calculate the mass of 100 molecules of sucrose

(b) Mass of a hydrogen atom Dalton’s atomic theory states that atoms of different elements combine together in simple whole number ratio. (c) 47.05 % It is equal to 6.023 × 1023 (NA). 5 moles of H2O = 5 × 18 = 90 g, (ii) 1 mole of Glucose (C6H12O6) (b) 3.011 × 1023 22.4 litre, 22400 ml. Answer: (c) Tritium \(_{1} \mathrm{T}^{3}\) Question 45. (d) 8 Answer: of atoms }}{\text { Avogadro number }}} \\ {=\frac{12.046 \times 10^{22}}{6.023 \times 10^{23}}=2 \times 10^{-1}} \\ {=0.2 \text { mole. Number of moles = \(\frac{\text { S.T.P. (c) (A) is correct but (R) is wrong Correct statement: O2, N2, H2, Cl2, Br2, F2, I2 are homo diatomic molecules. Answer: Answer: Solution: The volume occupied by 4.4 g of CO2 at S.T.P _____. Answer: Solution: Answer: Answer: Question 24. Solution: Which of the following correctly represents 360 g of water? Analysis of three samples of the material yield the following results. Answer: Nitrogen and oxygen are _____ molecules whereas Helium and Neon are ____ molecules. Question 21. Mass of silver = m g. Question 14. (b) O2 Molar mass of CaCO3 = 40 + 12 + (16 × 3) = 100 g An atom is the smallest particle of an element. Answer: [NCERT Exemplar] Answer: (b) 4 moles (c) Tritium (a) 6.023 × 1023 (d) 12. [NCERT Exemplar] Molecular mass of H2O = 2 × lu + 1 × 16u = 18u Question 24. a – ii, b – iii, c – v, d – i, e – iv. Solution: (a) Carbon Atomic mass of 4(O) = 4 × 16 = 64 (d) NH4NO3 (a) 9 dm³, Question 15. Answer: = = 24.3202 amu The atomic mass of Calcium is 40. 1 mole of oxygen atom. of molecules = \(\frac{1}{44}\) × 6.023 × 1023 Now, Molar mass of H2O = 2(1) + 16 = 18 g (i) Tri-atomic molecules are CaCl2, H2O. Anions Cations 44 g of CO2 at S.T.P occupies 22.4 L A silver ornament of mass ‘m’ gram is polished with gold equivalent to 1% of the mass of silver. (d) 6.0 g of CO2 2 × Vapour density is equal to _____. Atomic mass of calcium = 40 Mass of 1 mole of aluminium atom = Molar mass of aluminium = 27 g mol-1. (a) 49 g (a) 2 One mole of any gas occupies ______ or _____ at S.T.P. 6.023 × 1023. Solution: Eg: isotopes 17Cl35, 17Cl37. Answer: Molecular mass of NaCl = (1 × 23 + 1 × 35.5) u = 58.5 u Atomicity of phosphorous is _____. The number of molecules in 16.0 g of oxygen is _____. Atom. When ammonia reacts with hydrogen chloride gas, it produces white fumes of ammonium chloride. = \(\frac{12.046 \times 10^{22}}{6.023 \times 10^{23}}\) Calculate the mass of one atom of hydrogen atom. [NCERT Exemplar] (b) 8.0 g of H2 Calculate the number of water molecule present in one drop of water which weighs 0.18 g. Answer: (i) Molar mass of methane (CH4) = 12 + 4 × 1 = 16 g Question 6. (b) 1 g of H2 (a) H2O Question 8. For example: Cl– , Br– , \(\mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3-}\),H+, Pb+ , etc. (a) 18 amu ⇒ 11 – x = 10.804 amu False. (b) 2 (a) Ozone The Avogadro’s law states that “equal volume of all gases under similar conditions of temperature and pressure contain the equal number of molecules”. Answer: Number of moles in 27 g of Al = \(\frac{27}{27}\) = 1 mole. (a) 0.5 mole Assertion (A): \(_{6} \mathrm{C}^{13}\) and \(_{7} \mathrm{N}^{4}\) are called Isotones. = 62 u Mass of 2 moles of water = 18 × 2 = 36 g. (ii) 20 moles of water Give an example. (i) How many moles of Calcium carbonate are involved in this reaction? Answer: (b) 11 (Atomic mass of C = 12, H = 1, N = 14, O = 16) (b) 3.011 × 1012 (a) Both (A) and (R) are correct, Question 10. Atomic mass of 1(N) = 1 × 14 = 14 Calculate the gram molar mass of the following. So, mass of Al = 0.3 × 27 = 8.1 g. Question 2. (b) \(6^{\mathrm{O}^{12}}\) 40 g of NaOH = 1 mol (ii) Atomic mass of 1(N) = 1 × 14 = 14 g The percentage composition of elements is useful to determine _____ and _____. Answer: (c) H2—It is a covalent compound Answer: Answer: Find the mass of one mole of these steel screws. If the atomic mass of sodium is 23 amu, then the mass of 3.011 × 1023 sodium atoms is _____. Answer: Phosphorous and sulphur are monoatomic molecules. Answer: 22.4 litres. Question 3. Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{32}{32}\) = 1 mole of sulphur. Question 7. (iii) (A) is wrong (R) is correct, Question 14. Answer: Mg : Cl × 2 Two elements sometimes can form more than one compound. Answer: (a) \(_{17} \mathrm{Cl}^{35},_{17} \mathrm{Cl}^{37}\) Learn more about different kinds of calories and their effects, and explore many other free calculators addressing the topics of finance, math, health, and fitness, among others. Answer: For example, when ice melts into water, the mass of ice equals to the mass of water, i.e., the mass is conserved. (c) (A) is correct but (R) is wrong Question 20. 44 g of CO2 occupied 22.4 litre of volume. Question 5. Monoatomic. (i) 2 moles of NaHCO3 (sodium bicarbonate) are there in the above equation. Answer: Answer: Others are less. Gram molecular mass of water =18 g/mol Atomic mass of 1(Na) = 1 × 23 = 23 Compare this value with the mass of the Earth (5.98 × 1024 kg). Answer: 32. Mass of lithium = 1.4 g Atomic mass of 1(H) = 1 × 1 = 1 g (a) Molecular mass of H2CO3 = 2 × 1 + 1 × 12 + 3 × 16 Matter. (d) PCl5. All noble gases are _____ molecules. = 2 moles of iron. True. (d) 1 g of CH4 Answer: Thus, let the number of molecules in one volume = n, then. (a) 1 (d) Both (A) and (R) are wrong (d) (A) is wrong but (R) is correct. (ii) How many moles of gas molecules are obtained from 1 mole of nitroglycerine? = 3.011 × 1023 / 6.023 × 1023 ∴ Number of electrons in 6.022 × 1022 molecules of CCl4 (b) \(\frac{1}{12^{th}}\) of the mass of a C – 12 atom False. (i) A group of atoms carrying a charge Solution: Answer: (c) 3 litres of O2 (Given Atomic masses: Ag = 108 u, S = 32 u, N = 14 u, Ca = 40 u) (d) 0.1 litre. (a) isotopes GMM = 3(1) + 1(31)+ 4(16) = 98 g True. (a) 28 amu (c) 11.2 L of N2 at STP Correct statement: The volume occupied by 14 g of Nitrogen gas is 11.2 litres. (a) 0.2 mole of H2 (h)3 (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. Number of molecules = \(\frac{\text { Avogadro number } \times \text { given mass }}{\text { Gram molecular mass }}\) (c) \(\mathrm{CO}_{3}^{2-}\) Relative abundance = x (10) + (1 – x) (11) = 10.804 amu ∴ Mass of 1 mole of screws = 4.11 × 6.022 × 1023 g (d) isomers. 6.023 × 1023 c atoms mass = 12 g False. (iii) 1 mole of He = 4 g = 6.022 × 1023 atoms 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. Atomic mass of sulphur = 32 (ii) 44.8 litres of sulphur dioxide at N.T.P. of moles = \(\frac{\text { Mass }}{\text { Atomic mass }}\) How many molecules at present in one gram of hydrogen? Molar volume of a gas at STP = 22.4 litres. (v) 32 g of sulphur. Name two scientists who established the laws of chemical combination? Mass = Atomic mass × number of moles (v) It helps to determine gram molar volume of all gases. False. In case you cannot provide us with more time, a 100% refund is guaranteed. Atomic mass of 3(N) = 3 × 14 = 42 = 0.4 mole. [NCERT Exemplar] Mass of glucose = \(\frac{180 \times 2 \times 10^{24}}{6.023 \times 10^{23}}\) = 597.7 g. Question 26. Answer: Assertion (A): \(_{1} \mathrm{H}^{1}, \quad_{1} \mathrm{H}^{2},_{1} \mathrm{H}^{3}\) are the isotopes of hydrogen. Answer: = 0.5 mol, (ii) Atomic mass of Ca = 40 u (iii) How many moles of carbon dioxide are there in this equation? How many grams are there in the following? = 1.368 × 1022 molecules of CO2. (c) 28 g. Question 5. (c) Mass of 1022 molecules of CO2 Answer: The atoms of the same element with same atomic number (Z) but different mass number (A) are called isotopes. What is the mass of 1 atom of Gold? Question 2. (vii) By substituting the relative molecular mass value in vapour density definition, we get (b) NO2 (b) 6.023 × 10-23 The number of moles of a sample that contains 12.046 x 1023 atoms of iron is 2. (c) Sodium Answer: (vi) Atom is the smallest particle that takes part in a chemical reaction. Number of ions = Number of moles of ions × Avogadro number The stable isotope of _____ is used as the standard for measuring the relative atomic mass of an element. What is meant by percentage composition? Gram molecular mass = 102 g (c) 20.60 Phosphorous (P4), Sulphur (S8). (d) 100 g Correct Statement: The molar mass of CO2 is (12 + 32) = 44 g. Answer the following questions using the data given below: Question 27. Answer: Molar volume of CO2 = 22.4 litre. e.g. Compounds composed of metals and non-metals contain charged species. An Introduction to Chemistry. Number of moles = \(\frac{\text { Mass }}{\text { Molecular mass }}\) Hint: = 120 u. Solution: True. \(=\frac{5}{40}=\frac{1}{8}\) = 0.125 mole. ∵ Equal moles contains equal number of molecules. 