Stoichiometry • Calculations involving quantities of consumed reactants and formed products based on a BALANCED chemical equation. Mass Molar Mass Mole Coeff Bal Eqn Mole Molar Mass Mass Example 2 • The Haber Process involves reacting gaseous nitrogen and gaseous hydrogen to form ammonia. Determine the mass in grams of hydrogen gas required to form 1.00 x 103 g ammonia. Your Turn 2 • If you react 52.9 g of potassium chlorate (KClO3) with excess phosphorus
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Chemistry 2202 Review Final Exam Chapter 2: The Mole 1. Isotope – atoms of an element that have the same number of protons but different numbers of neutrons. Ex. The three forms of oxygen are called oxygen-16‚ oxygen-17‚ and oxygen-18. They all have 8 electrons and are written as 16/8 O (8 protons + 8 neutrons)‚ 17/8 O (8 protons + 9 neutrons)‚ and 18/8 O (8 protons + 10 neutrons). 2. 3. Mass Number – the sum of the protons and neutrons in the nucleus of one atom of a particular
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by the smallest number mole to reduce the decimals 3) If not whole numbers yet‚ multiply by some special factors to reduce decimals 1.25 x ¼ = 1 Al2(SO4)3 + 3 Cu : 2:3:1:3 ratio To determine amounts‚ use ratio and plug in numbers correctly Limiting/excess reactants Limiting:Reactants that are not completely used up in a reaction When this reactant is used up‚ the reaction stops Excess
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the elements. This arrangement of elements in the order of increasing atomic number with the elements having similar properties placed in vertical columns is known as periodic table. MATERIALS/REAGENTS AND EXPERIMENTAL PROCEDURE For the Group IA & IIA Elements‚ each small amount samples ofLi2CO3‚ Na2CO3‚ K2CO3‚ MgCO3‚ CaCO3 and BaCO3 was place in the different test tubes. After placing them in the test tubes‚ we identified the physical state‚ color‚ and appearance of each. Then we test the solubility
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Name: __________________________________ Teacher: ________________________________ DO NOT OPEN THE EXAMINATION PAPER UNTIL YOU ARE TOLD BY THE SUPERVISOR TO BEGIN Chemistry 2202 FINAL EXAMINATION June 2010 Value: 100% General Instructions This examination consists of two parts. Both parts are contained in this booklet and further general instructions are provided on appropriate pages. Part I – Multiple Choice (40%) Select the letter of the correct response from those provided. EITHER
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As the reaction was to set up to produce a Grignard reagent and then recrystallize it to obtain pure sample. The percentage yield obtained was 55% and its melting point was 161 co which is within the literature value 160-163 co. In addition to that the IR spectroscopy confirmed the molecule structure to be triphenylmethanol. Introduction: The Grignard reagents are alkyl magnesium halides‚ R-Mg-X were first introduced in 1900. These reagents are usually prepared by reacting one atom with one molecule
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These procedures are dependent on gravimetric analysis (the most accurate and reliable procedures). Important requirements for a successful gravimetric analysis include: a pure compound with an identifiable stoichiometry‚ the precipitation reaction must be complete‚ specificity of precipitation reagent in sample‚ the solid sample should be a reasonable-sized crystal‚ and the molecular weight should be reasonable enough for a good weight of the precipitate generated. For the full formation of the precipitate
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from complex mixtures. By isolating a protein‚ one will able to study its properties in detail and therefore be able to pinpoint which protein is responsible for a certain biological activity. Purified proteins also serve as valuable biochemical reagents. [2] Gluten – a protein composite most commonly found in wheat – possesses a unique property that allows it to be processed into bread and a variety of other foodstuffs. It is the ingredient responsible for adding texture and chewiness in baked
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Appendix APPENDIX 1 Chemical tests for functional groups Homologous series/ Typical compound Functional group(s) Alkanes CH3CH3 ethane C – C and C–H Alkenes CH2 = CH2 ethene C=C Chemical tests/Observations Add liquid bromine in ultraviolet light (or sunlight): White fumes of HBr liberated; decolourisation of bromine occurs slowly (a) Add Br2 in CCl4 at room temperature: Decolourisation of bromine occurs immediately CH2 = CH2 + Br2 → CH2BrCH2Br (b) Add acidified
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1 SOME BASIC CONCEPTS OF CHEMISTRY 1 UNIT 1 SOME BASIC CONCEPTS OF CHEMISTRY After studying this unit‚ you will be able to • understand and appreciate the role of chemistry in different spheres of life; • explain the characteristics of three states of matter; • classify different substances into elements‚ compounds and mixtures; • define SI base units and list some commonly used prefixes; • use scientific notations and perform simple mathematical operations on numbers;
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