Volume occupied by gas at NTP = moles × 22.4 = 0.5 × 22.4 = 11.2 liters. => x = (2.44×10-23)1/3 = 2.9×10-8 cm. 10 mL of 2(M) NaOH solution is added to 200 mL of 0.5 (M) of NaOH solution. Question 32. One mole is defined as the amount of substance of a system which contains as many entities like, atoms, molecules and ions as there are atoms in 12 grams of carbon - 12". of moles of solute /Volume of solution( l) = 1.4×1000/100 = 14 M, 14. Server 1 Server 2. An atom of some element X weighs 6.644 × 10-23 g. Calculate the number of gram-atoms in 40 kg of it. Question 28. 0.6 g of urea on strong heating with NaOH evolves NH3. A transition metal M forms a volatile chloride which has a vapour density of 94.8. Moles of CH3OH is 5.2, Xsolute = 5.2/(5.2+1000/18) = 5.2/(5.2+55.556) = 5.2/60.756 = 0.086, JEE Main Mole Concept Previous Year Questions with Solutions, CBSE Previous Year Question Papers Class 10, CBSE Previous Year Question Papers Class 12, NCERT Solutions Class 11 Business Studies, NCERT Solutions Class 12 Business Studies, NCERT Solutions Class 12 Accountancy Part 1, NCERT Solutions Class 12 Accountancy Part 2, NCERT Solutions For Class 6 Social Science, NCERT Solutions for Class 7 Social Science, NCERT Solutions for Class 8 Social Science, NCERT Solutions For Class 9 Social Science, NCERT Solutions For Class 9 Maths Chapter 1, NCERT Solutions For Class 9 Maths Chapter 2, NCERT Solutions For Class 9 Maths Chapter 3, NCERT Solutions For Class 9 Maths Chapter 4, NCERT Solutions For Class 9 Maths Chapter 5, NCERT Solutions For Class 9 Maths Chapter 6, NCERT Solutions For Class 9 Maths Chapter 7, NCERT Solutions For Class 9 Maths Chapter 8, NCERT Solutions For Class 9 Maths Chapter 9, NCERT Solutions For Class 9 Maths Chapter 10, NCERT Solutions For Class 9 Maths Chapter 11, NCERT Solutions For Class 9 Maths Chapter 12, NCERT Solutions For Class 9 Maths Chapter 13, NCERT Solutions For Class 9 Maths Chapter 14, NCERT Solutions For Class 9 Maths Chapter 15, NCERT Solutions for Class 9 Science Chapter 1, NCERT Solutions for Class 9 Science Chapter 2, NCERT Solutions for Class 9 Science Chapter 3, NCERT Solutions for Class 9 Science Chapter 4, NCERT Solutions for Class 9 Science Chapter 5, NCERT Solutions for Class 9 Science Chapter 6, NCERT Solutions for Class 9 Science Chapter 7, NCERT Solutions for Class 9 Science Chapter 8, NCERT Solutions for Class 9 Science Chapter 9, NCERT Solutions for Class 9 Science Chapter 10, NCERT Solutions for Class 9 Science Chapter 12, NCERT Solutions for Class 9 Science Chapter 11, NCERT Solutions for Class 9 Science Chapter 13, NCERT Solutions for Class 9 Science Chapter 14, NCERT Solutions for Class 9 Science Chapter 15, NCERT Solutions for Class 10 Social Science, NCERT Solutions for Class 10 Maths Chapter 1, NCERT Solutions for Class 10 Maths Chapter 2, NCERT Solutions for Class 10 Maths Chapter 3, NCERT Solutions for Class 10 Maths Chapter 4, NCERT Solutions for Class 10 Maths Chapter 5, NCERT Solutions for Class 10 Maths Chapter 6, NCERT Solutions for Class 10 Maths Chapter 7, NCERT Solutions for Class 10 Maths Chapter 8, NCERT Solutions for Class 10 Maths Chapter 9, NCERT Solutions for Class 10 Maths Chapter 10, NCERT Solutions for Class 10 Maths Chapter 11, NCERT Solutions for Class 10 Maths Chapter 12, NCERT Solutions for Class 10 Maths Chapter 13, NCERT Solutions for Class 10 Maths Chapter 14, NCERT Solutions for Class 10 Maths Chapter 15, NCERT Solutions for Class 10 Science Chapter 1, NCERT Solutions for Class 10 Science Chapter 2, NCERT Solutions for Class 10 Science Chapter 3, NCERT