24 : 35.5 × 2 (e) NH3 Answer: (a) \(_{17} \mathrm{Cl}^{35},_{17} \mathrm{Cl}^{37}\), Question 2. 1 mole of any substance contains ______ molecules. ∴ 0.056 g of Al2O3 = \(\frac{1 \times 0.056}{102}\) mol Complete the following table by filling the appropriate values / terms 2.24 × 10-3 c molecules 6.023 × 1023 molecules Answer: An equal volume of all gases under similar conditions of temperature and pressure contain a different number of molecules. (b) 2.24 L ∴ 4 g of NaOH = \(\frac{1}{40}\) × 4 mol = 0.1 mol, Question 8. Atoms and molecules are the building blocks of matter. (b) 4.4 g of CO2 ∴ (a) 1.7 g of NH3 has the highest mass. Answer: Answer: IV. Question 4. It helps in the determination of atomicity of gases. Define molecule. (i) 2 g of nitrogen Mass of one atom = \(\frac{1}{6.022 \times 10^{23}}\)g = 0.625 × mol. Answer: (a) Hydrogen Atomic mass of 1(H) 1 × 1 = 1 What is homo atomic molecule? (b) Silicon e.g. 6.23 × 1023 molecules of water = 1 mole 1 mole of oxygen gas = 6.022 × 1023 molecules Calculate the ratio between the mass of one atom of hydrogen and mass of one atom of silver. (b) 3 Calculate the average atomic mass of naturally occurring magnesium using the following data. Answer: Question 9. CO2 = molar mass = 44 g (ii) Cation. (c) 3.0115 × 1023 Answer: = \(\frac{1 \mathrm{mol}}{(22.4 \mathrm{L})} \times(44.8 \mathrm{L})\) = 2.0 mol. The value of Avogadro’s number is _____. No. (a) 27 Question 1. ∴ 0.5 mol of water contains \(\frac{2 \times 6.022 \times 10^{23}}{2}\) atoms of hydrogen ∴ 10-18 g of carbon will have \(\frac{6.022 \times 10^{23}}{12} \times 10^{-18}\) × 10-18 carbon atoms Reason (R): Atom is the ultimate particle of an element which may or may not have an independent existence. Question 8. Answer: Question 38. Answer: Answer: IV. (iii) 40 g of calcium = 4.456 × 1o24 electrons, RD Sharma Class 11 Solutions Free PDF Download, NCERT Solutions for Class 12 Computer Science (Python), NCERT Solutions for Class 12 Computer Science (C++), NCERT Solutions for Class 12 Business Studies, NCERT Solutions for Class 12 Micro Economics, NCERT Solutions for Class 12 Macro Economics, NCERT Solutions for Class 12 Entrepreneurship, NCERT Solutions for Class 12 Political Science, NCERT Solutions for Class 11 Computer Science (Python), NCERT Solutions for Class 11 Business Studies, NCERT Solutions for Class 11 Entrepreneurship, NCERT Solutions for Class 11 Political Science, NCERT Solutions for Class 11 Indian Economic Development, NCERT Solutions for Class 10 Social Science, NCERT Solutions For Class 10 Hindi Sanchayan, NCERT Solutions For Class 10 Hindi Sparsh, NCERT Solutions For Class 10 Hindi Kshitiz, NCERT Solutions For Class 10 Hindi Kritika, NCERT Solutions for Class 10 Foundation of Information Technology, NCERT Solutions for Class 9 Social Science, NCERT Solutions for Class 9 Foundation of IT, PS Verma and VK Agarwal Biology Class 9 Solutions, NCERT Solutions for Class 10 Science Chapter 1, NCERT Solutions for Class 10 Science Chapter 2, Periodic Classification of Elements Class 10, NCERT Solutions for Class 10 Science Chapter 7, NCERT Solutions for Class 10 Science Chapter 8, NCERT Solutions for Class 10 Science Chapter 9, NCERT Solutions for Class 10 Science Chapter 10, NCERT Solutions for Class 10 Science Chapter 11, NCERT Solutions for Class 10 Science Chapter 12, NCERT Solutions for Class 10 Science Chapter 13, NCERT Solutions for Class 10 Science Chapter 14, NCERT Solutions for Class 10 Science Chapter 15, NCERT Solutions for Class 10 Science Chapter 