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Answer: Nitrogen from free ammonia and the chloramines can be summed to provide a total ammonia-nitrogen value. The molecule is the smallest particle that takes part in a chemical reaction. (iv) Chemical equation of the reaction (v) Since hydrogen is diatomic The average atomic mass of hydrogen is _____ amu. Question 1. (d) $$_{33} \mathrm{As}^{77},_{34} \mathrm{Se}^{78}$$. (a) H2O, Question 17. Correct Statement: The gram atomic mass of an element is expressed in the unit grams. _____ is the smallest particle that takes part in the chemical reaction. (c) 47.05 % % relative abundance of B – 10 = ? Question 1. No. So let's start with an easy basic -- dry urea fertilizer. Question 3. Answer: Question 5. Applications of Avogadro’s law: Question 4. It helps to determine the gram molar volume of all gases, (i.e, 22.4 litres at S.T.P). False. Calculate the number of magnesium atoms in 20 g of chlorophyll. Distinguish between isotopes and isobars. (c) 11.2 L of N2 at STP, Question 18. Average atomic mass of Magnesium = atomic mass of Mg – 24 × % + atomic mass of Mg – 25 × % + atomic mass of Mg – 26 × % (v) H2SO4, Solution: Answer: = 12.046 × 1023 molecules. Now, Molar mass of H2O = 2(1) + 16 = 18 g Question 58. (c) 4 moles What are isotopes? (a) Both (A) and (R) are correct, Question 2. (b) Hydrogen chloride, Question 19. (d) 14 g Question 15. CO2 = molar mass = 44 g True or False: (If false give the correct statement). 2 × Vapour density. For additional information please see the AES Master Catalog or call our Tech Support Line at 407-598-1401. 392 g of sulphuric acid = 1 mol × $$\frac{392 g}{(98 g)}$$ = 4 mol. The average atomic mass of Boron = 10.804 amu. In water, most of the ammonia changes to ammonium ions (NH +). Question 5. Number of moles = $$\frac{\text { Number of molecules }}{\text { Avogadro’s number }}=\frac{1.51 \times 10^{23}}{6.023 \times 10^{23}}=0.25 \text { moles. Number of moles of SO2 = \(\frac{\text { Given volume of } \mathrm{SO}_{2} \text { at } \mathrm{S} . Question 23. Which one of the following represents the mass of 0.5 moles of water molecules? Question 32. (d) Mass of O – 16 atom Answer: 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 }$$ True. Answer: (c) (A) is correct but (R) is wrong (c) 640 moles No. Isotopes are the atoms of the same element may not be similar in all respects. Atomic mass of 1(H) 1 × 1 = 1 (c) 3 4. a – ii, b – iii, c – v, d – i, e – iv. (d) (A) is wrong but (R) is correct. Question 2. One mole. (c) O3 (a) 6.023 × 1023 Question 39. Calculate the number of atoms of oxygen and carbon in 5 moles of CO2. Answer: (c) relative molecular mass Question 27. The atoms of the different element with the same mass number (A) but different atomic number (Z) are called isobars. (b) valency Answer: (Atomic mass of C = 12, H = 1, N = 14, O = 16) Answer: Empirical formula, molecular formula. Question 9. Solution: (d) Protium (b) Nitrogen Like carbon, nitrogen has its own biogeochemical cycle, circulating through the atmosphere, lithosphere, and hydrosphere (Figure 5). $$2 \mathrm{NaHCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{Na}_{2} \mathrm{CO}_{3}+\mathrm{H}_{2} \mathrm{O}+\mathrm{CO}_{2} \uparrow$$ Artificial transmutation. (d) Helium. Question 11. Answer: (The atomic mass of nitrogen is 14, and that of hydrogen is 1) 1 mole of nitrogen ( 28 g) + 3 moles of hydrogen ( 6 g) → 2 moles of ammonia ( 34 g) Answer: 1 mole of nitrogen ( 28 g) + 3 moles of hydrogen ( 6 g) → 2 moles of ammonia ( 34 g) 3. Question 24. (a) Mass of a C – 12 atom (R) explain (A), Question 12. 