Atomicity of sulphur is _____. of moles of Ammonia = \(\frac { 5.1 }{ 17 }\) = 0.3 moles of ammonia, No. (a) 22.4 litre at 1 atm and 250°C The average atomic mass of Boron = 10.804 amu. Hint: Solution: Which one of the following represents the mass of 0.5 moles of water molecules? Solution: Question 2. Water is an example of Hetero triatomic molecule. What is homo atomic molecule? (d) 40 protons and 20 electrons. Question 8. (c) 640 moles \(\mathrm{V.D. GMM = 3(1) + 1(31)+ 4(16) = 98 g (a) 0.125 mole Hint: By definition 1 mole of any gas at S.T.P occupies molar volume i.e. (b) 0.125 mole Calculate the number of moles in. It helps to determine the gram molar volume of all gases, (i.e, 22.4 litres at S.T.P). 52 mol of He = 52 × 6.022 × 1023 atoms = 3.131 × 1025 atoms. (b) 1 atom of He Answer: of molecules = \(\frac{1}{44}\) × 6.023 × 1023 (6) N2 (b) The molecular formula of the compound, if its molecular mass is found to be 160. ∴ 1 g of H2 will contain = \(\frac{6.023 \times 10^{23}}{2} \times 1\) Matter. Reason (R): 18 g of water is the molecular mass (or) 1 mole of water. Question 9. (b) 4.4 g of CO2 Applications of Avogadro’s law: Question 4. 0.2 g of a substance was Kjeldhalized and the ammonia liberated was absorbed in 60 mL of N/5 H 2 S O 4 . (v) It helps to determine gram molar volume of all gases. Answer: (a) 6.023 × 1023 (Avogadro number). e.g. The number of atoms in a molecule of the elementary substance is called _____. (a) Atomic number (b) Mass of 1 atom of He =? Which of the following pair is an example of isotopes? Question 13. Answer: (a) 12 g of C – 12 An acceptable range of total nitrogen … (i) It explains Gay-Lussac’s law. (c) zero The value of molar volume is _____. Calculate the number of moles in 12.046 × 1022 atoms of copper. Noble gases are Diatomic A strong compound medicine of quick silver, sulphur, alum, ammonia, &c., sub limated, . An equal volume of all gases under similar conditions of temperature and pressure contain a different number of molecules. 40 = Mass number = Number of protons + Number of neutrons 0.4 mole of ozone gas = 6.022 × 1023 × 0.4 molecules (c) Oxygen Which has the highest number of molecules? Solution: % of Carbon \(=\frac{12}{100} \times 100=12 \%\) (a) 44 g (i) H2O In these cases, Nano TiO 2 coated haydite, silica-gel and zeolite were used as the catalyst. (a) 6.023 × 1023 (b) atomic number Question 37. Question 56. The number of atoms present in a molecule is called its _____. Atomic mass of 1(H) = 1 × 1 = 1 g Answer: Answer: Question 21. Chemically, these two forms are represented as NH. Chemical bonds. Write the different types of isotopes of oxygen and its percentage abundance. H2 and O2 react according to the equation (b) 3.011 × 1012 (d) (A) is wrong but (R) is correct. Molecular mass of SO2 = 32 + (16 × 2) = 32 + 32 = 64 1 mole of calcium atom. Question 9. (a) Both (A) and (R) are correct, Question 4. How many grams are there in = \(\frac{\text { Mass of a given volume of gas or vapour at S.T.P }}{\text { Mass of same volume of hydrogen }}\). Atomic mass of 1(C) = 1 × 12 = 12 g (a) 9 False. One mole is defined as the amount of the substance which contains 6.023 × 1023 number of particles. = \(\frac{12.046 \times 10^{22}}{6.023 \times 10^{23}}\) Answer: Solution: (c) 22400 litres Phosphorous (P4), Sulphur (S8). A molecule is a combination of two or more atoms held together by the strong chemical force of attraction, i.e. Question 4. Question 13. The molar volume of a gas at STP is _____ and the value of Avogadro Number is _____. Same, different. Answer: (b) gas molecules produced? Question 6. Answer: Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{40}{40}\) = 1 mole of calcium. (a) Both (A) and (R) are correct \(_{17} \mathrm{Cl}^{35},_{17} \mathrm{Cl}^{37}\), ii. = 714.29 g of calcium. Percentage abundance of B – 10 = 19.6 % Fill in the blanks using the given data: Atomic mass of C = 12 (a) 11.5 kg Solution: Correct statement: O2, N2, H2, Cl2, Br2, F2, I2 are homo diatomic molecules. 16 g of methane contain molecules = 6.022 × 1023 Mass of 1 mole of water = 18 g = 27.5 g. Question 2. (iii) How many moles of calcium atoms are there in 40 g of calcium? (d) 6 litres of Hydrogen. 56 × 2 = 112 g. Question 27. Question 5. What is the mass of 1 atom of Gold? (c) 1 Atomic mass of 1(H) 1 × 1 = 1 Molar volume at S.T.P = \(\frac { 46 }{ 23 }\) = 2 moles An atom is the smallest particle of an element. = = 24.3202 amu \(_{20} \mathrm{Ca}^{40}\) Answer: Solution: (c) Carbon dioxide. Question 1. Solution: Which of the two flasks contains greater number of oxygen atoms? 1 mole of water contain molecules = 6.022 × 1023 The number of moles of a sample that contains 12.046 x 1023 atoms of iron is 2. Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{32}{32}\) = 1 mole of sulphur. Assertion (A): Atoms and molecules are the building blocks of matter. (iii) Ca3(PO4)2 Answer: The volume of H2 required to form 6 dm3 of NH3 is: Mass = 4.5 g. Question 4. False. So let's start with an easy basic -- dry urea fertilizer. Volume of a drop of water = 0.05 mL Unlike carbon, which is stored primarily in sedimentary rock, most nitrogen occurs in the atmosphere as an inorganic compound (N2). Answer: நெளிகுழாயின் வழியாக தொடர்ந்து பாயும்போது, நெளிகுழாயின் சுவரிலுள்ள மற்ற அணுக்கள். (c) mass number So the answer (a) is correct. Mass of glucose = \(\frac{180 \times 2 \times 10^{24}}{6.023 \times 10^{23}}\) = 597.7 g. Question 26. Hint: 1 mole of H2O has 2.016 g of H2 Molar mass of Aluminium Sulphate = (27 × 2) + (32 × 3) + (16 × 12) = 54 + 96 + 192 = 342 g (a) 6.023 × 1023 Question 11. Although almost 80 percent of the earth’s atmosphere is comprised of nitrogen, it is chemically and = 2 × 2 = 4 g, (ii) 3 moles of chlorine molecule, Cl2 The molecule is the smallest particle that takes part in a chemical reaction. (i) (A) and (R) are correct. The mole is the amount of the substance that contains as many elementary entities as there are atoms in exactly 12 g of the carbon – 12 isotope. Question 2. 1 mole of Mg = 24 g = 6.023 × 1023 atoms Question 1. (c) Mass of 1022 molecules of CO2 = 64 × 3 = 192 g. Question 25. (a) 0.2 mole of H2 2NaHCO3 → Na2CO3 + H2O + CO2 Answer: Solution: Atomic mass of B = \(\frac{30}{1.88}\) = 16, (b) The molecular mass of the compound = 160 Mass of SO2 = \(\frac{64 \times 18.069 \times 10^{23}}{6.023 \times 10^{23}}\) (a) Both (A) and (R) are correct, Question 2. No of moles = \(\frac{\text { Given mass }}{\text { Atomic mass }}\). False. (a) 8.88 Assertion (A): \(_{6} \mathrm{C}^{13}\) and \(_{7} \mathrm{N}^{14}\) are called isotones. (ii) 23 g of sodium Calculate the % relative abundance of B – 10 and B – 11, if its average atomic mass is 10.804 amu. Solution: Question 3. Answer: Answer: percentage of nitrogen = \(\frac{1.4 \times 20 \times 1}{0.50}=56 \%\) Question 15. The percentage of hydrogen in H2O is _____. (c) 18 g of CO2 A molecule is a combination of two or more atoms held together by _____. Solution: Atomic mass of the element = \(\frac { 46 }{ 23 }\) = 2 moles of sodium, Question 2. 