Solutions for Class 10 Science Chapter 4, NCERT Solutions for Class 10 Science Chapter 5, NCERT Solutions for Class 10 Science Chapter 6, 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, JEE Main Chapter Wise Questions And Solutions. Solution — 0 /0. Practice Now. Mass of 5 moles of CaCO3 = 5 × 100 = 500g. 6.02Ã—10 22 molecules of N 2 at NTP will occupy a volume of In diatomic gases, No. = M × V(in liter) 3. Solution — => 4 × 0.75 = x × 1 JEE Main Previous Year Papers Questions of Chemistry With Solutions are available at eSaral. The ratio of masses of oxygen and nitrogen in a particular gaseous mixture is 1 : 4. = 40 × 1000/40 = 1000. Practice Now. 20 mole of O = 20 × 6.022×1023 = 1.204×1025 O atoms. #2 | Questions on Mole Concept (Chemistry) > Some Basic Concepts Of Chemistry. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number. A C-12 atom contains 12 nucleons (6 protons and 6 neutrons, A = Z + N) What is the mass of 4.20 mol of the element iron (Fe)? of solution in L) Download Mole Concept Previous Year Solved Questions PDF. Mass of Hydrogen atoms = 93×1 = 93 (1) MCl2 M C … A polystyrene, having the formula Br3C6H3(C3H8)n, was prepared by heating styrene with tribromobenzoyl peroxide in the absence of air. Most of our routine items are sold in specific numerical quantities along with definite names. Percentage composition and Molecula.. This allows us to talk about relative quantities of substances in the macroscopic world and to know the relative number of atoms (or smallest particles) in each bulk substance. Question 11. Given that the vapour density of a gas is 11.2. 10 mole of H = 10 × 6.022×1023 = 6.022×1024 H atoms 2. = Mass / 30 × Av. Download Mole Concept (Chemistry) notes for IIT-JEE Main and Advanced Examination. = 0.04375. Moles of oxygen atoms in 1 mole of Na2CO3.10H2O = 3+10 = 13 = 0.00166. Volume of 1 mole LiF arranged in cube Question 39. = 1.23×1023 cc. 1 mole of KClO3 contains = No. 3g of activated charcoal was added to 50 mL of acetic acid solution (0.06N) in a flask. 15. Which of these is … Length of edge of the cube = (9.78)1/3 = 2.138 cm, No. Solution — The density of a solution prepared by dissolving 120 g of urea (mol. mass = 60 u) in 1000 g of water is 1.15 g/mL. This number is also called Avogadro's number. = No. mass of C2H5OH = Mass of H2O/ mol. of atoms of A = (x/20) × N    [N is Avogadro constant] Highest 120/120. Charge on 1 mole Al3+ ions Which will be the same for these two titrations? Solved Examples on the Mole Concept. Empirical & Molecular Formula: Q.29-Q.32C. of atoms/Avogadro constant Question 45. Question 15. Then, Mole ratio const. 4. Molar Mass of $H_2O$ = 2 + 16 = 18 … Made by expert teachers. = Mass of one metal atom/density One mole of oxygen gas contains Avogadros number of atoms. = 2 × 6.022 × 1023 = 12.044 ×1023 oxygen atoms. The mole concept It is convenient to consider the number of atoms needed to make 12g of carbon and for this number to be given a name - one mole of carbon atoms. 2 × moles of O2 = y × moles of AxOy Mole: Mole is the measurement in chemistry.It is used to express the amount of a chemical substance. No. = Volume ratio [∵ Avogadro’s Principle – the molar ratios are also volume ratios for gases]. mass of W Oxygen is present in a 1-liter flask at a pressure of 7.6 × 10-10 mm of Hg at 0oC. 1 mole = 6.022 x 10 23 atoms or molecules or formula units of that substance. Find the charge of 1 g-ion of N3- in Coulombs. = 40 g of chlorine atom = 35.5g of chlorine atom, Given 71g of chlorine atom=2× 6.023× 1023. no. Solution — The word “mole” was introduced around the year 1896 by the German Chemist Wilhelm Ostwald, who derived the term from the Latin word moles meaning a ‘heap’ or ‘pile. 1/8 mole Answer-12 Post-Your-Explanation-12 13. Number of atoms in the following samples of substances is the largest in : 1mole of magnesium = 24g of Mg = 6.023×1023no.of Mg, no. No. Mole Concept Questions Sacred Texts contains the web’s largest collection of free books about religion, mythology, folklore and the esoteric in general. 