32. Mass % of Nitrogen = $$\frac{14}{17} \times 100$$ = 82.35%. (ii) 2 moles of sulphur molecules, S8 (d) 3.011 × 1024 Save my name, email, and website in this browser for the next time I comment. (c) 1.25 mole False. (c) 4 No. (d) Sodium. The gram molar mass of CO2 is: Assertion: The Relative Molecular Mass of Chlorine is 35.5 a.m.u. The percentage (N) in NO 3-is easily ... (NH4+) from Total ammonia nitrogen (TAN) in leachate from biofilters. (i) 2 g of nitrogen Gram molecular mass of water (H2O) = 2 × 1 + 16 = 18 g Solution: Standard atomic weight. Number of moles = $$\frac{\text { Mass }}{\text { Molecular mass }}$$ Assertion (A): 18 g water contains Avogadro number (6.023 × 1023) of particles. = 714.285 g of calcium Question 14. (b) 100 g (ii) How many grams of NH4Cl will be formed when the stopper is opened? Mass = No. A kind of herb, cool to the touch, but causing blisters afterwards, , Ammonia debilis, also used figuratively to persons. Atoms of the same element with same atomic number but having different mass number are called _____. (d) Hydrogen. Mass of SO2 = $$\frac{64 \times 18.069 \times 10^{23}}{6.023 \times 10^{23}}$$ Answer: (a) 22.4 litre H2 (g) + O2 (g) → 2H2O (g) Calculate the mass of glucose in 2 × 1024 molecules. Hint: 18 g of water = 1 mole (b) Protium $$_{1} \mathrm{H}^{1}$$, Question 6. Answer: Avogadro’s hypothesis is used in the deduction of atomicity of elementary gases. (a) 18 g Question 1. ∴ (a) 1.7 g of NH3 has the highest mass. of molecules = mole × Avogadro number = 4 × 6.023 × 1023 = 2.409 × 1024, Question 35. }}{\text { Molar volume at } \mathrm{S} . Solution: Question 18. Which one of the following element is used as the standard for measuring the relative atomic mass of an element in now a days? Relative atomic mass is otherwise known as _____. The atomic mass of sodium is 23. (iii) (A) is wrong (R) is correct Homework Statement Ammoniacal nitrogen can be determined by treatment of the sample with chloroplatinic acid; the product is slightly soluble ammonium chloroplatinate: H2PtCl6 + 2NH4 --> (NH4)2PtCl6 + 2H The precipitate decomposes … Number of moles = $$\frac{\text { Mass }}{\text { Molecular mass }}$$ Calculate the number of molecules in 360 g of glucose. Hetero atomic molecule. (a) 9 dm³ Volume of a drop of water = 0.05 mL The percentage composition of a compound represents the mass of each element present in 100 g of the compound. Assertion (A): $$_{18} \mathrm{Ar}^{40}$$ and $$_{20} \mathrm{Ca}^{40}$$ are isobars. Heterodiatomic molecules. Answer: Answer: \mathrm{T.P}}\) Answer: (b) 18 g Question 28. Percentage abundance of B – 10 = 19.6 % True. The volume occupied by 14 g of Nitrogen gas is 22.4 litres. The output is in mL and in drops (useful for small quantities of nano aquariums). Assertion (A): $$_{17} \mathrm{Cl}^{35}$$ and $$_{17} \mathrm{Cl}^{37}$$ are isotones. Chemically, these two forms are represented as NH. The ammonia evolved was absorbed in 50 ml of 0.5 M H 2 S O 4 . (a) O (a) 6.023 × 1023 (Avogadro number). (b) 5.6 litre (b) 6.023 × 1023 atoms of hydrogen and 6.023 × 1023 atoms of oxygen Answer: Answer: Solution: (c) Atomic mass Gram molar mass of H2O = 18 g. (ii) CO2 = 20 moles. 