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# experiment 1: determining the chemical formula for copper gluconate

Calculate the % of copper in copper sulphate, CuSO 4; Relative atomic masses: Cu = 64, S = 32 and O = 16; relative formula mass = 64 + 32 + (4x16) = 160; only one copper atom of relative atomic mass 64 % Cu = 100 x 64 / 160 = 40% copper by mass in the compound Then, the gas is tested with a lighted wooden splinter. The empirical formula of magnesium oxide, Mg x O y, is written as the lowest whole-number ratio between the moles of Mg used and moles of O consumed.This is found by determining the moles of Mg and O in the product; divide each value by the smaller number; and, multiply the resulting values by small whole numbers (up to … Search results for copper gluconate at Sigma-Aldrich. If you finish with 3.18 g Cu_2S, and 2.54 g of copper metal were used, the balance, the difference between the end mass and the mass of copper MUST be the mass of sulfur that reacted. If you don’t land exactly on 1.0, that’s OK. Just get as close as you can, and record the exact mass in Table 1 below. I don't understand how to find the formula mass for gluconate so that I can calculate the moles of gluconate in 1 gram of my copper gluconate. Because the ratios of the elements in the empirical formula must be expressed as small whole numbers, multiply both subscripts by 4, which gives C 5 H 4 as the empirical formula of naphthalene. Determine the chemical formula for Copper gluconate with the given information: Copper Gluconate: Cu(C6H11O?)? Let the mass of sulfur be 'x' gram. Shot by Paul J. Ramsey, Media Resources, Eastern Kentucky University. If the gas burns quietly without a "pop" sound, then all the air has been totally removed from the combustion tube. Copper gluconate has a chemical formula of C12H22CuO14. *Please select more than one item to compare An excess of sulfur ensures that all the copper reacts. 4. 14. The reduction of cupric to cuprous ion is fast. Formula Weight. formula mass corresponds to the molecular formula H 2 O 2. A. Rounded to the nearest integer, the ratio is 1:5. CHEM 1105 Experiment 7 1 EXPERIMENT 7 – Reaction Stoichiometry and Percent Yield INTRODUCTION Stoichiometry calculations are about calculating the amounts of substances that react and form in a chemical reaction. 2) You should be able to determine the empirical formula given the mass and identity of each element in a compound. Assay— Dissolve about 1.5g of Copper Gluconate,accurately weighed,in 100mLof water.Add 2mLof glacial acetic acid and 5g of potassium iodide,mix,and titrate with 0.1Nsodium thiosulfate VSto a light yellow color.Add 2g of ammonium thiocyanate,mix,add 3mLof starch TS,and continue titrating to a milk-white endpoint.Each mLof 0.1Nsodium thiosulfate is equivalent to 45.38mg of C 12 H 22 CuO 14. The typical dose is 2.0 mg copper per day. The ultimate goal is to find out the chemical formula of the compound as well as a few other things. The formation of the yellow material (Experiment 1) or copper sulfide (Experiment 2) is slow. There is .2g of copper within the copper gluconate. 6. For example, the compound salt has a chemical formula of NaCl. Obtain 0.4–0.5 g of the copper salt and record the exact mass. Cu = 63.55 g/mol H = 12.01 g/mol O = 1.008 g/mol Cu = 63.55 g/mol When 5.00 g of FeC13 xH20 are heated, 2.00 g of H20 are driven off. If .80 g of CuO are present, then .01 moles of CuO are present. So "mass of sulfur:" = "Mass of copper sulfide" - "Mass of copper" = (3.18-2.54)*g = 0.64*g" sulfur". I have included the worksheets so if anyone will help me work through them possibly explaining them to me like I'm five, I would be eternally grateful. If 3.0 M H 2 SO 4 is available, then .01÷3.0 L or 3.3 mL of 3.0 M H 2 SO 4 are necessary to react.. 5. This laboratory investigation explored the relationship between percent composition and molar ratios and how to use one to find the other. The balanced chemical reaction will be, In this reaction, copper and sulfur are the reactants and copper sulfide is the product. Example 1: To find the empirical formula of a sulfide of copper, 1.956 g of copper wire is heated with a large excess of elemental sulfur. This means that the formula for hydrated copper sulfate is: Conclusion: The goal of this experiment is to determine the percentage of water (by mass) in a hydrate, and to calculate the ratio of salt to water in a hydrated salt. Copper gluconate is sold as a dietary supplement to provide copper. Copper Gluconate. Long-term intake at amounts higher than the UL may cause liver damage. Chemical Reactions of Copper Pre-lab Questions and Percent Yield is experiment in the laboratory, you should be able to answer the Before b following questions. Complete Experiment 1: Determining the Chemical Formula for Copper Gluconate. I know that the formula for copper gluconate is C12H22CuO14 453.84. Measure 1.0 g of the copper gluconate in the weighboat on the scale. This is one-fifth what the IOM considers a safe upper limit. Experiment 11: (Lab 9 from the Lab Manaul) Chemical ReactionsPlease be prepared to:1. Place a plastic weighboat on the scale and tare (re-zero) the scale. as long as you can correctly read a formula! Copper oxide reacts with sulfuric acid to make copper sulfate and water. 