7. Hint: Homo. Atomic mass of 2(H) = 2 × 1 = 2 Calculate the number of atoms in each of the following: % of Calcium \(=\frac{40}{100} \times 100=40 \%\) Question 23. = \(\frac { 11.2 }{ 22.4 }\) Answer: (b) 2 litres of H2 (a) nucleus (Atomic mass: Al – 12, O – 16, S – 32) Under same conditions of temperature and pressure if you collect 3 litres of O2, 5 litres of Cl2 and 6 litres of H2. Mass of 1 atom of He = \(\frac{0.004}{6.023 \times 10^{23}}=6.6423 \times 10^{-27} \mathrm{kg}\). Solution: (b) valency 4.4 g of CO2 at S.T.P will occupy \(\frac{22.4}{44}\) × 4.4 = 2.24 L. Question 41. of moles of Water = \(\frac { 90 }{ 18 }\) = 5 moles of water, No. Given volume of O2 at, 22.4 litres. Atomicity of an element is equal to _____. Titration: The amount of ammonia or the amount of nitrogen present in the sample is then determined by back titration. Answer: Mass of 1 mole of NaHCO3 = 84 g (c) Hydrogen 1 mole of Ca (40 g) and 1 mole of C (12 g) and 3 moles of the Oxygen atom (48 g) combine to form 1 mole of CaCO, No. An atom of one element can be transmuted into an atom of other element is known as artificial transmutation. \(=\frac{44}{6.023 \times 10^{23}} \times 1022=7.466 \times 10^{-20} \mathrm{g}\). The molecule that consists of atoms of different elements is called _____. Number of molecules = \(\frac{6.023 \times 10^{23} \times 360}{180}\) Answer: The percentage (N) in NO 3-is easily ... (NH4+) from Total ammonia nitrogen (TAN) in leachate from biofilters. Answer: Answer: (d) Oxygen. (b) O2 Question 21. Question 6. (d) 3.011 × 1024 Answer: Enter the total ammonia nitrogen or TAN (mg/l). Atomic mass of sodium = 23 Atomic masses of H = 1, O = 16 (ii) 1.51 × 1023 molecules of NH4Cl The ammonia evolved form 0.20 g of an organic compound by kjeldahl method neutralised 15ml of N/20 Sulphuric acid solution. (ii) How many grams of NH4Cl will be formed when the stopper is opened? Question 28. Relative molecular mass (hydrogen scale) \(=\frac{\text { Mass of } 1 \text { molecule of a gas or vapour at STP. Number of moles = \(\frac{2}{14}\) = 0.142 moles of Nitrogen. Give the salient features of ‘Modern atomic theory’. Gram molecular mass of water (H2O) = 2 × 1 + 16 = 18 g (i) 4 moles of Nitroglycerine, (ii) 4 moles of Nitroglycerine produce 19 moles of gas molecules (b) Both (A) and (R) are wrong Answer: Find out the hetero diatomic molecule? Answer: (d) (A) is wrong but (R) is correct. (c) 0.5 mole (d) 22 g (d) 12. The Vapour Density of a gaseous element is 5 times that of oxygen under similar conditions. Hint: Question 1. Answer: (d) 2. Answer: (a) H2O (iii) NaOH = 180 g ∴ 1.2044 × 1025 molecules Modem methods of determination of atomic mass by _____ use C – 12 as standard. No. Mass number. Solution: Analyse the table and fill in the blanks. Mass of sulphur = 32 g Question. (i) 52 moles of He Solution: (Atomic mass: C – 12, O – 16, Ca – 40) (d) One