5H2O is ____. Number of moles = $$\frac{\text { Mass }}{\text { Atomic mass }}$$ Analyse the table and fill in the blanks. Which of the following pair indicates isotopes? Answer: (c) (A) is wrong but (R) is correct N2 + 3H2 → 2NH3 (The atomic mass of nitrogen is 14, and that of hydrogen is 1). Answer: , பொட்டாசியம், யூரியா, யூரிக் அமிலம், அதிகப்படியான நீர் ஆகியவை உள்ளிட்ட திரவங்களை சுரந்து அத்துடன் வெளிவிடுகிறது. Question 5. e.g., $$_{6} \mathrm{C}^{13},_{7} \mathrm{N}^{14}$$. (d) (ii) and (iv). Although there are differences between different samples, the amount of "crude protein" (CP) can be found by multipling the percent Nitrogen by a factor (usually 6.25). y = 1 –  x (d) 2 g of H2. The atomic mass of oxygen = (15.9949 × 0.99757) + (16.9991 × 0.00038) + (17.9992 × 0.00205) = 15.999 amu. (a) H2O Hint: 1 mole of H2O has 2.016 g of H2 (b) 2.24 L Define Atomicity. (a) 44 g ∵ Equal moles contains equal number of molecules. Mass = Atomic mass × number of moles Atomic mass of chlorine = 35.5 g (b) 22.4 litres (d) 100 g (b) (A) is correct but (R) is wrong (b) isobars Atoms of the same element that have same atomic number but different mass number are called isotopes. Hint: The ammonia … 1 mole of oxygen atom. (b) 11 that in the beginning, Earth had an atmosphere composed of carbon dioxide, methane. Answer: - conversion of ammonia nitrogen into organic nitrogen - wastes: organic and ammonia nitrogen - nitrification and denitrification • Ammonia and organic nitrogen in water bodies is an important parameter of their quality. Solution: (a) 1 litre of N2 Question 10. Question 17. Molecular mass of H2O = 2 + 16 = 18, (ii) CO2 (d) 0.1 L. Mass of 0.1 mole of NH3 = 1.7 g. (b) Mass of 1022 atoms of carbon = 30.115 × 1023 Answer: Hint: Mass of 6.023 × 1023 sodium atoms = 23 amu = 23 g. Gram molecular mass of glucose = 180 g The atomic mass unit, 6, 6. = 0.5 × 22.4 Question 22. (i) Mass of CaO = 56 g 44 g of CO2 occupied 22.4 litre of volume. How is Average atomic mass calculated? Solution: (a) 1 mole Answer: One mole, (ii) Calculate the gram molecular mass of calcium carbonate involved in this reaction. Answer: (a) 6.023 × 1023 Question 47. Atomic mass of C = 12 (c) (A) is correct but (R) is wrong (c) 4.4 g Answer: (i) H2O Volume of CO2 at S.T.P = 22.4 × 2.5 = 56 litres. Isobars are the atoms of the different elements with the same atomic number and different mass numbers. = 40 + 12 + 3(16) (a) Sulphur = 2 × 22.4 = 44.8 litres at S.T.P. Answer: Answer:. Question 8. False. Ammonia easily dissolves in water, and in this form is known as liquid ammonia, aqueous ammonia or ammonia solution. (ii) Mass of sodium bicarbonate in this equation is mass of 2 moles of NaHCO3. 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. ... needed we can calculate the number of mol of nitrogen atoms in the sample and then the % of protein in the milk sample. Atoms. use the molar mass and assume 100 g multiple by 100. (а) isotopes Answer: Write the applications of Avogadro’s Law. (c) 11.2 L of N2 at STP Number of moles = (b) 14 amu Hint: By definition 1 amu is defined as precisely 1 / 12th the mass of an atom of carbon – 12. Atomic mass of the element = $$\frac { 46 }{ 23 }$$ = 2 moles of sodium, Question 2. 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. A molecule is the smallest particle of an element or compound. (c) 1 Atomic mass of 4(O) = 4 × 16 = 64 Atomicity = $$\frac{\text { Molecular mass }}{\text { Atomic mass }}$$ Question 12. Therefore, the fraction of un-ionized ammonia is f = 0.0663. Answer: A district in the northwest of India, . (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. • TKN = ammonia + organic nitrogen • TN = NOx + TKN = NOx + ammonia + SON + PON. Solution: Number of molecules = 0.2678 × 6.023 × 1023 = 1.6129 × 1023 molecules. True. (iii) Molecular formula of the gases can be derived. Molecules, volume. An isotope of hydrogen without neutrons is _____. Question 28. 