Question 57. Gram molecular mass of CO2 = 44 g Question 5. Correct statement: O2, N2, H2, Cl2, Br2, F2, I2 are homo diatomic molecules. (R) explain (A). (OR) True. H2O has molar mass = 18 g mol-1 Answer: Define Vapour density. (d) 11.5 g. = 1 × 40u + 1 × 12u + 3 × 16u = 100u Correct statement: The atoms of certain elements such as hydrogen, oxygen and nitrogen do not have an independent existence. Carbon C – 12. (b) Both (A) and (R) are wrong Question 40. Question 32. Hint. of moles of NaOH = \(\frac { 2 }{ 40 }\) = 0.05 moles of NaOH, 1 g Au = \(\frac{1}{197}\) mol = \(\frac{1}{197}\) × 6.02 × 10, 1 g Na = \(\frac{1}{23}\) mol = \(\frac{1}{23}\) × 6.02 × 10, 1 g Li = \(\frac{1}{7}\) mol = \(\frac{1}{7}\) × 6.02 × 10. Answer: Answer: (c) 22.4 litre (v) 1023 atoms of calcium. = 5 × 256 = 1280 g, (iv) 4 moles of phosphorous molecule, P4 22400. (v) Atoms may not always combine in a simple whole number ratio. True. (b) 2.24 L (d) 44.8 litre. 22.4 litres. Answer: Answer: False. (i) H2O (d) 6 litres of Hydrogen. (b) 100 g (a) Mass of sodium atoms carried by Krish = (5 × 23) g = 115 g (ii) 23 g of sodium Question 32. (c) 1 The gram molecular mass of oxygen molecule is: Atomic mass of 3(C) = 3 × 12 = 36 False. False. A mole is the amount of a substance which contains the same number of chemical units (atoms, molecules or ions) as there are atoms in exactly 12 g of carbon-12. of moles = \(\frac{\text { Mass }}{\text { Atomic mass }}\) (or) \(\frac{\text { Mass }}{\text { Molecular mass }}\) ⇒ Total moles of ions = 0.1 × 2 = 0.2 moles The stable isotope of _____ is used as the standard for measuring the relative atomic mass of an element. Reason: An atom of aluminium is 27 times heavier than 1 / 12th of the mass of the C – 12 atoms. If the atomic mass of sodium is 23 amu, then the mass of 3.011 × 1023 sodium atoms is _____. = \(\frac{1 \mathrm{mol}}{(22.4 \mathrm{L})} \times(44.8 \mathrm{L})\) = 2.0 mol. (i) Ion (iii) 40 g of calcium Answer: The average atomic mass of an element is calculated by adding the masses of its isotopes, each multiplied by their natural abundance on the Earth. Answer: Hint: 18 g of water = 1 mole Answer: (a) Atomic mass of A = \(\frac{70}{1.25}\) = 56 (h) O3 Solution: of molecules = \(\frac{1}{28}\) × 6.023 × 1023 Answer: (c) \(\frac { 1 }{ 2 }\)th of the mass of a C – 12 atom The Avogadro’s law states that “equal volume of all gases under similar conditions of temperature and pressure contain the equal number of molecules”. Let the fraction of relative abundance of B – 11 = y (c) C – 12, Question 8. (d) (A) is wrong but (R) is correct. (i) (A) and (R) are correct. (b) Glucose The percentage composition of elements is useful to determine _____ and _____. For example, water, ammonia, carbon dioxide. (a) 27 Calculate the number of moles present in: (g) P4O10 Calculate the mass of CO2 which contains the same number of molecules as are contained in 40 g of SO2. The statement does not clarify whether we are talking about atoms or molecules of nitrogen. Oxygen. The volume occupied by 1 mole of a diatomic gas at S.T.P is _____. The volume occupied by 1 mole. Answer: (d) Both (A) and (R) are wrong (b) atomic number Solution: So (b) is the smallest mass as 6.6423 × 10-27 kg. (b) 20 protons and 20 neutrons Law of conservation of mass states that mass can neither be created nor destroyed in a chemical reaction. Compare this value with the mass of the Earth (5.98 × 1024 kg). (ii) How many moles of oxygen atoms are there in this? = 0.5 mole. Answer: Question 39. (ii) Tetra-atomic molecules are NH3, PCl3. (v) 1 mole of Ca = 40 g = 6.02 × 1023 atoms of Ca = 40 + 12 + 3(16) = 714.29 g of calcium. Except for _____ atoms of most of the elements are found in the combined form with itself or atoms of other elements. Question 21. Which of the following has the smallest mass? Question 2. Answer: Calculate the formula mass of sodium carbonate (Na2CO3.10H2O). (d) 6.0 g of CO2 Answer: Atoms which have the same number of protons but different number of neutrons are called _____. (d) 18 g of CH4. Correct statement: The number of atoms present in the molecule is called its Atomicity. (a) Both (A) and (R) are wrong] It is used to determine the atomicity of gases. The gram molecular mass of water is _____. 44.8 litres of sulphur dioxide at N.T.P. Answer: Mass = Atomic mass × number of moles (a) 0.2 mole of H2 For 100 moles each of sodium atoms and ions there would be a difference of 100 moles of electrons. The difference in the mass of 100 moles each of sodium atoms and sodium ions is 5.48002 g. Compute the mass of an electron. y = % abundance of B – 11 = 100 – 19.6 = 80.4 % (c) 2 g of He 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. Question 6. 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