1 molecule of O2 = 2 oxygen atoms Practice Now. The empirical formula for hydrocarbon A is C 2 H 7 O. => No. The solved questions answers in this Test: Mole Concept quiz give you a good mix of easy questions and tough questions. 1 mole of H2SO4 contains 2 mole of H, 1 mole of S, and 4 mole of O Solution — How many iron atoms are there in a haemoglobin molecule? No. Find the ratio of the volumes of the gases. Solution — of molecules in 5.6 L gas = 0.1 × 6.022×1023 Solution — = 1021/6.022×1023 1 mole of phosphorus weighs 31g, therefore, atomic mass of phosphorus is 31. Calculate the average atomic mass of chlorine- Mole Calculations, also commonly known as Mole Concepts & Chemical Calculations had been identified by students and educators alike, to be one #1 Killer Topic in GCE ‘O’ Levels Chemistry, IP Chemistry, IB Chemistry and IGCSE Chemistry.. Based on only these two elements, estimate the mass percentage composition of the universe. Solution — From the formula Br3C6H3(C3H8)n, we have, The mole concept. = 3 × 1.602×10-19 × 6.022×1023 Coulombs 1 mole of Cl = 6.022×1023 Cl atoms Question 43. Pressure = 7.6 × 10-10 mm Hg of atoms of hydrogen= 4 moles of hydrogen atom. The number 6.02214076× 1023 is known as the Avogadro constant and is denoted by the symbol ‘NA’. Create your notes while watching video by clicking on icon in video player. The molality of the solution will be (molar mass, NaCl = 58.5 g mol-1), Mass of weight W2 of NaCl in 1L solution W2 = 3×58.5 = 175.5g, Mass of H2O in solution (W1) = 1250-175.5 = 1074g, m = W2×1000/Mw2 ×W1 = (175.5×1000)/58.5×1074.5 = 2.79m. = No. Question 34. Q. Molar mass (i.e., molecular mass in g) = 40+12+3×16 = 100g The density of He gas at NTP is 0.1784g/L. Solved Examples. No. = 9.12×1023 /7.42 Solution — => 11.4 L of SO2 = 0.5 mole SO2 = 0.5× 6.022×1023 = 3.011×1023 SO2 molecules. Calculate the number of oxygen atoms in 0.2 mole of Na2CO3.10H2O. The ratio of number of their molecule is : Given ratio of masses of oxygen and nitrogen = 1:4, Ratio of number of molecules = w/(32×NA)÷4w/(28×NA). It is found that in 11.2 liters of any gaseous compound of phosphorus at NTP, there is never less than 15.5 g of P. Also, this volume of the vapour of phosphorus itself at NTP weighs 62 g. What should be the atomic mass and molecular mass of the phosphorus? = 7.6 × 10-10/ 760   [1 atm = 760 mm Hg] 1 … 2. Solution — Question 36. Question 1. of moles in 0.05 liter of H2SO4 Equal masses of oxygen, hydrogen and methane are taken in a container in identical conditions. Calculate the number of oxygen atoms in 1 mole of O2. 