0.5 mole of oxygen gas = 6.022 × 1023 × 0.5 molecules Mass of 1 mole of He = 4 g (or) 0.004 kg. (b) 2, Question 7. = $$\frac{6.023×10^{23}}{18}$$ × 0.18 5 × 1023 molecules of glucose? (a) 22.4 litre at 1 atm and 250°C x + y = 1 Calculate the number of moles in: (a) Deuterium $$_{1} \mathrm{H}^{2}$$ (a) Hydrogen Number of moles of O2 $$=\frac{\text { Volume at S.T.P }}{\text { Molar volume }}$$ $$=\frac{3}{22.4}$$ = 0.1339 moles HP Training Module File: “ 38 Measurement of Ammonia and Organic Nitrogen.doc” Version March 2000 Page 7 Hint: Question 20. Atomic masses of C = 12, O = 16 Which one of the following is the most abundant element in both the Earth’s crust and in the human body? V.D = $$\frac{\text { Mass of } 1 \text { molecule of a gas or vapour at S.T.P. 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 (d) 6 litres of Hydrogen. The isotope tritium contains 1 proton and neutron in the nucleus. (c) 18 g (b) 4 moles Answer: Molar mass of CaCO3 = 40 + 12 + (16 × 3) = 100 g (c) 24.011 amu (d) 3 × 1010. 22400. (b) V ∝ n It is available in a white crystalline form or as dirty-white granules. Answer: Question 18. Molar mass of H2SO4 = (1 × 2) + (32 × 1) + (16 × 4) Which of the following has the largest number of particles? Mass % of an element = \(\frac{\text { Mass of that element in the compound }}{\text { Molar mass of the compound }} \times 100$$ Question 1. (а) 0.1 mole of NH2 (d) isomers. = 2 × 2 = 4 g, (ii) 3 moles of chlorine molecule, Cl2 ∴ Average atomic mass of Magnesium is 24.3202 amu. (a) 11.2 litre The Relative molecular mass of a molecule is the ratio between the mass of one molecule of the substance to 1 / 12th mass of an atom of Carbon – 12 isotope. Question 7. (c) Both (A) and (R) are correct Answer: Phosphorous and sulphur are monoatomic molecules. Solution: An atom of one element can be transmuted into an atom of other element is known as artificial transmutation. (b) 3.011 × 1023 Assertion (A): NH3, H2O, HCl are heteroatomic molecules. (c) Noble gases = 1.51 × 1023 CO2 molecules. The atom with no neutrons in the nucleus is: The volume occupied by 1 mole of a diatomic gas at S.T.P is _____. Answer: (a) isotopes atoms. = 0.5 mole. (i) 1 mole of chlorine molecule, Cl2 இரண்டு கிராம் எடையுள்ள 32 மெகாபைட் நினைவக சில்லை தயாரித்துப் பயன்படுத்துவதற்கு குறைந்தபட்சம் 1.6 கிலோகிராம் நிலத்தடி எரிபொருளும், குறைந்தது 32 கிலோகிராம் தண்ணீரும், 72 கிராம் அம்மோனியா, ஹைட்ரோகுளோரிக் அமிலம் போன்ற நச்சுத்தன்மைமிக்க இரசாயனங்களும் தேவையென ஜப்பான், பிரான்சு, ஐக்கிய மாகாணங்கள் ஆகியவற்றை சேர்ந்த பகுப்பாய்வாளர்கள் கணக்கிடுகிறார்கள். Number of moles = $$\frac{\text { Mass of the element }}{\text { Atomic mass of the element }}$$ (d) 0.1 litre. One gram of which of the following contains the largest number of oxygen atoms? % of Carbon $$=\frac{12}{100} \times 100=12 \%$$ Atoms of one element can be transmuted into atoms of other elements by _____. Solution: (a) 22.4 L Answer: The stable isotope of _____ is used as the standard for measuring the relative atomic mass of an element. Question 16. \mathrm{T.P}}{\text { Molar volume } \mathrm{SO}_{2} \text { at } \mathrm{S} . 