Balancing Equations Balancing equations is a fundamental skill in Chemistry. Solving a system of linear equations is a fundamental skill in Algebra. Remarkably‚ these two field specialties are intrinsically and inherently linked. 2 + O2 ----> H2OA. This is not a difficult task and can easily be accomplished using some basic problem solving skills. In fact‚ what follows is a chemistry text’s explanation of the situation: Taken from: Chemistry Wilberham‚ Staley‚ Simpson‚ Matta Addison Wesley
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Experiment 5 Determination of Empirical Formulas of Hydrate and Oxide Compounds Room #216 Locker# 1137 Date of Experiment: May 11‚ 2014 Date of Submission: May 16‚ 2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass
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Purpose The purpose of this lab is to identify the different features that come about by using oxidation reduction and recording the observations‚ these tests will help determine the specific qualities each solution has. Hypothesis I theorize that nothing will happen with Magnesium because it is such a soft metal. Zinc should turn a greener color‚ because that’s what happens to a lot of statues and sculptures. I theorize that iron will tarnish badly because in air it can get tarnished so oxidation
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SYNTHESIS AND CHEMISTRY OF K2S2O8 ABSTRACT In this experiment‚ a sample of K2S2O8 was prepared by the electrolysis of an aqueous solution of H2SO4 and K2SO4. The peroxodisulfate anion‚ S2O82-‚ was also observed for its ability to serve as a counterion for precipitation by preparing a copper (II) complex by reacting hydrated copper (II) sulfate with ammonium peroxodisulfate in the presence of pyridine. This same ability‚ coupled with its strong oxidizing ability allowed for stabilization of
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Writing Complete Equations Practice For each of the following problems‚ write complete chemical equations to describe the chemical process taking place. Important note: There are a few physical processes on this sheet – You can’t write an equation for a physical process! 1) When lithium hydroxide pellets are added to a solution of sulfuric acid (dihydrogen sulfate)‚ lithium sulfate and water are formed. 2) When dirty water is boiled for purification purposes‚ the temperature is brought up to
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brown and separates into small strands of brown liquid within the clear liquid. Heterogeneous| K.|AgNO3 + NH3||Slight bubbling‚ clear liquid. Heterogeneous| |after exposure to bright light||Bubbling intensifies and color remains clear. | L.|NH3 and CuSO4||Pale blue color. Extremely small and light blue solids at the bottom of the solution. Heterogeneous| Part F: Testing of Various Foods with the NaOCl + KI solution Foods|Presence or Absence of Starch| Chocolate pudding|No reaction| Chocolate
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Osmosis is the diffusion of a solvent across a selectively permeable membrane that occurs in response to differences in solute concentrations (Allen and Harper 2014).Osmosis can fall under the category of passive transport which does not require energy. With osmosis being a type of diffusion it is viewed as molecules moving from a high concentration to a low concentration. To further explain if there is a low water concentration‚ high amounts of solutes will be present. Water will most likely move
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Electrolysis a) Electrolysis is the decomposition of a substance to give simpler substances. The substance being electrolysed has to be an ionic compound. b) The substance being decomposed is called the electrolyte. c) In electrolysis the electric current enters and leaves the electrolyte by conducting rods called electrodes. The positive electrode is called the anode and the negative electrode is called the cathode. d) For electrolysis to occur the electrolyte must be in liquid form so that
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Variation of Conductance with Temperature in Electrolytes Index 1.Certificate.................................................................3 2.Acknowledgements.....................................................4 3.Aim..........................................................................5 4.Apparatus..................................................................6 5.Important Terms........................................................7 6.Conductivity...
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boiling and carefully boil it to dryness. Note any color changes. 4. Put the evaporating dish on the lab bench and let it cool. C. Deliquescence and Efflorescence 1. Place a few crystals of Na2CO3 x 10H2O‚ CaCl2‚ KAl(SO4)2 x 12 H20‚ and CuSO4 in an a separate evaporating dish next to the CoCl2 prepared in part B. 2. To see weather the samples gained or lost mass‚ weigh each of them on a top-loading balance and record to the nearest hundredth. 3. Weight them again after an hour
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