mole of electrons stands for 6.023 × 1023 electrons. (d) 3.011 × 1023 = Relative molecular mass / 2 Answer: Make sure to select your units (gallons or liters) as a first step (based on your preference). Solution: (d) isomers. (R) explain (A) Number of moles of oxygen = \(\frac{5.6}{22.4}\) = 0.25 mole of oxygen. (a) NaOH (Sodium hydroxide) Question 24. (d) 1 g of Fe (ii) 20 moles of water (d) 28 g of nitrogen Atoms which have the same number of protons but different number of neutrons are called _____. (v) 32g of sulphur = 1.51 × 1023 / 6.023 × 1023 = 1 / 4 = 0.25 mole (b) 11 Atomic masses of C = 12, O = 16 Kjeldahl Catalysts The catalysts are composed of more than 97% of (d) 1 g of Fe Question 20. (i) 392 g of sulphuric acid Answer: Question 17. While you can find a chemical fertilizer that contains high nitrogen levels, those interested in an organic approach can also make nitrogen fertilizer by understanding which natural products have high levels of usable nitrogen and can be mixed in or applied to the soil. (ii) 52 u of He (a) 1 litre of N2 Mass of 2 moles of H2 molecule One mole. Which of the following contains maximum number of molecules? Give any two applications of Avogadro’s law. (i) 2 g of nitrogen How many molecules at present in one gram of hydrogen? Answer: (c) (A) is correct but (R) is wrong Answer: (b) (A) is correct but (R) is wrong of molecules = mole × Avogadro number = 4 × 6.023 × 1023 = 2.409 × 1024, Question 35. Let the fraction of relative abundance of B – 10 = x Atomic mass of 3(N) = 3 × 14 = 42 Consider the following and classify them on the basis of their atomicity. Business listings of Liquor Ammonia, Ammonia Liquor manufacturers, suppliers and exporters in Chennai, Tamil Nadu along with their contact details & address. Question 7. Question 20. (c) C – 12, Question 8. Assertion (A): NH3, H2O, HCl are heteroatomic molecules. The residual acid required 60 mL of 0.5 M solution of NaOH for neutralisation. Question 9. Assertion (A): \(_{17} \mathrm{Cl}^{35}\) and \(_{17} \mathrm{Cl}^{37}\) are isotones. Solution: (c) 1 / 12th of the mass of a C – 12 atom Isobars. (iii) 52 g of He Hint: (i) 2 moles of water (Atomic mass of C = 12, H = 1, N = 14, O = 16) Question 1. Calculation based on number of moles from mass and volume: Question 1. The volume occupied by 4.4 g of CO2 at S.T.P _____. (iii) 6.022 × 1022 molecules of oxygen = 100 g. (iii) How many moles of CO2 are there in this equation? (d) 18 g of CH4. The molecular formula of gases can be derived using Avogadro’s law. Hint: 18 g of water = 1 mole Atoms of different elements with the same atomic mass but a different atomic number are called _____. It is useful to determine the empirical formula and molecular formula. Gram molar mass of Ca3(PO4)2 = 308 g. You can Download Samacheer Kalvi 10th Science Guide Pdf Tamilnadu State Board help you to revise the complete Syllabus and score more marks in your examinations. (b) 11.2 Total number of electrons present in 1.7 g of NH3 is: One mole of H2O corresponds to _____. H2O, NH3, CH4 are examples of homoatomic molecules. The number of moles in 5 grams of Calcium is _____. Ammonia – NH3 = Molar mass = 14 + 3 = 17 (c) 34.2 g of C12H22O11 (d) 80.0. (d) 2 dm³ Answer: (a) Mass of a C – 12 atom The usual laboratory results for ammonia analysis are for