of laboratory assignment 3 was to measure the rate at which a chemical reaction takes place. For the purpose of this lab we measured the rate a balanced oxidation/reduction reaction between iodine‚ hydrogen‚ and bromate ion occurs. The above reaction occurs slowly so we used a coupled iodine clock reaction to measure the rate of the oxidation/reduction reaction because it occurs much faster but is still dependent upon the other reaction. To accomplish this‚ two mixtures were prepared in separate
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bDATES PERFORMED: JANUARY 8‚ 2013 CHEMICAL EQUILIBRIUM D.M. TAN1 AND P.B. ALEGRO2 1DEPARTMENT OF MINING‚ METALLURGICAL‚ AND MATERIALS ENGINEERING‚ COLLEGE OF ENGINEERING 2 INSTITUTE OF CHEMISTRY‚ COLLEGE OF SCIENCE UNIVERSITY OF THE PHILIPPINES‚ DILIMAN QUEZON CITY‚ PHILIPPINES RECEIVED JANUARY 15‚ 2013 RESULTS AND DISCUSSION A. Iron- Silver Equilibrium The first part of the experimentation focuses in the iron-silver system. Silver nitrate (AgNO3) was added to ferrous
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CHEMISTRY 1 (FSC 1114) CHEMICAL BONDING MOKAN A/L VELAN (SCPNG0000019030) SANDEEP SINGH JASPREET SINGH TABLE OF CONTENT Contents IONIC BOND 2 METALLIC BOND 9 The "Sea of Electrons" Theory 14 Conductors‚ Insulators and Semiconductors 16 25 IONIC BOND Ionic bond is formed when electron transferred from a valence shell of an atom to the valence shell of another atom. Ionic bond involves electron transfer across two atoms. The atom which donates the electron is called cation
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2.MATERIALS and METHODS 2.1. Nature of Reactants 2.1.1 We placed 3mL of 3 M HCl into each of 3 seperate test tubes. Next we added mossy zinc to the first test tubes‚ Sn granules to the second and Cu filings to the third and compared the rates of evolution of hydrogen gas in each test tube. 2.1.2. We mixed 3mL of 0.02 M KMnO4 and 2mL of 3 M H2SO4 in a test tube and stirred using a glass rod. Next‚ we divided the solution into two. We added 2mL of 0.03 M Na2C2O4 solution to the first half and
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this reaction at 25(C. A. 1020 kJ/mol B. -1.22 ( 103 kJ/mol C. 2.00 ( 103 kJ/mol D. -1.42 ( 103 kJ/mol E. -198 kJ/mol 2. For the reaction H2(g) + S(s) ( H2S(g)‚ (H( = -20.2 kJ/mol and (S( = +43.1 J/K·mol. Which of these statements is true? A. The reaction is only spontaneous at low temperatures. B. The reaction is spontaneous at all temperatures. C. (G( becomes less favorable as temperature increases. D. The reaction is spontaneous
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Grade 10 Science –Chemistry Ionic Compounds Science Perspectives 10 - Section 5.6 Pages 192-195 Compound • A Pure Substance composed of two or more elements in a FIXED RATIO Ionic Compound • A compound made up of one or more positive metal ions (cations) and one or more negative non-metal ions (anions) Ionic Bond • The simultaneous strong attraction of positive and negative ions in an ionic compound. As noted‚ ionic bonding occurs between metals and non-metals. Yet‚ “why
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effect of changing temperature on the amount of solutet will dissolve in a given amount of water. In this experiment‚ you will completely dissolve different quantities of potassium nitrate‚ KNO3‚ in the same volume of water at a high temperature. As each solution cools‚ you will monitor temperature using a computer-interfaced Temperature Probe and observe the precise instant that solid crystals start to form. At this moment‚ the solution is saturated and contains the maximum amount of solute at that
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Physical and Chemical Reactions Lab #4 Alesa Cannon Objective: To investigate the physical and chemical properties of a pure chemical substance. Procedure: 1. Half-fill one well of a 24-well plate with 6 M HCl and half-fill a second well of the 24-well plate with 6 M NaOH. Suck up these chemicals into their labeled pipets for later use. 2. Perform the following steps on each of the substances to be tested. Complete all tests of one substance and record your observations before proceeding
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stops. The equivalence point is when the H+ ions are neutralized by OH- ions‚ which occurs when both are used up in the reaction causing the pH to be 7. The molarity of NaOH from the indicator was exactly .500 M‚ but the molarity for the equivalence point from the second derivative was .688 M. This resulted in a range of roughly 27.3%‚ which is way over the 15% error mark of each other. This may have occurred due to the
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The speed of chemical reactions – class experiment By Julia Shuker Year 10 science – Miss Phillips – Term 2 – 2013 – Julia Shuker Aim The aim of the experiment was to investigate the factors that increased or decreased the speed of chemical reactions between two different chemical reactions. Hypothesis If certain factors‚ such as concentration‚ temperature‚ catalyst and surface area are increased then the reaction rate will also increase due to the particles
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