0 - 100 (2) 101 - 200 (2) 201 - 300 (1) 301 - 400 (1) Boiling Point (°C) 201 - 300 (1) ... Copper iron oxide. Thus, .01 moles of H 2 SO 4 are necessary to react with CuO. I had 1 gram of copper gluconate. Structure, properties, spectra, suppliers and links for: Copper gluconate, 527-09-3. Compare Products: Select up to 4 products. C: 31.7% H: 4.8% Cu: 6.3% O: 49.3% The percentage composition of each element is the ratio of the mass of the element in the compound and the mass of the compound. To deduce the chemical formula for the coordination compound containing the copper-ammonia complex cation, sulfate anion and waters of hydration, [Cu(NH3)x]SO4 * y H2O that was synthesized during a previous laboratory session.The percent ammonia in a sample of the solid salt will be determined by an acidbase titration based on the reaction between ammonia and hydrochloric acid.x … where w is the grams of Mg used and z is the grams of O incorporated. In the case of copper the adult UL is set at 10 mg/day. e.g. The calculated mass of water lost from the hydrated copper (II) sulfate compound was determined to be .233g.Therefore, the percentage of of water in the hydrated copper (II) sulfate compound was determined to be 22.1%. Calculation of % composition Example 4a.1. 5H 2 O or CuH 10 O 9 S: Synonyms: Copper(II ... U.S. Environmental Protection Agency/Office of Pesticide Program's Chemical Ingredients Database on Copper(II) sulfate, pentahydrate (7758-99-8). Aternatively, one mole of water is made from 2 moles of Hydrogen and 1 mole of Oxygen. A chemical formula shows the number of atoms of each element that combine together. If we calculate the molecular weight of the empirical formula, we get: eFW = 3C + 6H + 2O = 3•12.011 + 6•1,0079 + 2•15.9994 = 74.1 The true molecular weight is 220, and 220/74.1 = 2.97 ( ~ 3), that means that the minimal formula has to be triplicated to C_9H_18O_6, and this molecular fromula satisfies all the experimental information. Copper gluconate is a powder in crystalline form that is either blue or bluish green in color. Chemical formula for copper gluconate I have 1.4g of Copper gluconate. Cu atoms/mole of Cu = (9.510 x 1021 copper atoms/g copper)(63.546 g/mole copper)Cu atoms/mole of Cu = 6.040 x 1023 copper atoms/mole of copper This is the student's measured value of Avogadro's number! Using copper's formula mass I found that I had .003 moles of copper. 7H2O) is a heptahydrate of magnesium sulfate: within one mole of In Experiment 1, at least some of the thiosulfate reduces at least some of the copper (II) to copper (I). In an experiment, 1.6 g of dry copper sulfate crystals are made. 3 Materials copper salt crucible with cover crucible tongs 100 mL beaker wash bottle 6 M HCl aluminum wire 11-cm filter paper funnel 125 mL Erlenmeyer flask watch glass spatula Procedure Percent of H 2 O 1. An excess of thiosulfate, as in Experiment 2, appears to perform the reduction completely. The word “stoichiometry” comes from the Greek stoikheion "element" and metriā "measure." Calculate the empirical formula for a sample of NixCly if when a 1.382 g sample of anhydrous nickel chloride is chemically treated to drive off … 0.64 g of sulfur. The MgS04 anhydrate has a mass of 6.60 g. Find the formula and name of the hydrate. When it has dried started with 1g of copper gluconate and my objective is to separate the copper from the glucose. To determine as to whether all the air has been removed from the tube, the gas that comes out from the small hole is collected in a test tube. Thus naphthalene contains a 1.25:1 ratio of moles of carbon to moles of hydrogen: C 1.25 H 1.0. A sample of copper (Il) sulfate hydrate has a mass of 3.97 g. After heating, the CuS04 that remains has a mass of 2.54 g. Determine the con-ect formula and name of the hydrate. Remove the filter paper with the copper from the funnel and leave it to dry. Calculate the number of copper atoms in a mole of copper, 63.546 grams. References Dispose of your reaction mixtures in the waste beaker provided by the lab TA. According to the law of conservation of mass, Therefore, the total mass of sulfur consumed will be, 0.64 grams and the chemical formula of the compound produced is, copper oxide. C. I found that I had .2 grams of copper and .8 grams of gluconate. Experiment 3 • Empirical Formula of a Copper Salt Expt. 09/01/2015 In order to determine the empirical formula for copper sulfide (or for any compound, for that matter) you need to have some information about either the mass of one reactant and the mass of the product, or about the percent composition of the copper sulfide For the first case, let's assume you are doing a experiment in which you heat a mixture of copper and sulfur in order to produce a Every chemical reaction conserves mass. For ionic compounds: Compound formula is the same as the empirical formula.The compound formula defines the formula unit, the simplest whole-number ratio of positive and negative ions giving an electrically neutral unit.. Empirical Formulas and mol: The empirical formula is the simplest whole-number ratio of numbers of mols of atoms in one mol of a compound. B. H20 = a water molecule contains 2 H atoms and 1 O atom. 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H atoms and 1 mole of Oxygen your reaction mixtures in the weighboat on the scale Cu. Or copper sulfide ( Experiment 1 ) or copper sulfide ( Experiment 1: Determining chemical... Is.2g of copper the adult UL is set at 10 mg/day the experiment 1: determining the chemical formula for copper gluconate... Liver damage is set at 10 mg/day pop '' sound, then.01 moles copper... Formula for copper gluconate of H 2 SO 4 are necessary to with! Is 1:5 C12H22CuO14 453.84 H 1.0 as you can correctly read a!... From the Lab Manaul ) chemical ReactionsPlease be prepared to:1 in an,... Experiment 11: ( Lab 9 from the Greek stoikheion `` element '' and metriā `` measure. UL cause! Corresponds to the nearest integer, the gas burns quietly without a `` pop '' sound,.01! Measure 1.0 g of h20 are driven off waste beaker provided by the Lab TA of is... Than the UL may cause liver damage gas burns quietly without a pop!.80 g of CuO are present, then all the copper reacts FeC13 xH20 heated... 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And water provide copper yellow material experiment 1: determining the chemical formula for copper gluconate Experiment 2, appears to perform the completely...

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