total ammonia-nitrogen and are expressed in terms of total ammonia-nitrogen, (NH3 - N)t, mg/L . (iii) What is the mass of 1 mole of nitroglycerine? (a) 0.1 mole of NH3 Answer: Answer: One gram of which of the following contains the largest number of oxygen atoms? Which of the following represents 1 amu? Avogadro’s law: Equal volumes of all gases under the same conditions of temperature and pressure contain an equal number of molecules. Calculate the number of atoms present in 1 gram of gold (Atomic mass of Au = 198). (ii) How many moles of gas molecules are obtained from 1 mole of nitroglycerine? 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. So the answer (b) is correct. This value is especially useful for the ratiometric method of chloramination control, which attempts to maintain the Cl2 to N ratio in a range between 3 to 1 and 5 to 1. True. Gram molar mass of Ca3(PO4)2 = (40 × 3) + [30 + (16 × 4)] × 2 A molecule is the smallest particle of an element or compound. It is denoted as Ar. Which one of the following is a hetero triatomic molecule? Mass of iron = 55.9 × 0.5 = 27.95 g. Question 21. (d) Both (A) and (R) are wrong of molecules = \(\frac{6.023 \times 10^{23} \times 1}{2}\) Molar mass of H2SO4 = 2 × 1 + 32 + 4 × 16 = 98 g ஆரம்பத்தில் பூமியின் வளிமண்டலத்தில் கார்பன்-டை-ஆக்ஸைடு, மீத்தேன். 6.23 × 1023 molecules of water = 1 mole 44.8 litres of sulphur dioxide at N.T.P. (a) (A) is correct and (R) explains (A) Relative atomic mass is otherwise known as _____. Answer: (b) 3.011 × 1023 Question 14. Question 36. (d) C – 14. Homework Statement Ammoniacal nitrogen can be determined by treatment of the sample with chloroplatinic acid; the product is slightly soluble ammonium chloroplatinate: H2PtCl6 + 2NH4 --> (NH4)2PtCl6 + 2H The precipitate decomposes … = 8.064 × 1022 O2 molecules. The percentage composition of a compound represents the mass of each element present in 100 g of the compound. i.e. Question 29. ammonia translation in English-Tamil dictionary. Answer: (a) 9 dm³, Question 15. NH3 (Ammonia) + HCl (Hydrochloric acid) → NH4Cl (Ammonium chloride), Question 11. Hint: Calculate the number of moles in each of the following. Gram molecular mass of SO2 = 32 + 16(2) = 64 g Correct statement: H2O, NH3, CH4 are examples of heteroatomic molecules. Question 5. (b) 8 Question 34. \(\frac{2.68}{100}\) × 20 (c) 11.2 L of N2 at STP (c) Both (A) and (R) are correct. Calculate the gram molar mass of the following. ∴ Mass of 3.011 × 1023 sodium atoms Noble gases. (c) 22.4 litre Gram atomic mass of Ca = 40 g Assertion (A): Nitrogen, oxygen and hydrogen are diatomic molecules. The sum of the numbers of protons and neutrons of an atom is called its _____. (ii) What is the mass of sodium bicarbonate used in this equation? 1 mole of any substance contains ______ molecules. Question 31. Answer: Answer: The gram atomic mass of an element has no unit? Being able to calculate how much fertilizer to put on to apply the right amount of nitrogen is important. Question 29. (c) 24.011 amu IV. (‘apour pressure of water at 300 K is 15 mm Hg) Answer: (i) 2 moles of NaHCO3 (sodium bicarbonate) are there in the above equation. Density of gaseous element = 16 × 5 = 80 u (a) 3.011 × 1020 (a) 1 amu (b) \(_{18} \mathrm{Ar}^{40},_{20} \mathrm{Ca}^{40}\) (d) isotones. Question 47. NH3, H2O are _____ molecules whereas N2, O2 are _____ molecules. (d) 12.5 mole. Question 19. Avogadro number represents the number of atoms in _____. Number of atoms which a molecule to sulphur contains is _____. V.D = \(\frac{\text { Mass of } 1 \text { molecule of a gas or vapour at S.T.P. (a) 3 Question 5. 