1 mole of the vapour of phosphorus weighs 124g, therefore, molecular mass of phosphorus is 124. Question 4. No. MCQ quiz on Mole Concept multiple choice questions and answers on Mole Concept MCQ questions on Mole Concept objectives questions with answer test pdf for interview preparations, freshers jobs and competitive exams. The density of a particular crystal of LiF is 2.65 g/cc. Solution: We can solve this problem in to ways; 1st way: 6,02x1023 amu is 1 g 24 = 1 mole 1. of moles of Cu 2. => x = 3, Applying POAC for O atoms, of atoms in 100 u of He = 100/4 = 25 He atoms. = 0.25 × 0.075 A. At room temperature, the density if water is 1.0 g/mL and the density of ethanol is 0.789g/mL. 1 mole molecules of any ideal gas occupies 22.4 L at NTP. ∴ moles of CaWO4 × at. Solution — Q.1: How many moles of iron are present in a pure sample weighing 558.45 grams? Answered by Expert NEET NEET Chemistry Some Basic Concepts in Chemistry mole concept Asked by pradeepthakur8969 28th June 2019 1:27 PM . Mole Concept Previous Year Questions with Solutions are given here. Atomic mass of Al = 27 We know mole fraction = moles of solute/(moles of solute + moles of solvent), Let mass of water is 1 kg . 1 mole of SO2 = 22.4 L (at NTP) = 1 × 100 g =  100 g. Question 2. If a mole were to contain 1× 1024 particles, what would be the mass of (i) one mole of oxygen, and (ii) a single oxygen molecule? The molar ratios are also volume ratios for gases (Avogadro’s principle). Calculate the standard molar volume of oxygen gas. of mole of KClO3 = 122.5g/122.5g = 1 mole. Solution — Question 14. Like the word "dozen" represents the number 12, so "mole" represents the number 6 x 10 23. So, the atomic mass of X = 40. This is where the mole concept is widely used. Solution — = 6.644 × 10-23 × 6.022×1023 of electron in 1 molecule of CH4 = 6+4 = 10 electrons Calculate the number of atoms in 5.6 liters of a (i) monoatomic, and (ii) diatomic gas at NTP. No. Liberated NH3 will combine with which of the following HCl solution? Question 8. Q3: Is mole a unit? = Molar ratio   (Avogadro’s principle – the molar ratios are also volume ratios for gases) of atoms of B Question 30. Any measurement can be broken down into two parts – the numerical magnitude and the units that the magnitude is expressed in. = 0.01875, Total no. A. Solution: 1 mole of KBr contains 1 mole of potassium ions (K+) and 1 mole of bromide ions (Br-). Solution — Solution: 1 mole of Ag atoms = 108 g = 6.022 x 10 23 atoms. Problems Based On Mole Concept (With Solutions) – Exam Secrets Free Question Bank for JEE Main & Advanced Chemistry Some Basic Concepts of Chemistry The mole concept = 32/1 × 1024 Number of atoms in the following samples of substances is the largest in : (1) 127.0g of iodine. If the molar mass of the hydrocarbon is 141 g/mol, determine the molecular formula for this hydrocarbon. Given a solution of HNO3 of density 1.4 g/mL and 63% w/w. Q. Mass of 1 mole X atoms Question 20. = (16 × 107/Av. of LiF molecule per mole Answer: GAM of Helium = 4 g Number of mole atoms in 4 g of Helium = 6.022 × 10 23 Number of atoms in 1 gofHelium = $$\frac { 1 }{ 4 }$$ × 6.022 × 10 23 So, 1 mole of O2 = 2 mole oxygen atoms Moles of C2H5OH in V mL = Moles of H2O in 175 mL Watch Next Video. = 2.65 × 1010. of moles of CO2 left Solution: We can solve this problem in to ways; 1st way: 6,02x1023 amu is 1 g 24 Solution — = 0.025 + 0.01875 Empirical & Molecular Formula: Q.29-Q.32C. Unable to watch the video, please try another server . Suppose the side of cube = x cm = diameter of mercury atom Total no. 7. 4. The empirical formula for hydrocarbon A is C 2 H 7 O. 13. of moles of solute/ Volume of solution in Liters = 1.201×1024/2 Change ), You are commenting using your Google account. Mass of 1 mole He = Density at NTP × Standard molar volume = 0.1784 × 22.4 ≈ 4g. Mixed Concept problems: Q.1-49-Q.85. Calculate the number of Cu atoms in 0.635g of Cu. ( Log Out /  These short solved questions or quizzes are provided by Gkseries. 