Experiment 7 empirical formula lab report

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please solve tha following papers 119,120,121,122

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solve them in the same files.

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please check the attachment1/15/13 10:28 AM Page 119 Experiment 7 Prelaboratory Assignment Empirical Formulas Date __________ Lab Sec. ______ Name ____________________________________________ Desk No. __________ 1. Elemental mercury was first discovered when a mercury oxide was decomposed with heat, forming mercury metal and oxygen gas. When a 1.048-g sample of the mercury oxide is heated, 0.971 g of mercury metal remains. Note: Do not attempt this experiment in the laboratory because of the release of toxic mercury vapor. a. What is the mole ratio of mercury to oxygen in the sample? Richard Megna/Fundamental Photographs exp07.qxd b. What is the empirical formula of the mercury oxide? 2. A 2.60-g sample of titanium chemically combines with chlorine gas to form 10.31 g of a titanium chloride. a. What is the empirical formula of titanium chloride? b. What is the percent by mass of titanium and the percent by mass of chlorine in the sample? 3. a. Experimental Procedure, Part A. List two reasons for using crucible tongs to handle the crucible and lid after their initial firing. b. Why is it best to cool the crucible and lid (and sample) in a desiccator rather than on the laboratory bench? Experiment 7 119 exp07.qxd 11/15/13 10:28 AM Page 120 4. Experiment Procedure, Part D.2. State the reason for the use of the fume hood. 5. Experiment Procedure, Part D.3. Characterize a cool flame. 6. A sample of pure iron was covered with an excess of powdered elemental sulfur. The mixture was heated to a temperature where a reaction occurred and the excess sulfur was volatilized. The following data were collected. Complete the table. See Report Sheet Record the calculated value with the correct number of significant figures. Calculation Zone 1. 2. 3. 6. 7. 8. Mass of crucible and lid (g ) Mass of crucible, lid, and iron sample (g ) Mass of Fe sample (g ) Final mass of crucible, lid, and Fe/S compound (g ) Mass of Fe/S compound (g ) Combination Reaction of Iron and Sulfur _______ 19.746 _______ 20.422 _______ 21.195 _______ _______ _______ a. Mass of S in compound (g ) b. Mass ratio of Fe to S in compound _______ Part 8b Part 8c Part 8d _______ Show calculation. c. Moles of Fe in compound _______ Show calculation. d. Moles of S in compound Part 8e _______ Show calculation. e. Mole ratio (empirical formula) of Fe to S Show calculation. f. Percent by mass (%) 120 Empirical Formulas ____________%Fe _______ ____________%S exp07.qxd 11/15/13 10:28 AM Page 121 Experiment 7 Report Sheet Empirical Formulas Date __________ Lab Sec. ______ Name ____________________________________________ Desk No. __________ Indicate whether the following data are for Part B, Part C, or Part D. __________ Identify the original sample __________ Trial 1 Trial 2 1. Mass of crucible and lid (g ) ______________________ ______________________ 2. Mass of crucible, lid, and sample (g ) ______________________