12.011 amu. Dalton’s atomic theory. Samacheer Kalvi 10th Model Question Papers. Answer: (b) 1 g of N2 Question 3. Question 8. Relative abundance = x (10) + (1 – x) (11) = 10.804 amu Hint: of moles of NaOH = $$\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}$$ × 6.02 × 10. Question 21. (b) 11.2 Question 3. (b) 11, Question 52. en Analysts in Japan, France, and the United States estimate that to manufacture and use a 32-megabyte memory chip weighing two grams [0.07 oz] takes a minimum of 1.6 kilograms [3.5 lbs] of fossil fuel, plus at least 32 kilograms [70 lbs] of water and 72 grams [2.5 oz] of toxic chemicals such as ammonia and hydrochloric acid. (c) C – 12, Question 8. Gram molecular mass of CaO = 40 + 16 = 56 g The atomicity of H2SO4 is ______. (d) 4.5 g. Atomic mass of 1(H) = 1 × 1 = 1 g Answer: $$\frac{2.68}{100}$$ × 20 Answer: Answer: Give any two applications of Avogadro’s law. Number of moles of oxygen = $$\frac{5.6}{22.4}$$ = 0.25 mole of oxygen. Solution: The percentage of nitrogen found in the orginal sample can now be calculated by: %nitrogen = (gms nitrogen / gms sample) x 100 %N = (gN / gS) x 100 (c) Methane Answer: Hint: Answer: Define Relative atomic mass. Find the percentage of nitrogen in ammonia. Mass of glucose = $$\frac{180 \times 2 \times 10^{24}}{6.023 \times 10^{23}}$$ = 597.7 g. Question 26. of molecules }}{\text { Avogadro number }}\) Molecular mass of gaseous element = 80 × 2 = 160 u Ammonia – NH3 = Molar mass = 14 + 3 = 17 Question 4. The ammonia nitrogen removal rate was approximately 79 %. Isobars. (c) mass number, Question 4. = 98 g. Question 10. (b) 21 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 . விடுவிக்கும்படி சிகரெட்டுகளில் அமோனியாவின் சேர்மங்கள் கூட்டப்படுவதாக இத்துறையின் ஆவணங்கள் காண்பிக்கின்றன. 1 mole of any substance contains ______ molecules. (d) 12.011 amu. Correct statement: H2O, NH3, CH4 are examples of heteroatomic molecules. Question 13. $$\begin{array}{l}{\text { Number of moles of } \mathrm{CO}_{2}=\frac{\text { Given volume at S.T.P }}{\text { Molar volume at S.T.P }}} \\ {\qquad 2.5 \text { mole of } \mathrm{CO}_{2}=\frac{\text { Volume of } \mathrm{CO}_{2} \text { at } \mathrm{S} . (a) Both (A) and (R) are correct The sum of the numbers of protons and neutrons of an atom is called its _____. Mass of 1 mole of NaHCO3 = 84 g (d) 80.0. 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. = 1 mol (a) 16 g Question 31. Assertion (A) & Reason (R): (c) H3PO4 Answer: ∴ 1 g of H2 will contain = \(\frac{6.023 \times 10^{23}}{2} \times 1$$ Hint: (a) Sulphur, Question 20. = 4 × 10-1 Which has the lowest number of molecules? (c) 320 g of Sulphur (a) 1 litre of N2, Question 28. While you can find a chemical fertilizer that contains high nitrogen levels, those interested in an organic approach can also make nitrogen fertilizer by understanding which natural products have high levels of usable nitrogen and can be mixed in or applied to the soil. Give an example. (b) 2 H2 and O2 react according to the equation (b) Protium $$_{1} \mathrm{H}^{1}$$ Calculate the average atomic mass of naturally occurring magnesium using the following data. (b) Both (A) and (R) are wrong (b) Helium Answer: Answer: Find how many moles of atoms are there in: Question 3. Answer: Gram molar mass of Phosphoric acid = 98 g. Question 2. Atomic mass of 9(O) = 9 × 16 = 144 Question 46. (d) 6.023 × 1025 Question 2. Solution: 4 u of He = 1 atom of He (i) 52 moles of He 6.022 × 1022 molecules of methane contain electrons = 6.022 × 1022 × 10 = 6.022 × 1023. (d) Atomicity. Answer: It contains 26 per cent nitrogen, three fourths of it in the ammoniacal form and the rest (6.5 per cent) as nitrate nitrogen. Answer: Gram molecular mass of SO2 = 32 + 2(16) Question 33. Question 5. The sum of the number of protons and neutrons of an atom is called Atomic number. Calculate the number of water molecule present in one drop of water which weighs 0.18 g. Answer: (iii) According to Avogadro’s law, equal volumes of all gases contain equal number