0.030 C. 0.30 D. 3.0. It has been estimated that 93% of all atoms in the entire universe are hydrogen and that the vast majority of those remaining are helium. mass of W. As both CaWO4 and FeWO4 contains 1 atom of W each, = 0.025, No. moles of carbon atoms = 12/12 = 1 of atoms = 2 × No. of moles of CaCO3 1 mole of water (H 2 O)contains 2 moles of hydrogen atoms and 1 mole of oxygen atoms. No. Mole Concept, Class 9 Science. Solution — ∴ No. There will be total 20 MCQ in this test. = 0.25 × 6.022 × 1023 No. = Mass of CO2/Molecular mass = 1:16:2. Let the volume of ethanol containing the dame number of molecules as are present in 175mL of water be V mL. Standard molar volume Moles of CH4 = 1.6/16 =0.1 Calculate the volume of 20g H2 at NTP. => 0.0001 mole of H2SO4 contains 0.0001 mole SO42- Question 22. 1 mole = 6.022 x 10 23 atoms or molecules or formula units of that substance. Mass of one mole of oxygen molecule (O2) 8. = 10-12 atm. The molecular weight of haemoglobin is about 65,000 g/mol. What is the Mole Concept? Separate 20.0 cm 3 solutions of a weak acid and a strong acid of the same concentration are titrated with NaOH solution. 0.030 C. 0.30 D. 3.0. This contains 14 Multiple Choice Questions for Class 11 Test: Mole Concept (mcq) to study with solutions a complete question bank. Calculate the total number of electrons present in 1.6 g of CH4. Watch Previous Video. const. Made by expert teachers. If we have x atoms of Carbon and y atoms of Hydrogen, Given one molecule of compound ( CxHyOZ ) contains half as much oxygen as required to burn one molecule of compound CXHY completely to CO2 and H2O. Solution — ∴ y = x × N/20 => x = 20y/N This short notes on Mole concept and Stoichiometry will help you in revising the topic before the NEET Exam. Calculate the apparent volume occupied by one atom of the metal. It is a very very big number (6 followed by 23 zeros). Determine the molarity of HNO3 solution. Question 21. Volume = mass / density = 100g/1.4 g/ml = (100/1.4)ml, Molarity = no. Molarity = 120 / 60 1120 / 1.15 = 2 × 1.15 1120 × 1000 = 2.05 M = 120 / 60 1120 / 1.15 = 2 × 1.15 1120 × 1000 = 2.05 M. Q. 40 ACC- CH-MOLE CONCEPT BANSAL CLASSES Private Ltd. ‘Gaurav Tower’, A-10, Road No.-1, I.P.I.A., Kota-05 SOLVEDEXAMPLES Q.1 Naturallyoccurringchlorineis 75.53%Cl35 which hasan atomicmassof34.969amu and 24.47% Cl37 which has a mass of 36.966 amu. Question 12. The molarity of this solution is. = (2x/40) × N Some Basic Concepts of Chemistry Mole Concept Test 2 Start Test ATTEMPT THIS TEST AND COME BACK TO CHECK YOUR RESULT Lowest-24/120. When dealing with particles at an atomic (or molecular) level, even one gram of a pure element will contain a huge number of atoms. 1 molecule of H2SO4 contains 1 SO42- ion = 2 × 12 CIE IGCSE Chemistry exam revision with multiple choice questions & model answers for The Mole Concept. An atom of some element X weighs 6.644 × 10-23 g. Calculate the number of gram-atoms in 40 kg of it. 11.2 L (½ mole) of any gaseous phosphorus compound contains at least ½ mole, 15.5g, of phosphorus. ∴ Volume of 1 Hg atom = x3 and 0.224 L of H 2 gas at S.T.P is equivalent to. The Mole: A mole of a substance is the amount that contains the same number of units as the number of Carbon atoms in 12 grams of carbon-12. = Avogadro constant = No. Solution — Mass of given sample of C2H6 = mass of 107 CH4 molecules = 16 × 107/Av. So one mole of HCl = 2 mole of urea = 2×0.6/60 = 0.02 mol. = No. = volume occupied by 1 mole (i.e., 32g) of the O2 gas at NTP Stoichiometry: Q.33-Q.40D. of mole of A = x/20 No. 5. Solution — These short objective type questions with answers are very important for Board exams as well as competitive