Chapter Exercise 33 Chapter 34 Importance of redox reactions in modern ways of living Class Practice 36 Chapter Exercise 37 Part Exercise 39 Chapter 35 Energy changes in chemical reactions Class Practice 42 Chapter Exercise 43 Chapter 36 Standard enthalpy change of combustion‚ neutralization‚ solution and formation Class Practice 44 Chapter Exercise 46 Chapter 37 Hess’s Law Class Practice 48 Chapter Exercise 51 Part Exercise 53 Chapter 25 Simple molecular substances with non-octet structures and
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Abstract: The purpose of this experiment was to determine the concentration of an unknown amount of copper sulfate using the spectronic 20. Four solutions of different concentrations of H₂O and CuSO₄ were put into the spectronic 20 to observe their absorption of light. Then‚ a graph was created to plot down the measurements. Using the calibration curve of the graph‚ the concentration of the unknown substance was found out to be .12M. Background/Introduction: Beer’s law (which states that
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complexes will be compared by the color each reflects and by the energy of the waves each absorbs. The purity of the synthesized complex will also be found. Procedure Part I: Preparation of the Complex A sample of copper sulfate pentahydrate (6.285g) was weighed out. The copper sulfate pentahydrate was dissolved in water (11.99mL) in a 250mL beaker. The solution was heated on a hot plate to 90 degrees Celsius. A sample of potassium oxalate monohydrate (10.006g) was dissolved in water (50.0mL).
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separate some light sources in to constituent colors and find out the wavelength of some atomic emissions. We will also try to compare the line spectra found from gas discharge tubes and flame emissions. Finally‚ we will measure the absorbance of Copper sulfate solution as a function of wavelength. Experimental Method: We start our experiment by looking through a Spectroscope at the outside sunlight‚ a regular light bulb (incandescent) and a fluorescent light. This will give us a good observation
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empirical formula for hydrated copper sulfate. In doing this lab‚ one was able to see the gradual change in the composition of a hydrate into an anhydrous salt. The lab was carried out with numerous steps. First‚ one had to safely prepare by putting on goggles. One then had to wash and heat the dish with the flame for about three minutes. After allowing the dish to cool‚ one had to weigh the evaporating dish and record the weight. Two to three grams of copper sulfate hydrate was then added to the
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B. K.‚ R. K. Shukla‚ and V.S Agashe‚ 1972). The Biuret test for protein was used to determine the presence of peptide bonds in proteins. The color of samples before was clear. Both sodium hydroxide and copper sulfate were clear color as well. When you added sodium hydroxide and copper sulfate into the samples‚ protein would turn into purple. The structure of proteins was form by the
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energy than the reactants Enthalpy changes are normally quoted at standard conditions. Standard conditions are : • 1 atm pressure • 298 K (room temperature or 25oC) • Solutions at 1mol dm-3 • all substances should have their normal state at 298K Standard enthalpy change of formation In an exothermic reaction the ∆H is negative In an endothermic reaction the ∆H is positive When an enthalpy change is measured at standard conditions the symbol is used Eg ∆H The enthalpy of formation of an element
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anode | Glucose (C6H12O6) | No | Nothing changes | Nothing changes | Dilute Sulfuric Acid (H2So4) | Yes | Bubbles | Bigger bubbles | Sucrose (C12H22O11) | Yes | Light bubbles | Light but more visible bubbles and light brown liquid | Copper Sulfate (CuSo4) | Yes | Light bubbles | Changes color to brown and oxidation is observed | Ethanol (c2H5OH) | No | Nothing changes | Nothing changes | Calcium Hydroxide (Ca(OH)2) | Yes | Light bubbles | Light bubbles but more than in anode |
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(l) Water is added to make a pumpable slurry. Flotation (separation of valuable content) Cu2S(s) + H20 (l) CaCO3(s) (added to give a basic PH level) pine oil or C2H5OH (liquid called a frother) C3H5KOS2 (potassium amyl xanthate to make the copper particles cling to the bubbles as they rise to the surface) O2 (pumped into bottom of tank‚ agitates soloution and starts to froth‚ bringing bubbles to the surface) Cu2S particles adhere to the bubbles‚ which is separated from the liquid‚ tailings
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Copper (II) Sulfate Purpose: The purpose of this lab is to find out how many moles of water there are in one mole of Copper Sulfate (CuSO x HO) and the percent by mass of water in the hydrate. This will be accomplished by heating a determined mass of the hydrate to remove the water‚ and by measuring the salt left over. Introduction: This laboratory experiment will be done to find out how many moles of HO are present per one mole in the hydrate CuSO. A hydrate is a compound that has a fixed number
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