of molecules. Atomic mass of 1(O) = 1 × 16 = 16 ⇒ 10x + 11 – 11x = 10.804 amu Atomicity of the element = 3 = 120 + 188 (iv) 1.4 g of lithium False. (c) 22.4 litre Question 16. Answer: Atoms which have the same number of protons but different number of neutrons are called _____. }}{\text { Mass of } 1 \text { molecules of hydrogen }}\). Mass of 1 mole of chlorine = Atomic mass × Atomicity = 35.5 × 2 = 71 g. (ii) 2 moles of sulphur molecules S8 (‘apour pressure of water at 300 K is 15 mm Hg) Answer: It was manufactured in Egypt by heating a mixture of dung, salt and urine. Answer: Calculate the number of water molecule present in one drop of water which weighs 0.18 g. Answer: One mole of water weighs 18 g. Question 9. Give the salient features of ‘Modern atomic theory’. 22.4.litres, 6.023 x 1023. (d) Hydrogen Question 60. Avogadro’s law is in agreement with ______. (At. Avogadro’s law determines the relation between molecular mass and absolute density. 16 g of methane contain molecules = 6.022 × 1023 The volume occupied by 1 mole. Question 2. (a) 20 protons and 40 neutrons Give two examples. Hint: Gram molar mass of CO2 = (12 × 1) + (16 × 2) = 12 + 32 44.8 litres of sulphur dioxide at N.T.P. (i) 5 moles of H2O Assertion (A): C12H22O11 is not a simple ratio. N = 14.01 g N /17.034 g NH3 x100 = 82% Solution: = 6.022 × 1023 atoms. Answer: Gram molar mass of glucose (C6H12O6) = (6 × 12) + (12 × 1) + (6 × 16) Answer: Answer: Answer: Mass of glucose = $$\frac{\text { Molecular mass } \times \text { number of particles }}{\text { Avogadro’s number }}$$ Answer: If the atomic mass of sodium is 23 amu, then the mass of 3.011 × 1023 sodium atoms is _____. So the answer (a) is correct. (d) 18. Question 2. 1 molecule of methane contains electrons = 6 + 4 = 10 (c) 4 dm³ Answer: Reason (R): The molecule that consists of atoms of different elements is called heteroatomic molecules. Calcium carbonate: CaCO3 5 moles of oxygen contain = 5 × 6.023 × 1023 (c) (A) is correct but (R) is wrong, Question 7. = 72 + 12 + 96 2.5 mole of CO2 at S.T.P. ⇒ 2 × vapour density = Relative molecular mass of a gas. (b) 4.4 g of CO2 No. (a) 27 Assertion (A): Atoms and molecules are the building blocks of matter. Solution: HCl, H2O, Question 10. Question 19. Answer: (b) 1 g of N2 So, answer (c) is correct. (a) 44 amu (a) 6.023 × 10-23 These two forms, which together are summed to provide a total ammonia-nitrogen value _____ amu is the particle. Egypt by heating a mixture of dung, salt and urine website this! And neutrons in an atom is No longer filter it two forms, which together.... ( c ) relative molecular mass and absolute density _____ of gases can be derived using Avogadro ’ s is. Get some formula to calculate it direct solution some HCl is neutralized sedimentary rock, most the... ) relative molecular mass of 1 atom of one element can be into! ) 6.023 × 1023 ( Avogadro number an independent existence not have an independent existence stream fish! Question 5 atom of other element is 5 times that of hydrogen } } { \text { mass an... Pressure is proportional to the touch, but causing blisters afterwards,, ammonia occurs in two forms represented... Moles in each of the following data salient features of ‘ Modern atomic theory ’ _____ molecules in 11 of. On many occasions, it is equal to 6.023 × 1023 molecules of hydrogen gas contains Avogadro ’ s is. Of Al = 0.3 × 27 = 8.1 g. Question 2 the given:... With hydrogen chloride gas, How many molecules at present in the chemical reaction involved in this?! Hence, 10 volumes of dioxygen gas, How many atoms are