exams IIT-JEE, AIIMS, NEET etc. Question 24. = 6.022 × 1023/ 6.022 × 1023 of moles of Carbon atoms Question 1: Calculate the mass of (i) an atom of silver (ii) a molecule of carbon dioxide. Mole concept and Stoichiometry is an important topic from NEET Exam Point of view. => V = 566.82 mL. const × 30) × Av. = 227.5 mass of W = Moles of FeWO4 × at. 1 mole of diatomic gas (1 molecule contains 2 atoms) occupies 11.4 L at NTP. 1 mole of water (H 2 O)contains 2 moles of hydrogen atoms and 1 mole of oxygen atoms. This course will contain the solutions of previous year questions for NEET of LiF molecules present in 1 mole (6.639+18.998=25.937g). Solution — = 0.44×10-13 × 6.022 × 1023 Gas Laws Mole Concept Extended activities. BYJU’S provides accurate solutions prepared by our specialised experts. Molecular mass of CO2 = 12 + 2 × 16 = 44, Total no. Mass percentage of Helium = (28/93+28) × 100 = 23.14%. Question 7. = mass/density The ratio of mass percent of C and H of an organic compound (CxHyOz) is 6 : 1. If atomic mass of Mg atom is 24 g, find mass of 1 Mg atom. The density of mercury is 13.6 g/cc. A 5.2 molal aqueous solution of methyl alcohol, CH3OH, is supplied. = Mass of Cu/Atomic mass mass of H2O Solution — Question 33. MOLE CONCEPT. of Fe atoms in a haemoglobin molecule = 227.5/56 ≈ 4. What is the Mole Concept? What conclusions can be drawn from these data the product of the reaction? What amount of oxygen, O 2, (in moles) contains 1.8 ×10 22 molecules? mass of W = Moles of W in FeWO4 × at. of moles of Br = 3 × moles of Br3C6H3(C3H8)n An open vessel at 300 K is heated till ⅖ th of the air in it is expelled. = 25.937/2.65 Solution — 4 × moles of A4 = x × moles of AxOy There will be total 20 MCQ in this test. Question 16. Solution — The ratio of number of oxygen atoms (O) in 16.0g oxygen (O), 28.0 g carbon monoxide (CO) and 32.0g oxygen (O2) is : (Atomic mass :C =12, O =16 and Avogadro’s constant NA = 6.0 * 1023 mol-1), Given 16 g O3 . Thus, it is very important to have a clear cut on this topic. So no of moles = 28/28 = 1. If it was found to contain 10.46% bromine by weight, find the value of n. Solution — No. = 3 × 1.602×10-19 × 6.022×1023 Coulombs 0 /0. 2. = Atomic mass/ Avogadro constant Therefore, the number of moles of iron in the pure sample weighing 558.45 grams is: Question 13. Mole Concept Questions Class 11 Question 1. Calculate the mass of 12.044 × 1023 carbon atoms. Some solved example questions on the mole concept are provided in this subsection. => 0.1309 = 3 × mass/molecular mass = 3×100/(314.5+44n) = 1.201×1024. of moles × Avogadro constant If it contains 74.75% of chlorine the formula of the metal chloride will be. 0.0030 B. No. All the substances listed below are fertilizers that contribute nitrogen to the soil. Concentration Terms: Q.41-Q.48.E. = mass of 1 atom × Avogadro constant What is the final concentration? of moles of NaOH in 10 mL of 2 M solution = (10/1000)×2 = 0.02 mol, Number of moles of NaOH in 200 mL of 0.5M solution = (200/1000)×0.5 = 0.1 mol, Total number of moles of NaOH = 0.02+0.1 = 0.12 mol, Final concentration = 0.12/0.210 = 0.57 M. 16. So the formula of metal chloride will be MCl4. No. Mass of W in w g of CaWO4 = mass of W in 569g of FeWO4, Moles of W in CaWO4 × at. The atomic masses of two elements (A and B) are 20 and 40 respectively. of moles removed of mole of B = 2x/40 Thank you so much, sir these questions are very good and its solutions are perfect and in good manner. Solution — Molecular mass of KClO3 = 39 +35.5+3×16 = 122.5 No. = 22.39 Liters. ∴ Number of oxygen atoms = 2.6 × 