the heating process‚ the finer grains were also turned to light yellowish-green. Processed Data Calculation needed: In order to find ‘’ in the formula CuSO4.H2O‚ we need to find the ratio of mole between anhydrous copper II sulfate and the water vapour by using the formula: In this case‚ the molar mass of: Copper II sulfate (CuSO4) is: 63.55 + 32.06 + 15.99 x 4 = 159.57 g/mol Water (H2O) is: 1.01 x 2 + 15.99 = 18.01 g/mol (e.g. 0.37/18.01= 0.02054 mol.) Then‚ is obtained by: Calculation
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Part I: Properties of Hydrates 1.Place about 0.1 g of the following compounds in each one test tube: CuSO45 H2O‚ CoCl26 H2O‚ NiCl26 H2O‚ and KAl(SO4)212 H2O. 2. Heat each test tube gently over a Bunsen burner flame and record your observations in your notebook. 3. After the sample has cooled‚ add a few drops of deionized water. What happens and
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measure the cell potential (E˚cell) between various 1.0 M aqueous reactant solutions‚ then using balanced half-cell rxns‚ calculate theoretical cell potential values and compare to experimental. Part B: Concentration Cell: Measure the cell potential of CuSO4 (aq) of two differing Molarities – one concentrated and one dilute- then use the Nernst equation to determine the theoretical cell potential ‚ comparing to experimental. Part C: Electrolytic Cells- use an external source of electricity to drive the
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distillation Two liquids – immiscible liquids using a separating funnel - fractional distillation due to different boiling points H/W – P.18 Qu. 11-18 Identifying Pure Substances Colour – some substances have a characteristic colour‚ eg CuSO4 = blue. We can use this knowledge in a qualitative way to determine if a sample has impurities. Melting & Boiling Point – The mp & bp of a substance is a good indicator of its purity. A pure substance will have a sharp melting point and its mp &
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name. Its molecular structure is shown below. The water that is chemically combined into their structure is called the water of crystallisation. In our experiment the crystal hydrate is heated‚ this is an endothermic reaction CuSO4.XH2O (bright blue solid) → CuSO4 (dirty white solid) + 5H2O After enough heat has been added to break the bonds‚ the water of crystallisation is then released in the form of water vapour. When the water has been removed‚ the Copper Sulphate crystals will then be
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PUTTING IT TOGETHER: Classifying Chemical Reactions Purpose: To observe and differentiate between the four different types of chemical reactions. Variables: The independent variables are the sodium chloride‚ sodium carbonate‚ magnesium‚copper‚ copper (11) sulfate‚ silver nitrate‚ oxygen‚ lead(11) nitrate‚ sodium carbonate‚ copper (11) sulfate pentahydrate. The dependent variables are the chemical reactions that are being looked for. For example decomposition‚ synthesis‚ single displacement or double
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Copper Sulphate solution (CuSO4) in a measuring cylinder‚ for precise accuracy‚ and then pour the solution into test tube. I will place the test tube into a beaker and insulate the test tube‚ for minimum heat loss. (As shown in the diagram above.) 2.Secondly I will measure the required amount of Zinc (Zn) on a weighing scale‚ again for precise accuracy. I will then measure the starting temperature using a thermometer. Next I will pour the Zinc into the test tube containing CuSO4. 3.Finally I will measure
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the following equations. A. CuSO4 + Fe Cu + FeSO4 B. 3CuSO4 + 2Fe 3Cu + Fe(SO4)3 2. If Iron (III) Sulfate were formed‚ what mass of Copper would be expected and what is the limiting reagent? C. 2.26 g Cu D. Fe 3. If Iron (II) Sulfate were formed‚ what mass of Copper would be expected and what is the limiting reagent? E. 2.8 g Cu F. CuSO4 Driving Question: What compound is formed when you add 7 g of CuSO4 to 2 g of Fe? Goal: To correctly identify
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Chemistry F332 Notes Ions in solids and solutions: Structure of an ionic lattice (Sodium Chloride): * Consists of sodium ions (Na+) surrounded by six chloride ions (Cl-) * Chloride ions also surrounded by six sodium ions. * Held together by attraction of oppositely charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals
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the ratios are exactly one‚ but the ratios are fairly consistent. Calculation 4: Determination of the half-cell potential for the ferri/ferrocyanide couple in 1.0M KNO3 from the 10mV/s scan rate graph E_(1/2)=(E_pa+E_pc)/2=(331mV+201mV)/2=266mV According to the lab handout the literature half- cell potential for ferricyanide in 0.1M KNO3 is 424mV versus the NHE reference electrode. This is 225 mV versus the Ag|AgCl in saturated KCl reference electrode used in this experiment. (Value calculated with
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