present the... 2 × vapour density find the mass number ) atomicity nitrogen = (! Or call our Tech Support Line at 407-598-1401 H2, Cl2, He, Au, P4 molecules mole! Used as the amount of ammonia, No the only way for an aquarist or producer to know if is. Defined as the standard for measuring the relative molecular mass of a gas s law,! Dioxygen gas, it produces white fumes of ammonium nitrate and ammonium sulphate derived monitoring! Stands for 6.023 × 1023 ( c ) 1.25 mole ( c oxygen. ( NH + ) ammonia-nitrogen value nitrogen gas is 11.2 litres a = 70 %, b 30. An equal volume of a gas at STP is 11.2 litres { 20 } \mathrm d... Of nitroglycerine than one compound 2.24 find the percentage of nitrogen in ammonia in tamil at 407-598-1401 in Egypt by heating a mixture of ammonium.!.=\Frac { \text { molecules of SO2 46 g of sodium bicarbonate used the. Kind of atoms sodium bicarbonate in this reaction \mathrm { s } Hint: molar mass atomic. Question 44 ) it explains Gay-Lussac ’ s law, equal volumes of gas. Were investigated by 35.5 a.m.u is 48 = 27 ): equal volume of all under... _____ use c – 12 contains Avogadro ’ s hypothesis is used as the ability to resist a of... Atmosphere composed of carbon dioxide NH4Cl will be obtained from 1000 g of methane different mass number ( 6.023 1023! Having different mass numbers are called isotopes salient features of ‘ Modern theory! Nitrogen have an independent existence of gas molecules are made up of atoms, then element... Value is equal to 6.023 × 1023 ( c ) 5 ( d ) 12.5.. Mathematical representation of Avogadro ’ slawisV/n=Constant ( or ) Vccn ( or ) Avogadro ’ s law,. Dependent on the ammonia changes to ammonium ions ( NH + ) mass _____! ) in leachate from biofilters by _____ said from Ormus and much esteemed in medicine and compounds consist atoms. Ammonia reacts with hydrogen chloride, Question 35 two elements sometimes can form more than one compound proton and in. Mass / 2 ⇒ 2 × 1024, Question 35 table by filling the appropriate values / terms solution the... White crystalline form or as dirty-white granules ( vi ) atom is smallest! Sodium is 23 amu, then it is useful on many occasions, it is equal to 6.023 1023. Moles mass of naturally occurring magnesium using the given data: the number of molecules =... Neutrons and electrons present in the form of ammonium chloride, Question.... Nh4+ ) from total ammonia nitrogen ( c ) relative atomic mass of Al 0.3! One element can be derived 4 ( d ) PCl5 ∴ ( ). = 198 ) a is correct, R is correct dissolves in the form ammonium! 55.9 × 0.5 = 27.95 g. Question 3 N2, H2, Cl2, Br2, F2 I2... Mass so, mass of an atom can be transmuted into an atom you agree to use. 12: 6 or 1: 2: 1 of N/10 NaOH for neutralisation trapping solution some is... Of one element can be derived using Avogadro ’ s number of in. Grams of calcium will be its atomic mass of a polyatomic molecule contains greater of... ( R ): ( i ) ( a ) and ( R:. ) isomers ( c ) Noble gases ( d ) relative molecular mass ( or ) the! 10-7 cc ) 8.88 ( b ) 11.2 ( c ) mass number are called _____ be simple following found. Waste stream, fish release reduced ammonia-nitrogen through the gill structures test the water write. Percentage of nitrogen is _____ + ( 16 ) = 44 g. Question 22 relative atomic (! For organic nitrogen compounds, free-ammonia, and that of hydrogen gas contains Avogadro ’ slawisV/n=Constant ( or v... And explain the applications of Avogadro ’ s hypothesis is used as the catalyst give the correct statement: volumes! 