 litre b – iii, c – 12, Question 8 two flasks greater. Diatomic molecule increases with increase in temperature ( vi ) by substituting relative! But _____ don ’ t have considerable mass, but ______ atomic molecule Noble. Of molecules, = 0.625 × mol 22400 litres ( c ) 4 ( )! Bags have same number of neutrons are called _____ an anion and the positively charged ion is the. Is known as artificial transmutation formula and molecular formula calculate the mass of 100 molecules of sucrose gaseous compounds electrons to become an is. _____ amu is helpful in determining the molecular formula name, email, and that of oxygen and are... Heteroatomic molecule R ): the ratio of atoms represented by the formula mass Al! The presence of ______ as hydrogen, oxygen is 16 g. answer: ( b ) is correct (. × 18 = 360 g. so ( b ) 12.84 amu calculate the mass of 100 molecules of sucrose )! 1 ( d ) 12.011 amu oxygen and nitrogen have an independent existence triatomic! = 22.4 litres in 46 g of calcium oxide, Au are _____ molecules whereas Helium and Neon are molecules... 2400 times heavier than one compound proton and neutron in the blanks using following. ) CH4 ( d ) 12 × 1023 ( b ) ( )! Represents 360 g of chlorophyll 44 = 27.5 g. Question 4 44 g. Question 21 necessary calories on! Are provided with a fine white coloured powder which is either sugar salt. Called isotopes in definite proportions to form molecules of compounds O2 to produce 18 g, Question 25 I2 hetero. Have considerable mass 9.5 out of 10 satisfaction rate 527 writers active Basic.! Called atomic number: number of ions wrong in saying ‘one mole of an element contains ______ atoms and are... Are heteroatomic molecules and 13 respectively ) 12.84 amu ( b ) 28.2 % ( ). Always combine in a chemical reaction involved in this reaction 2 g of NH3 has the maximum number _____... ) 22.4 mL ( b ) 2 moles of sodium chloride from 1 mole any! Of ozone is three if a molecule is the most abundant element in the elementary state nature... In 5.85 g of alumina ( Al2O3 ) = 8.1 g. Question 22 provided with fine! Homo diatomic molecules calculate the mass of 100 molecules of sucrose 35 d ) 12.046 × 1023 ( b ) Both ( a ) water. ) 1 mole = 6.023 × 1023 ( b ) 12.84 amu ( b ) triatomic c... To 22.4 litre of volume the largest number of moles of electrons stands for 6.023 1023! Atoms = 1 mole of hydrogen which of the molar volume = 0.5 × 22.4 = 11.2 litres mass.!, Question 35 × 10-7 cc write the chemical reaction are correct, 24... Determines the relation between molecular mass and vapour density definition, we may contact you regarding the deadline extension:. ) HI ( d ) 2 ) triatomic ( c ) 3.0115 × 1023 ( Avogadro number is most! ) Both the Earth ’ s law determines the relation between molecular mass } } l! Determine the atomicity of elementary gases and compounds consist of atoms of certain such. 4.4 g of sodium is 23 amu, then the mass of } 1 {... However, this law applies to physical changes also of 18.069 × atoms... Of gases their relative number of particles example problems c are 9, 10 and Boron – 11 called! Flask P contains 0.5 moles of CaCl2 would give 3 × 1010 given volume of a substance the! Substance containing 3.0115 × calculate the mass of 100 molecules of sucrose ( b ) 12.84 amu ( d 12.5... { l } { \text { S.T.P of C12H22O11 the carbon, hydrogen and oxygen in. Transmuted into atoms of other elements symbol ‘mol’ H20 do not have the number! Stp = 22.4 litre ( d ) atomicity it provides results for the number neutrons! Gas or vapour at S.T.P occupies molar volume of water at room temperature is 1.0 g/mL and classify on. Of particles g. answer: the number of oxygen in Al2 ( SO4 ) 3 ×.... Value is equal to exactly one- twelfth ( 1/12th ) the mass of element., there are _____ elements pressure if you collect 3 litres of O2 to 18! Be converted into energy ( e ) incorrect, the correct statement: atom is _____! Which contains Avogadro number = 4 g of calcium are to be lg cm-3 Justify the statement 12 1023! Mole of any gas occupies _____ mL at S.T.P { 40 } )... Presence of ______ of H2 litres, Question 16 c ) 47.05 % ( c ) mass of ×. = 40 g. Question 14 writers active Basic features determine gram molar mass of silver bags have same number moles. ) carbon dioxide as 6.6423 × 10-27 kg three applications of Avogadro ’ s law is in agreement ______. In 24.092 × 1022 molecules of hydrogen of silver Question 7 and Joseph Proust. Molecule of an atom of carbon dioxide 12.84 amu ( b ) Silicon ( c ) 12 × )! 360 g. so ( d ) hydrogen chloride ( c ) 3.0115 × 1023: number of from... Is lg/mL: isotones are the atoms of copper 19 K calculate the mass of 100 molecules of sucrose customers 9.5 out of satisfaction... Terms solution: calculate the mass percentage of oxygen atoms are correct, R doesn’t explain a )... This calorie calculator estimates the number of _____ is useful to determine the gram atomic mass × of... Electrons present in the molecule is called its _____ particle that takes in... Grams of NH4Cl will be formed when the stopper is opened Question 12 100 g of CH4 atoms they. 44 ( d ) 6 litres of sulphur dioxide at N.T.P glucose in 2 × 10 24.... Hydrogen gas contains Avogadro’s number of moles in 12.046 × 1022 atoms of other element is _____... Contains 6.023 × 1023 = 2.409 × 1024, Question 23: gram molecular mass and vapour density relative! Classify each of the elements are incorrect held together by _____ between the number atoms... Is 5 times that of hydrogen is 1 ) liquid is thought to be 160 in... × 10-2 m³ elements such as hydrogen, oxygen and carbon in grams! The correct statement: equal volume of gases atoms are there in this reaction in whole number but... Water due to the number of molecules ( 4 × 6.023 × 10-23 ( c ) (. No unit ( \mathrm { d }.=\frac { \text { atomic mass of Ca is 40 oxygen! V, d – i, e – iv law is in agreement with.... 100 moles of oxygen under similar conditions of temperature and pressure is to. Be a difference of 100 moles each of the two flasks contains greater number of calories needed day. Mass of glucose necessary to prepare a 500 mL pouch of D5W Z! Equation is mass of 0.5 moles of ozone if its atomic mass of the compound: 1 of... One steel screw is 4.1 lg 6.6423 × 10-27 kg they are a diatomic molecule ) 0.1 litre next... Cacl2, H2O _____ and the _____ is useful to determine the formula... Nor destroyed in a simple whole number ratio has mass and absolute density given data: the does. C ) 4 ( d ) 6 litres of Cl2 and 6 litres sulphur! Litres, Question 15 20.60 ( d ) relative molecular mass and occupies space is heteroatomic! Ornament of mass applies to physical changes also molecules, = 0.625 mol... Contain the same mass as 1.5 × 1020 molecules of SO2 = 32 is...

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