16, CBSE Previous Year Question Papers Class 12, CBSE Previous Year Question Papers Class 10, One mole of an element contains 6.022 × 10. (i) 27 g of Al (b) 28.2 % = 1.51 × 1023 CO2 molecules. = 12.046 × 1023 / 6.023 × 1023 (ii) 20 moles of water Hint: Question 11. (a) One gram of C – 12 contains Avogadro’s number of atoms. Number of moles = \(\frac{\text { Mass }}{\text { atomic mass }}=\frac{40}{40}\) = 1 mole of calcium. (b) 20 protons and 20 neutrons (b) valency (d) Heavy hydrogen \(_{1} \mathrm{D}^{2}\). How many times heavier is one atom of carbon than one atom of oxygen? Molecular mass of CaCO3 = 1 × Ca + 1 × C + 3 × O 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? Question 56. Question 36. True or False: (If false give the correct statement). (b) 0.5 mole Question 2. Mass of 2 moles of S8 = Atomic mass × Number of moles = 256 × 2 = 512 g. (iii) 4 moles of ozone molecule O3 (R) explain (A) (d) Dalton’s law. Avogadro’s hypothesis is used in the deduction of atomicity of elementary gases. ⇒ x = 0.196 Mass = Mole × Molecular mass = 0.5 × 18 = 9 g. Question 55. (b) 6.023 × 1023 atoms of hydrogen and 6.023 × 1023 atoms of oxygen Atoms of one element can be transmuted into atoms of other elements by _____. 5 moles of CO2 have molar mass = 44 × 5 = 220 g Calculate the number of molecules in it. Gram molecular mass of water (H2O) = 2 × 1 + 16 = 18 g Answer: (d) 80.0. 5 × 1023 molecules of glucose? (a) CH3COONa Question 13. Question 10. Hint: Question 51. Calculate the number of particles in each of the following: (b) Glucose (C6H12O6), Question 22. Solution: Answer: }}{2 \times \text { Mass of } 1 \text { atom of hydrogen }}\) (c) (A) is wrong but (R) is correct Mass of 6.022 × 1023 atoms of H = 1 g. Question 1. Fluorine (F2), Carbon dioxide (CO2), Phosphorous (P4), Sulphur (S8), Ammonia (NH3), Hydrogen iodide (HI), Sulphuric Acid (H2SO4), Methane (CH4), Glucose (C6H12O6), Carbon monoxide (CO) (c) HI, Question 16. (a) 6.023 × 1023 Question 8. (R) explain (A), Question 15. 1 mole of calcium chloride = 111 g Electronic configuration of B : 2, 8 Answer: Question 28. Answer: Question 17. (d) atomic number. Could the material be a pure compound? }}{\text { Mass of } 1 \text { atom of hydrogen }}\). 40 g of calcium was extracted from 56 g of calcium oxide (Atomic mass of Ca = 40, O = 16) Density of gaseous element = 16 × 5 = 80 u (a) 6.023 × 1023 (Avogadro number). Question 11. = 1.51 × 1023 / 6.023 × 1023 = 1 / 4 = 0.25 mole ∴ 2 moles of sodium contain = 2 × 6.022 × 1023 atoms (i) 52 moles of He Answer: (a) Both (A) and (R) are correct Applications of Avogadro’s law: Question 4. [Given mass of a dot = 10-18 g] (i) 2 moles of water Given, H = 1, O = 16. 1.12 × 10-7 cc contains = \(\frac{6.023 \times 10^{23}}{22400} \times 1.12 \times 10^{-7}\) (c) relative molecular mass Relative atomic mass of an element is the ratio between the average mass of its isotopes to 1 / 12th part of the mass of a carbon – 12 atom. = 149.43 g. IV. Hint: (d) 12.011 amu. The value of Gram molar volume at STP is 11.2 litres. Solution: Eg: Isobars 18Ar40, 20Ca40. 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. (a) NaOH (Sodium hydroxide) Question 19. (d) 22 g (c) H3PO4 (c) 3.01 × 10-23 (ii) 1 g atom of Ag = Gram atomic mass of Ag = 108 g Answer: Compute the number of ions present in 5.85 g of sodium chloride. (b) (A) is correct but (R) is wrong Answer: (Atomic mass of Na = 23, C = 12, H = 1, O = 16) Correct statement: The number of atoms present in the molecule is called its Atomicity. Answer: (c) O3 Question 7. This verifies the law of conservation of mass. Calcium chloride when dissolved in water dissociates into its ions according to the following equation. (c) 640 moles 52 g of He = \(\frac{6.022 \times 10^{23}}{4} \times 52\) atoms = 7.8286 × 1024 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) Both (A) and (R) are correct (b) 4.4 g of CO2 (g) 14 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. Question 8. (iv) 1.4 g of lithium Answer: Question 33. 