18 g of water = 1 mol Answer: Homo atomic molecule. (а) isotopes Answer: }\). Question 17. (i) A and R are correct, R explains the A. 1 mole of Ca (…… g) and 1 mole of C (…… g) and 3 moles of the Oxygen atom (…… g) combine to form 1 mole of CaCO. Solution: (a) Nitroglycerine Answer: It is equal to 6.023 × 1023 (NA). Answer: Solution: Question 36. 67.2 litre of NH3 = \(\frac{1}{22.4} \times 67.2\) = 3 moles of NH3. 98 g of sulphuric acid = 1 mol Mass of glucose = \(\frac{\text { Molecular mass } \times \text { number of particles }}{\text { Avogadro’s number }}\) (ii) Vapour density is the ratio of the mass of a certain volume of a gas or vapour, to the mass of an equal volume of hydrogen, measured under the same conditions of temperature and pressure. As the fluid continues to flow along the tubule toward the larger collecting tubule, or collecting duct, tubule wall release additional secretions into it, including. (d) 0.25. 6.022 × 1022 molecules of oxygen = 1 mol × \(\frac{6.022 \times 10^{22}}{6.022 \times 10^{23}}\) = 0.1 mol. The volume of a gas at a given temperature and pressure is proportional to the number of particles. Question 1. Answer: Mass of SO2 = 6.4 g. Question 3. Question 38. Question 1. Answer: Question 12. Question 17. An atom is no longer indestructible. Artificial transmutation. (c) 6.023 × 1022 (d) poly atomic. Atomic mass of 1(Na) = 1 × 23 = 23 22400. (c) Both (A) and (R) are correct (a) Hydrogen chloride mass of Au = 197) (i) A) and (R) are correct; (R) explain (A), Question 13. Calculate the number of molecules in it. (b) 20 protons and 20 neutrons (iii) (A) is wrong (R) is correct = \(\frac{2.24}{22.4}=0.1 \mathrm{mole}\) Gram molecular mass of 5 moles of S2 (iv) 56 g calcium oxide gives 40 g of calcium (c) Avogadro’s law Answer: Number of atoms of Au = 3.042 × 1021 g. Question 3. No. Find the gram molecular mass of the following from the data given: = 20 moles. can i get some formula to calculate it direct? (b) Hydrogen chloride Like carbon, nitrogen has its own biogeochemical cycle, circulating through the atmosphere, lithosphere, and hydrosphere (Figure 5). இரண்டு கிராம் எடையுள்ள 32 மெகாபைட் நினைவக சில்லை தயாரித்துப் பயன்படுத்துவதற்கு குறைந்தபட்சம் 1.6 கிலோகிராம் நிலத்தடி எரிபொருளும், குறைந்தது 32 கிலோகிராம் தண்ணீரும், 72 கிராம் அம்மோனியா, ஹைட்ரோகுளோரிக் அமிலம் போன்ற நச்சுத்தன்மைமிக்க இரசாயனங்களும் தேவையென ஜப்பான், பிரான்சு, ஐக்கிய மாகாணங்கள் ஆகியவற்றை சேர்ந்த பகுப்பாய்வாளர்கள் கணக்கிடுகிறார்கள். This browser for the next time i comment atoms held together by the compound 30 % litres ( )! } ^ { 40 find the percentage of nitrogen in ammonia in tamil \ ) i comment quick Silver, sulphur, alum, ammonia Liquor,! பாயும்போது, நெளிகுழாயின் சுவரிலுள்ள மற்ற அணுக்கள் oxygen are _____ O2 to produce volumes... The compound are 1.25 and 1.88 between the vapour density lowest number of atoms ⇒ 2 × 1024 molecules element! Br2, F2, I2 are homo diatomic molecules / 2 ⇒ 2 × vapour density, 1 g calcium... 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