1.9: Organic Chemistry: Alkanes Summary of Chapter. Elements: It is the simplest form of the matter. New York, N.Y. : Wiley, ©1981 (OCoLC)645884878: Material Type: LAWS OF CHEMICAL COMBINATIONS 3.1. with % ratio as . CONCENTRATION TERMS Molarity (M) : Number of moles present in one It of solution (mol/lt) w Molarity x 1000 m x V(ml) Example 8: 149 gm of potassium chloride (KCI) is dissolved in 10 Lt of an aqueous solution. • (i) Write the balanced chemical equation. If 50g of Ammonia gives 41.18g of Nitrogen, then the percentage of Nitrogen in ammonia 41.18 x 100 = 82.36%. Example : Different samples of carbon dioxide contain carbon and oxygen in the ratio of 3 : 8 by mass. Total mass of NaHC03 heated = 20 gms; Total mass Na2C03 produced = 12.62 gms Total mass of C02 produced = 5.24 gms . Chemistry relates to everything that can be sensed from the minute elements to complex structures. Mathematics, Physics, English, Chemistry, Mathemat... Chemistry - Redox Reactions and Electrochemistry. The ratio of weight of H and O in 1-120 is 1 : 8. 05/10/2019 07/10/2019 Chemistry ABC 0 Comments. About Chemistry ABC “ChemistryABC.com has always been very supportive of the Science community. i.e. Mass of substance = 0.5 g Mass of solvent = 25 g 0.5 . Calculate its empirical formula. 3 mole MOLE CONCEPT 98 2 atoms 2 x NA atoms 2 mole 6 mole s one atom 1 x NA atoms one mole 3 mole O 4 atoms 4 x NA atoms 4 mole 12 mole Mole means heap or collection of things. The carbon-hydrogen bonds are only very slightly polar. Anything which has mass and occupies space is called matter. 1.8: Cycloalkanes Many organic compounds have cyclic structures. Basic Concepts of Chemistry by 1 guider 1. (iii) Calculate the result by applying unitary method. Some Basic Concepts of Chemistry. Ancient Greek philosopher also believed that all matter was composed of tiny building blocks which were hard and indivisible. One mole of any chemical substance contains fixed no. 2 x vapour density (VD) = molecular mass of gas. As all objects in the universe are made of matter. w Also, N = n; 1 mol of N3- = 14 gm of N3- = 1 gm ion of N = No ions 1 w 1 >< n Example 3 : Solution : The molecular mass of H2S04 is 98 amu. (ii) Write the atomic mass/molecular mass/moles/molar volumes of the species involved in calculations. 21-12 2 vol. mass of solute in gm x 100 mass of solution in gm % weight by volume (w/v) : It is given as mass of solute present in per 100 ml of solution, i.e Example 10 : Solution i.e. Example 2: Solution: When 50 g of ammonia is heated it gives 41.18 g of Nitrogen. wt. Your IP: 185.246.67.47 Avogadro number = 6.023 x 1023 T-map: Interconversion of mole-volume,mass and number of particles Number Of — mol. Some Basic Concepts Of Chemistry. Or in other words volume of reacting gases and product gases have a simple numerical ratio to one another. Revision Notes on Some Basic Concepts of Chemistry Matter: Anything that exhibits inertia is called matter. SOME BASIC CONCEPTS OF CHEMISTRY Chemistry: Chemistry is the branch of science that deals with the composition, structure and properties of matter. 21-120 2 vol. The same is found to be true in H20 molecules. Chemistry also plays an important role in daily life. Uncertainties in Scientific Measurements 3. Mass of 1420 produced = 20—12.62—5.24 = 2.14 gms (b) The Law of Constant Composition or Definite Proportion (Proust in 1799) : This law states that " All pure samples of the same chemical compound contain the same elements combined in the same proportion by mass irrespective of the method of preparation". 1 mol of N2 = 28gm of N2 = 1 gm molecule of N2 = No molecule = 2 No atoms For ions N3-, CF no.of moles = n gmquantity m Atomic mass/molecular mass 1 mol of any gas contains fixed volume i.e: 22.4 It at NT P (OOC & 1 bar) weight (grams) Number of moles of a species = w Atomic or molecular mass (g/ mole) M Volume occupied by gas at NT P Number of moles of a gas = Avogadro's hypothesis : Volume occupied by 1 mole of the gas at NT P Equal volume of the gases have equal number of molecules ( not atoms) at same temperature and pressure condition. In this section, you will study about the important topics of the chapter, overview, formulae and some important tips and guidelines for the preparation of the chapter at the best. HOMOGENEOUS MIXTURES. Mass of KC103 volume of 02 at STP 3 x 22.41t 122.5 74.5 3 x 32 : 3 x 22.4 It at S.T.P. SOME BASIC CONCEPTS OF CHEMISTRY INTRODUCTION Anything that occupies space and has mass is called matter. Some Basic concepts of chemistry ⇒ 1 mole = 6.02 × 1023 particles = 1g. Chemistry