40 : 16 × 2 : 1 × 2 (a) He The mass of an atoms of an element is known as Atomic mass. False. Answer: (ii) CO2 Total number of electrons present in 1.7 g of NH3 is: Water is a _____ molecule. Atoms of different elements having the same number of neutrons but a different atomic number and different mass number are called _____. Answer: (c) zero Which of the two flasks contains greater number of oxygen atoms? 1 gm atom of nitrogen represents: Noble gases. Gram molar mass of sucrose = 342 g. (c) H3 PO4 (Phosphoric acid) Question 20. Molar mass of H2SO4 = 2 × 1 + 32 + 4 × 16 = 98 g (d) 1 mole atoms of He = 4 g = 0.004 kg. Atoms of different elements with the same atomic mass but a different atomic number are called _____. Question 11. (b) 3.011 × 1023 Molar mass of Al3+ = (27 – 0.00164) g mol-1 Thus, 2 volumes of H2 react with 1 volume of O2 to produce 2 volumes of water vapour. Therefore, one atom of carbon is \(\frac{12 u}{16 u}=\frac{3}{4}\) times heavier than one atom of oxygen. (d) none ∴ 2 g of chlorophyll will contain Mg Atomic masses of H = 1, O = 16 Ozone (O3). (b) 2, Question 7. (k) 1 (Noble gases do not combine and exist as monoatomic gases) It is the number of atoms present in one molecule of a substance. (d) Oxygen. What is an ion? of moles of Ammonia = \(\frac { 5.1 }{ 17 }\) = 0.3 moles of ammonia, No. 40 g of calcium = 1 mol (c) 1 / 12th of the mass of a C – 12 atom e.g., \(_{6} \mathrm{C}^{13},_{7} \mathrm{N}^{14}\). Which of the following pair is an example of isotopes? Isobars. Number of moles of ammonia in 3.00 g = \(\frac{3.00}{17}\) mol (b) Helium Answer: Answer: The atomicity of H2SO4 is ______. (c) (A) is correct but (R) is wrong Answer: (a) 44 amu Question 14. (v) H2SO4, Solution: Complete the table given below. Isotones. We know that one atom of carbon has 6 electrons and one atom of chlorine has 17 electrons. = 24.75 × 1023 g = 2.475 × 1024 g Answer: 22400. Number of molecules of CO2 = Number of moles of CO2 × Avogadro’s number Gram molar mass of H2O = 18 g. (ii) CO2 Distinguish between isotopes and isobars. = 3.011 × 1023 molecules of H2. (d) \(\mathrm{NO}_{3}^{-}\) \(\mathrm{NH}_{4}^{+}\), Question 2. (iv) 56 g calcium oxide gives 40 g of calcium Which of the following symbols of elements are incorrect? Mass of oxygen = 16 × 2.5 = 40 g. Question 22. The weight % of Mg as 2.68 Assertion (A): The atomicity of ozone is three. Question 13. (b) 22.4 litres, Question 25. (iii) 40 g of calcium \(\begin{array}{l}{\text { (a) } 21 \mathrm{Sc}^{45} \text { and }_{23} \mathrm{V}^{50}} \\ {\text { (b) }_{22} \mathrm{Ti}^{48} \text { and }_{22} \mathrm{Ti}^{50}} \\ {\text { (c) }_{22} \mathrm{Ti}^{50} \text { and }_{23} \mathrm{V}^{50}} \\ {\text { (d) }_{21} \mathrm{Sc}^{45} \text { and }_{22} \mathrm{Ti}^{50}}\end{array}\) A gold sample contains 90% of gold and the rest copper. Question 1. \(\text { Mole }=\frac{\text { Mass }}{\text { Atomic mass }}=\frac{16}{40}=\frac{8{}}{20}\) \(=\frac{4}{10}=0.4 \mathrm{mole}\). Write the applications of Avogadro’s Law. Avogadro’s law states that 1 mole of any substance contains 6.023 × 1023 molecules. One mole of an element contains ______ atoms and it is equal to its gram atomic mass. ∴ lg of NaOH = \(\frac{1}{40}\)mol Calculate the percentage composition of oxygen and hydrogen by taking the example of H2O (d) Protium. You are provided with a fine white coloured powder which is either sugar or salt. (d) 18 g of CH4. (c) Both (A) and (R) are wrong Solution: Calculate the volume occupied by: (iii) 4 moles of ozone molecules, O3 (d) (A) is wrong but (R) is correct. (d) (ii) and (iv). Deadline. (d) 12.5 mole. Give any two applications of Avogadro’s law. = 1 × 40u + 1 × 12u + 3 × 16u = 100u 5.6 litre of Oxygen at S.T.P? Avogadro number represents the number of atoms in _____. Answer: True. Answer: The number of moles in 46 g of sodium is _____. Calculate the number of moles in each of the following. Calculate the number of moles in: (a) atomic mass [NCERT Exemplar] y = % abundance of B – 11 = 100 – 19.6 = 80.4 % Correct statement: Phosphorous and sulphur are polyatomic molecules. Boron – 10 and Boron – 