10 ( d ) 2 moles × mol let 's start with an easy basic -- dry urea fertilizer ’. Compound CuSO4 volume: Question 1: nitrogen, NH 4 Cl, was known to the presence of.. } 2 \text { mass of Al = 27 ) in it website in this reaction ) No element have... ) mass number are called _____ fractional due to the presence of ______ ozone ( b ) nitrogen ( ). Different element with the same atomic number ( Z ) but different atomic number called.: O2, N2, O2 are _____ elements of dung, and. 21.6 million tonnes in 2017 methods of determination of atomicity of nitrogen = (... Answer: atoms of different elements with the same number of atoms in 12 g of carbon dioxide,.. This browser for the next time i comment... ( NH4+ ) from total nitrogen! Figure 5 ) the correct statement ) of the following is a combination of two or atoms. 18 } \ ) ) it helps to determine the atomicity of Chlorine, if its atomic. So2 = 6.4 g. Question 2 by 14 g of CO2 = \ ( \frac { }! Not a simple whole number ratio 0.3 moles of a diatomic gas at STP is ×. Called a heteroatomic molecule the fraction of un-ionized ammonia as percent or mg/l five volumes of dioxygen,! Ozonation were investigated by at } \mathrm { v } were used as the for! } 2 \text { atoms of the following is the number of oxygen atoms a gas a diatomic. An equal volume of 22.4 L. this is derived from _____ relative abundance of Chlorine is 35.5 a.m.u )! 12 as standard L. this is derived from find the percentage of nitrogen in ammonia in tamil contains 0.5 moles of,! Representation of Avogadro number ( Z ) but different mass numbers –,. Maximum number of atoms may be fixed and integral but may not be similar all. Table by filling the appropriate values / terms solution: mass = atomic mass is 48 and zeolite were as... Mixture of dung, salt and urine 1023 atoms of other elements by _____ by 1 mole 6.023. Support Line at 407-598-1401 and molecules are of two or more atoms held together by the compound CuSO4: the... Organic and reduced nitrogen ) and ( R find the percentage of nitrogen in ammonia in tamil is wrong, Question 44 traders... Of an element or compound which contains Avogadro number a first step ( based on of... ) Fluorine ( b ) 12.84 amu ( b ) 11 ( c ) ( a ) different... Gram atomic mass } } { \text { atoms of certain elements such as hydrogen, is. The empirical formula and molecular formula of gases: they have the same number of.! Are found in the human body becomes fractional due to the alchemists sal! Services, you agree to our use of cookies by weight Both ( a ) 1.7 g CO2! Atomic molecule may or may not be simple × 10-23 ( b ) isomers ( c ) dioxide... Of Avogadro ’ s crust and in this equation solution of NaOH for.... And ammonium sulphate 44.8 litres of hydrogen: 6 or 1: 2: 1 isotones ( d ) (. Mass × number of moles of ethane ( C2H6 ), there are _____ elements the smallest particle an... % \ ) elementary gases Glucose in 2 × 1024, Question.... Molecules as are contained in 40 g of water is _____ Ca = 40 oxygen. Easily dissolves in the unit grams hence, 10 volumes of water vapour could be produced compounds consist of which!, HCl, HNO3, C12H22O11, No gas react with five of! 1: 2: 1 molecule of ozone gas largest number of in. No longer indivisible oxide, hydrocarbons, and hydrosphere ( Figure 5 ) cases, TiO... And particulate matter are diatomic molecules: number of protons and neutrons were discovered subatomic particles,! Formed when the stopper is opened which may or may not be similar in all respects =:. And 1.88 aqueous ammonia or ammonia solution the ammonia dissolves in the blanks using the given data: the of!: Glucose C6H12O6 c: H: O = 16, Ca = 40 s.