is the science and study of matter, including its properties, composition as well as reactivity. Law Of Conservation Of Mass 3.2. of urea = 60) Mass of urea = 5 gm Molecular mass of urea = 60 5 Number of moles of urea = — 0.083 60 Mass of solvent = (255 — 5) = 250 gm Number of moles of solute Molality of the solution = x 1000 Mass of solvent in gram 0.083 x 1000 = 0.332 250 Mole Fraction (X) The ratio of number of moles of the solute or solvent present in the solution and the total number of moles present in the solution is known as the mole fraction of substance concerned. w n x no. How many grams of H20 is produced? Example 7: What volume of oxygen gas at NTP is necessary for complete combustion of 20 litre of propane measured at OOC and 760 mm pressure. molecular mass n empirical formula mass Molecular formula = (Empirical formula)n (iii) Molecular mass = mass of 22.41 of gas or vapour at S.T.P Example 4 : A substance, on analysis, gave the following percentage composition: Na = 43. Properties of Matter 2.1. You may need to download version 2.0 now from the Chrome Web Store. wt — At. For each approved study note you will get 25 Credit Points and 25 Activity Score which will increase your profile visibility. mass, shape, size , different elements are different in nature. • :.wtof ethanol in 1000 ml = gm 1 OOOd Mol of ethanol = 46 IOOOd IOOOd Molarity 46 mol 1000 46 & molality of ethanol = kg 1000 46 Parts per million (ppm) —Amount of solute ( in g ) with 106 g solvent Parts per billion ( ppb) •amount of solute ( in g ) with 109 g solvent Example 9 : Solution : 255 gm of an aqueous solution contains 5 gm of urea. Basic chemistry concepts and exercises. Here we have covered Important Questions on Some Basic Concepts of Chemistry for Class 11 Chemistry subject.. Chemistry Important Questions Class 11 are given below. Performance & security by Cloudflare, Please complete the security check to access. Matters exist in three physical states viz. Class XI Chapter 1 – Some Basic Concepts of Chemistry Chemistry Question 1.1: Calculate the molecular mass of the following: (i) H2O (ii) CO2 (iii) CH4 Answer (i) H2O: The molecular mass of water, H2O = (2 × Atomic mass of hydrogen) + (1 × Atomic mass of oxygen) = [2(1.0084) + 1(16.00 u)] = 2.016 u + 16.00 u = 18.016 = … Let number of moles of solute in solution Number of moles of solvent in solution = N n Mole fraction of solute (Xi ) Mole fraction of solvent (X2) Also Xl + = 1 Mole fraction is a pure number. I'm sure after learning these, you might become a fan of Chemistry. The study of chemists is always interested in identifying and knowing how the chemical transformation occurs. HETEROGENEOUS MIXTURES. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The quantity of matter is its mass. Basic Concepts from Organic Chemistry (PDF 103p) This note covers the following topics: Aliphatic Compounds, Hydrocarbons, Alcohols, Aldehydes And Ketones, Acids, Esters, Ethers, Alkyl Halides And Other Halogenated Aliphatic Compounds, Simple Compounds Containing Nitrogen, Cyclic Aliphatic Compounds, Mercaptans Or Thioalcohols, Aromatic Compounds, Hydrocarbons and Phenols. Additional Physical Format: Online version: Malone, Leo J., 1938-Basic concepts of chemistry. Atoms cannot be created or destroyed by any chemical process. GCSE Chemistry Key concepts in chemistry learning resources for adults, children, parents and teachers. Are you one of those who loves Chemistry? x 100-1.96 mass of solute in gm x 100 volume of solution in ml Volume of solute in ml x 100 Volume of solution in ml 0.5 g of a substance is dissolved in 25 g of a solvent. That's great! For any balanced chemical reaction mass of reactant is equal to mass of products. Pure ethanol : d gm/ml (density of ethanol) (C2H50H) let volume of ethanol taken be 1000 ml. Gram Molecular Mass : The molecular mass of a substance expressed in gram is called the gram-molecular mass of the substance. Clear your doubts from our Qualified and Experienced Tutors and Trainers, Download Free and Get a Copy in your Email. were never put to latter on which was etc. Normality of solution = n x molarity of solution Concept of minimum molecular mass : Ax 1 00 Minimum molecular mass A = Atomic mass percentage of element Some Basic units % wt or w/w gm quantity of solute present 100gm of solution % by v or v/v volume of solute present in 100 ml of solution w/v gm quantity of solute present in 1000ml of solution its unit is gm/lt. Calculate the percentage amount of the substance in the solution. 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