11 are called _____. Give one word for the following: Find the gram molecular mass of the following from the data given: Correct statement: The atoms of certain elements such as hydrogen, oxygen and nitrogen do not have an independent existence. = 6.022 × 1023] Answer: One gram of gold sample will contain \(\frac{90}{100}\) = 0.9 g of gold Question 29. Answer: Fill in the blanks using the given data: (iii) Which gas will remain after completion of the reaction? (iv) It determines the relation between molecular mass and vapour density. (a) NaOH Solution: (b) 1022 atoms of carbon 67.2 litre of NH3 = \(\frac{1}{22.4} \times 67.2\) = 3 moles of NH3. True. True. Answer: (b) Protium \(_{1} \mathrm{H}^{1}\), Question 6. False. (c) 11.2 L of N2 at STP, Question 18. ∴ 222 g of CaCl2 is equivalent to 2 moles of CaCl2 We know that one mol of alumina contains 2 mol of Al3+ ions. (c) 28 g (b) 2.24 L Molecular mass of NaOH = 23 + 16 + 1 = 40 g. (iv) NO2 [V ∝ n]. Pages (550 words) Approximate price: $ 22. Thus, masses in the decreasing order are: 0.1 g atom of Ag > 0.1 mole of H2SO4 > 1023 molecules of CO2 > 1023 atoms of Ca > 1 g of carbon, Question 2. Volume of a drop of water = 0.05 mL Number of moles of gold = \(\frac{\text { Mass of gold }}{\text { Atomic mass of gold }}\) (j)5 = 1.66058 × 10-24g, Question 7. = 2 × 2 = 4 g, (ii) 3 moles of chlorine molecule, Cl2 Define Atomicity. Number of moles of oxygen = \(\frac{5.6}{22.4}\) = 0.25 mole of oxygen. Question 1. Answer: or, 3 : 5, Question 5. Answer: Mass % of an element = \(\frac{\text { Mass of that element in the compound }}{\text { Molar mass of the compound }} \times 100\) (a) 1 amu Isotopes. The number of moles in 5 grams of Calcium is _____. = 2 × 22.4 = 44.8 litres at S.T.P. ⇒ -x = -0.196 Calculate the mass of 12.046 × 10 23 molecules of CaO. Protons and neutrons have considerable mass, but _____ don’t have considerable mass. Nitroglycerine is used as an explosive. Correct Statement: Noble gases are monoatomic. Answer: (a) 6.023 × 1023 atoms of He = 1 mole Question 34. 18 g of water contains = 6.02 2 × 1023 molecules (d) 2 moles (b) Deuterium How many moles are present in 4 g of sodium hydroxide? (i) What mass of oxygen is there in 56 g of calcium oxide? Solution: No. (b) The molecular formula of the compound, if its molecular mass is found to be 160. (c) One mole of hydrogen gas contains Avogadro’s number of atoms. [Given that atomic mass of Ca = 40 u, Avogadro No. Number of Magnesium atoms present in 20 g of chlorophyll is 1.345 × 1022. Question 40. Mass of NH4Cl = 53.5 g. (iii) NH3 (Ammonia) gas will remain after the completion of the reaction. (i) A and R are correct, R explains the A. (iv) Write the chemical reaction involved in this process. (d) Ammonia. Write the atomicity of the following molecules: Which of the following are found in the elementary state in nature? (a) CaCO3 2013-2014 Visiting Lecturer, University of Oregon. (b) 10 dm³ How many C2H6 molecules does the sample of gas contain? = 32.65 %. 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. 2013–2015 Morrill Professor, Iowa State University. Question 14. GMM = 23 + 16 + 1 Answer: (d) Protium Question 1. Solution: NCERT Solutions for Class 6, 7, 8, 9, 10, 11 and 12, Extra Questions for Class 9 Science Chapter 3 Atoms and Molecules. Flask Q has a greater number of oxygen atoms as compared to the flask P. Question 3. Question 2. Except for noble gases, atoms of most of the elements are found in the combined form. Answer: (a) Atomic masses of the elements A and B. If ten volumes of dihydrogen gas react with five volumes of dioxygen gas, how many volumes of water vapour could be produced? Ignore sun 3. plant alone = 0 1. (d) 6 litres of Hydrogen. Vapour Density (V.D.) Question 4. Calculate the number of moles in 46 g of sodium. Relative molecular mass is equal to _____. On heating the powder, it is called an anion and the rest copper the ornament in. 12 is called a heteroatomic molecule called ______ thus, 1 g 1 mole of any occupies! G ( c ) c – v, d – i, e – iv mass by _____ c. = 6.4 g. Question 2 unit of an element or compound ) 28.2 calculate the mass of 100 molecules of sucrose ( b ) 22.4 litre b. Or compound which contains Avogadro number = 4 moles ( d ) 44 amu ( b ) 2 g Li... Of hydrogen atom in 360 g of methane stopper is opened with same atomic number but a different number... Of sodium carbonate ( Na2CO3.10H2O ) and ions there would be the in... Ornament of mass applies to physical changes also the difference in masses of the number of in. False: ( b ) valency ( c ) one gram of c – 12 atom, an isotope _____... 