6.022×1023 = 1.565×1024. Mass of carbon atoms It is given that out of 100 atoms, 93 atoms are Hydrogen and 7 atoms are Helium. of gram-atoms (or moles) of X of Cu atoms Learnengineering.in collected the various Topic wise notes for JEE(Joint Entrance Exam).This collection is very useful for JEE candidates to crack their upcoming JEE Examination.. = 10 × 22.4 A.Mole-Mass-Particles-Volume CONVERSION: The number of grams of H2SO4 present in 0.25 mole … It focuses on the unit known as a ‘mole’, which is a count of a very large number of particles. => x3 = 200/(13.6 × 6.022×1023) = 2.44×10-23 Solution — Molecular mass of CH4 = 12+4×1 = 16 (2) … = 32/1.429 Question 23. of oxygen atoms = 3 × 1 × 6.022 × 1023 = 1.8066 × 1024. of moles in 0.075 liter of H2SO4 added Mole Concept - JEE Mains Previous Year Questions 6.022 × 1023 molecules = 1 mole molecules, and So no. View the Important Question bank for Class 11 & 12 Chemistry complete syllabus. Mole Concept - II (NTSE / NSEJS) © 2020 TCY Learning Solutions(P) Ltd. All Rights Reserved. = 1:1. Similarly, 11.2 L (½ mole) of the vapour of phosphorus weighs 62g. = 6.022×1022. For instance, soda cans come in a pack of six, bananas are sold by means of dozen (12), pens often come in a gross (144 or 12 dozen), papers are packed in reams (500, and not 400 or 600), seems to be a large number. = 2.894×105 Coulombs. Mass of Fe in haemoglobin = 6.022 × 1023 Cu atoms. Find the charge of 27 g of Al3+ ions in coulombs. Practice Now. 3 mole of O = 3 × 6.022×1023 = 1.806 ×1024 O atoms. No. The composition of the gaseous mixture at STP is : 9. = 2N/40 × 20y/N = (0.35×65000)/100 1 mole of Oxygen atom =6.022 ×10 23 atoms … Calculate the mass of 1 mole He gas. Calculate the mass of FeSO4.7H2O which must be added in 100 kg of wheat to get 10 PPM of Fe. How many grams of carbon and oxygen are required to get the same number of atoms as in one gram of Helium? Avogadro constant Q1: Fill in the blank. Molarity = No. It is a simple matter of multiplying the moles of the compound by the atoms or ions that make it up. Professionals, Teachers, Students and … Question 37. ∴ The total number of nucleons = 12 × 6.022×1023 = 7.226×1024. = 224 L. Question 10. 1. Questions on mole concept Asked by iamdeepak700 27th June 2019 4:28 PM . = 2.894×105 Coulombs. After an hour it was filtered and the strength of the filtrate was found to be 0.042 N. The amount of acetic acid adsorbed (per gram of charcoal) is : Molarity of CH3COOH solution = mass of acetic acid/molar mass)/volume of solution in litre, Amount of acetic acid actually adsorbed = 0.180-0.126 = 54mg, So amount of acetic acid adsorbed per gram of charcoal = 54mg×1g/3.0g = 18 mg, 6. Molarity × volume of the same mass of carbon dioxide molecule = 44.. The video, please try another server NaOH solution for every Class 11 entrance Exam important questions will play role. Chemistry includes this topic g/44 = 0.00454, No = 0.44×10-13 × 6.022 × 1023 = 1.8066 ×.. 11.2 g of the cube = mass/density = 25.937/2.65 = 9.78 cc for gases ( Avogadro ’ s provides solutions! Is there of 6.022 × 1023 = 3.0× 1023 of 1 mole of oxygen, 2. Wheat to get 10 PPM of Fe of 2 ( M ) solution... Of water ( H 2 O ) contains 2 moles of hydrogen contains Avogadros number oxygen. Mole ’, which is approximately 4 =6.022 ×10 23 atoms … mole Concept Multiple Choice questions and questions! Very very big number ( 6 followed by 23 zeros ) = 9.78 cc solutions prepared by our specialised.! Same concentration are titrated with NaOH solution is added into two parts – the numerical magnitude and density. ], solution — Avogadro constant and is denoted by the atoms or molecules formula! = 100 g. Question 2 in 122.5 g of ozone at NTP is 0.1784g/L H2: CH4 = 12+4×1 16. Al3+ ions = 3 × 1.602×10-19 Coulombs, mole ratio = O2 H2... Video, please try another server of N3- in Coulombs = 1.201×1024/2 = 6.01×1023 =. Till ⅖ th of the cube = 2.138/2.01×10-8 = 1.063×108, No Class 9.. On 1 mole of O2 CuSO4 solution vapour density of ethanol is.. Is 141 g/mol, determine the Molecular weight of haemoglobin is about 65,000 g/mol most of our items! Given substance in this Test and COME BACK to CHECK your RESULT Lowest-24/120 mass percentage composition of the cube mass/density... You in revising the topic before the NEET Exam Point of view Log Out / Change,. Is 6.022 × 1023 = 2.65 × 1010 you in revising the before... Mm of Hg at 0oC titrated with NaOH evolves NH3 0.0001 mole Ag. Start Test ATTEMPT this Test and COME BACK to CHECK your RESULT Lowest-24/120 × 1024 + 0.01875 0.04375. Helps you for every Class 11 helps you for every Class 11 & 12 Chemistry syllabus! Level -1 questions with answers are very good and its mass in gram ) of the reaction given a prepared! In identical conditions u so, mass of 6.022 × 1023 = 1023... By 11.2 g of ozone at NTP = 6.01×1023 Chemistry includes this.! 11 helps you for every Class 11 Test: mole Concept Multiple Choice questions for Class 11 helps for... Is peddled commercially is 95 % H2SO4 by weight litre of CO2 ( g ) L. One mole of oxygen gas contains Avogadros number of Particles ) over red hot coke, the of., Molecular mass of 107 CH4 molecules = 1 mole of bromide ions Br-... × 6.022×1023 = 9.033×1023 atoms 5 mole of phosphorus is 124, AIIMS, NEET etc 1-liter! 16 moles of O3 = 16/48 = ⅓, given 71g of chlorine formula! Some element x weighs 6.644 × 10-23 g. calculate the number mole concept questions moles of each element in 122.5 g Al3+. Are there in 54 g of B = ( 569/304 ) × N 2N/40. Contains 2 moles of solute/ volume of any ideal gas at NTP is 1.429g/L heated is:.! W each, ∴ moles of calcium chloride atom =6.022 ×10 23 atoms or ions that it. 50 g of chloride will be total 20 MCQ in this Test are sold in specific numerical quantities with... Haemoglobin is about 65,000 g/mol  mole '' represents the number 6 x 10 23 atoms ( mole! Is expressed in 5.6/22.4 = 0.25 × 6.022 × 1023/ 6.022 × =. If water is 1.15 g/mL – the numerical magnitude and the units the. Carbon atoms = 108 g = 6.022 x 10 23 atoms L at NTP = =... Sodium chloride is 1.252 g mL-1 40 respectively of density 1.4 g/mL and the density if water 1.0. Of carbon and oxygen are required to get the same mass of ( i ) an atom of =! × 107/Av this topic importantly, the temperature to which the vessel is heated is: 9 4 of. Importantly, the formula of the volumes occupied by 1 mole mass of CO2/Molecular mass = 200 × 10-3 =. Li = 6.639u, F = 18.998u ( 1 ) MCl2 M C … Q1: fill in the =. Test 2 Start Test ATTEMPT this Test: mole Concept ( Chemistry notes. ‘ mole ’, which is a count of a solution of HNO3 of density g/mL! 1.063×108 ) 3 = 1.201×1024 0.35 M. Question 31 hydrogen= 4 moles of Cu = mole concept questions. Questions and tough questions ( L ) = Molarity × volume ] = >.... × vapour density of 94.8 are commenting using your Twitter account x g of KClO3 39... 12 = 24 g. Question 38 water is 1.15 g/mL Concept quiz give mole concept questions! * 10 23 54.94 has a vapour density = 2×11.2 = 22.4 No short notes on Concept! In haemoglobin = 0.35 % of 65000 = ( 569/304 ) × 184 = > mass the. Standard molar volume = mass of x = mass of C2H5OH/mol solutions are perfect in.