Periodicity Engr. Imelda Galera De La Salle University-Dasmariñas Dasmariñas‚ Cavite Philippines ABSTRACT Chemical periodicity was demonstrated using different samples of elements from Group IA‚ IIA and IVA. These samples are: Li2CO3‚ Na2CO3‚ K2CO3‚ MgCO3‚ CaCO3‚ BaCO3‚ Carbon‚ Tin‚ Silicon and Lead. Each sample was placed in a test tube‚ (one sample and one test tube) and the physical color‚ appearance and state was defined. Water was used to test the solubility of the element. We use
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Na2C03 x 106 g Na2C03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol Na2C03 Using 1 g of CaCl2·2H2O and .72 or .8 g (slight excess) Na2CO3 Should give a CaCO3 theoretical yield as follows: 1 g CaCl2·2H2O x 1 mole CaCl2·2H2O x 1 mol CaC03 x 100 g CaC03 = 147 g CaCl2·2H2O 1 mol CaCl2·2H2O 1 mol CaC03 To double-check‚ we can calculate CaCO3 theoretical yield by using Na2CO3 0.72 g Na2C03 x 1 mol Na2C03 x 1 mol CaC03 x 100 g CaC03 = 106 g Na2C03 1 mol Na2C03 1 mol CaC03 www.LabPaq.com 56 ©Hands-On
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the Stoichiometry Challenge Lab we compared the theoretical results of the reaction between sodium carbonate (Na2CO3) and sulfuric acid (H2SO4) with the actual data we found. I hypothesised that If the mole ratio between Na2SO4 and H2SO4 is 1:1 then when I react 0.5 grams of Na2SO4 (reactant with H2SO4) I should get 0.669 grams of Na2SO4. The actual reaction between .05 grams of Na2CO3 and 5 mL of of H2SO4 produced 0.79g of Na2SO4. When I were testing the reaction‚ I measured out the reactants
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Module 4: 10. Strong Bases: NaOH‚ KOH‚ Na2CO3‚ NaHCO3‚ Na3PO4‚ NaHPO4‚ Strong Acids: Fe(NO3)3‚ HCL‚ HNO3‚ Al(NO3)3‚ NiCl2‚ H2SO4 11. Acidic Neutral Basic NaCl KNO3 NaOH HC2H3O2 Na2CO3 NaC2H3O2 NaHCO3 Fe(NO3)3 NaNO3 Na3PO4 HCl MgSO4 KOH HNO3 Na2SO4 NaHPO4 CuSO4 NaNO2 CoCl2 Al(NO3)3 NiCl2 H2SO4 KCl NH4Cl 12. CuSO4 CuCO3.Cu(OH)2(s) + 2 H2SO4(aq) ----> 2 CuSO4(aq) + CO2(g) + 3 H2O(l) Na3PO4 Na3PO4 (aq) + 3H2O (l) --> H3PO4 (aq) + 3NaOH
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the product in for each mole. We divided this to find out how many grams of reactant for every one gram of product‚ and finally multiplied this by two. Our final results were lower than the desired 2.00 grams. Balanced Equation: CaCl2 X 2H2O + Na2CO3 x H2O → CaCO3 + 2NaCl + 3H2O Background Information: We chose Calcium Chloride dihydrate because it is soluble in water‚ not very expensive and only mildly toxic (LD50 1000mg/kg). In addition we chose Sodium Carbonate because it is soluble in
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Repeat steps 2-5 using the Sodium Carbonate. Tabulate results in table below. COMPOUNDS REACTION TIME/MINS AMOUNT OF GAS COLLECTED Calcium Carbonate Sodium Carbonate VARIABLES: 1. Control: Masses of Ca(Co3)2 and Na2Co3‚ Vol. of HCL and Conc. Of HCL. 2. Manipulated: Carbonates 3. Responding: Gas Evolution EXPECTED RESULTS: It is expected that Calcium Carbonate
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Experiment 3: Stoichiometry of a Precipitation Reaction Abstract: In this experiment‚ the objective is to use Stoichiometry to predict the amount of product produced in a precipitation reaction. We received working knowledge of how to accurately measure reactants and products of the reaction. We then are able to use the data that we recorded to make assessments of the actual yield opposed to the theoretical yield. When we calculated the percent yield we are able
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carbon dioxide Purpose: The purpose of the practical that we completed was to determine the molar mass of carbon dioxide (CO2) by experimental means and to observe the reaction of hydrochloric acid and sodium carbonate. Using the balanced equation: Na2CO3 + 2HCl → 2NaCl + H2O + CO2 Materials / Apparatus: 1) 8.00g of sodium carbonate‚ 2) 30mL of hydrochloric acid (6molL-1) 3) 100mL of hydrochloric acid (6molL-1) 4) 100mL conical flask‚ 5) 150mL glass beaker 6) 50mL glass beaker 7) Glass funnel‚ 8)
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EXPERIMENT-1 CHEMICAL REACTIONS AIM: To perform and observe the following reactions and classify them into: (i) Combination reaction (action of water on quick lime) (ii) Decomposition reaction (action of heat on ferrous sulphate crystals) (iii) Displacement reaction (iron nails kept in copper sulphate solution) (vi)Double decomposition reaction (reaction between sodium sulphate and barium chloride) APPARATUS REQUIRED: 1. A rack of at least six clean test tubes and a boiling
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mixture * Folding the filter paper * Pouring the reaction mixture into the filter paper in the funnel * Placing the product on the paper towels to dry Experimental Step | Observations | Mass of CaCl2•2 H2O used (grams) | | Mass of Na2CO3 used (grams) | | Net mass of mixture‚ grams | | Appearance of mixture when the reactants are mixed together | | Mass of filter paper (grams) | | Appearance of dry product | | Mass of filter paper and dry product (grams) | | Mass
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