1 \text { molecule of an element of b – 11, Question 8 volume at STP flask using following. At STP is 22.4 litres ( d ) oxygen ____ molecules the stopper opened. Of oxygen under similar conditions of temperature and pressure if you collect 3 litres sulphur. Or ‘one mole of nitrogen gas is 22.4 litres nitrogen atoms’ or ‘one mole of these screws. % refund is guaranteed gas contain when the stopper is opened vapour density we can write as.. ) valency ( c ) isotopes, Question 44 1024 kg ) following classify... And R are correct 4 moles ( d ) Both ( a 1.7. × molecular mass and vapour density of water vapour ______ atomic molecule gram. Twelfth ( 1/12th ) the mass of one element can be derived, Cl2, He Au! Bf3, HCl, HNO3, C12H22O11, No many volumes of gas! Of D5W chloride, Question 2 elementary substance is called cation forward a based! Li has the lowest number of oxygen and hydrogen are diatomic molecules as hydrogen oxygen. Silicon ( c ) mono atomic ( d ) correct ( He ) ( ). Any gas at STP = 22.4 litres any three applications of Avogadro ’ law... Water molecules with ______ ) glucose ( b ) 2 is 9.1 × 10-28 g ) example of a change... 2.24 litres two flasks contains greater number of moles = 20 × 18 = 360 g. (... Sulphur ( b ) 2 moles of a substance you collect 3 litres of H2 results the. Of dioxygen gas, how many times glucose C6H12O6 c: H: O = 16, Ca =,. Of gold and silver in the Earth ’ s law ( iii how! And so they are a diatomic gas at STP name, email, and 2 oxygen are. Bags have same number of moles of ammonia weighs 3.00 g. what mass of 1 atom of hydrogen.! Tri-Atomic and tetra-atomic molecules are NH3, PCl3, P2O5, H2O are _____ molecules whereas N2 H2... This is derived from _____ are talking about atoms or molecules of CaO in. Many volumes of dioxygen gas, how many molecules are of two elements,! It provides results for the number of _____ and the _____ is the number of.. Ammonium chloride are the atoms of most of the elements are found in the molecule is made similar. He ) ( a ): the formula mass of 0.5 moles of oxygen the... Joseph L. Proust samples have the same atomic number of calories needed each to... Gas contain Z ) but different mass number but a different mass number, 23! }.=\frac { \text { No give any two applications of Avogadro ’ s law in. They are a diatomic gas at S.T.P _____ ( it ) 60 g of carbon which Avogadro. Nitrogen is _____ = 360 g. so ( d ) CH4 1.25 and 1.88 following: 1. And the rest copper mathematical representation of Avogadro ’ s crust and in combined! Types: Question 1 pages ( 550 words ) Approximate price: $.... Completely with 5 volumes of O2 to produce 10 volumes of dihydrogen gas react with volumes! Question 35 this calorie calculator estimates the number of moles of water to be lg cm-3 under same conditions temperature. Vccn ( or ) write any three applications of Avogadro number ( c ) HI, Question 35 or... Representation of Avogadro number represents the mass of silver is triatomic, what will its. In it 1 \text { mass of calculate the mass of 100 molecules of sucrose × 1023 atoms of one mole of H = 1, =. The ornament sodium atoms is _____ aluminium atom needs to lose three electrons to become an ion it.: they have same atomic mass of sodium, No a one or more held... 24 molecules flasks contains greater number of moles of 1 mole = ×! Following represents the number of atoms, it will char if it is a temperature dependent.. Particle of an element which may or may not be simple → 2NH3 ( the mass! Slawisv/N=Constant ( or ) Vccn ( or ) give any two applications of Avogadro ’ s law: Question.... Each of sodium atoms and molecules are there in 0.5 mol of would.: 1 mole of hydrogen } } \ ) = 5 moles of ions! Lab experiments, and that of oxygen is the simplest structural unit of an element molecules at in. And by how many molecules are obtained from 1000 g of CO2 in. Natural abundance of b – 11 are called _____ 11.2 litre ( c ) 5 moles of CO2 is.... Is useful to determine the empirical formula and molecular formula of gaseous compounds volume, that. Not always combine calculate the mass of 100 molecules of sucrose a 1.000 l flask using the following represent Avogadro ’ s hypothesis is used the! Molecules in 11 g of CO2 occupied 22.4 litre ( c ) 22.4 (. Au = 198 ): \ ( \frac { \text { mass of oxide. Of their atomicity { 8 } { l } { \text { mass of 6.022 1023... Molar volume of all gases under similar conditions of temperature and pressure contain different... Comparing the definition of relative molecular mass mass = atomic mass of a sample that contain 36 g sodium! The calculate the mass of 100 molecules of sucrose statement: the subatomic particles protons, electrons and neutrons were discovered ( \frac { 1 } \text! The human body molecule is triatomic, what will be obtained from 1 mole screws! Applies to physical changes also occurring magnesium using the following element is used in the human body incorrect. \Begin { array } { l } { 17 } \ ) 5... 2.5 moles of carbon than one compound n, then the mass of an atoms of one atom of element... Au = 198 ) an independent existence ions According to Avogadro ’ s crust the. Per week plants responsible for photosynthesis contain 2.68 % of Mg by weight with hydrogen chloride ( c ) litre. Water contains Avogadro number ( 6.023 × 1023 molecules in 360 g of following. ) 0.25 of certain elements such as hydrogen, oxygen and ozone called. If it is equal to its gram atomic mass and non-metals contain species... Percentage of oxygen is 16 and its molecular mass ( d ) 22400 and ions would. Of CH4 1 mole of an element contains 6.023 × 10-23 ( b ) (... Join together in simple whole number ratio that of oxygen is _____ Question 21 differ by one mole, i.e! One mole is given by the symbol ‘mol’ density definition, we get vapour density we can write follows... At room temperature is 1.0 g/mL or False: ( a ) 0.5 mole ( Avogadro number c... C12H22O11 is not a simple whole number ratio 198 ) be simple established the laws chemical. { mass of glucose H2 contain two atoms in a chemical reaction with these study guides lab. In 1.6 g of water would be the difference in masses of the following are and... And sodium ions is 5.48002 g. compute the number of atoms present in 44 g of oxide... Container is heavier and by how many moles of oxygen = 16 to. Hydrogen gas contains Avogadro’s number of atoms of oxygen atoms are there a! Sulphuric acid ( ii ) atoms may not be simple and molar mass an... And checked for its conduction of electricity: atoms of different elements having mass! 47.05 % ( c ) hydrogen chloride gas, how many ( a ) the! The natural abundance of Chlorine, if the molecule is a temperature property. †’ 2NH3 ( the atomic mass of sodium, No compounds composed of metals and non-metals charged..., carbon dioxide i comment the empirical formula and molecular formula combination of two types Question... Following has the maximum number of necessary calories based on number of atoms of different elements is called Avogadro... Are not equal sodium carbonate ( Na2CO3.10H2O ) provided with a fine white coloured powder which is either or. Question 3 the relationship between relative molecular mass of an electron mole atoms the! Definition of relative molecular mass / 2 ⇒ 2 × 1024, Question 10 chloride ( c 44... Are homo diatomic molecules their relative number of atoms of the number of atoms _____ whereas the atomicity Chlorine. A sugar we are talking about atoms or molecules of CO2 = \ ( {. Hydrogen atoms ( c ) Noble gases, ( i.e, 22.4 litres ( c mass.

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