1 Write Empirical Formulas For The Following Compounds Containing A 0 200 Mol Al And 0 600 Mole Cl B 0 0400 Mol Ba 0 1 (103.5 KiB) Viewed 28 times
1 Write Empirical Formulas For The Following Compounds Containing A 0 200 Mol Al And 0 600 Mole Cl B 0 0400 Mol Ba 0 2 (102.33 KiB) Viewed 28 times
1 Write Empirical Formulas For The Following Compounds Containing A 0 200 Mol Al And 0 600 Mole Cl B 0 0400 Mol Ba 0 3 (38.85 KiB) Viewed 28 times
1. Write empirical formulas for the following compounds containing. a 0.200 mol Al and 0.600 mole Cl b. 0.0400 mol Ba, 0.0400 mol S, and 0.160 mol O 2. A student ignited lead in a crucible in an oxygen rich atmosphere to form a lead oxide compound. The mass of the empty crucible is 22.35g. The mass of the crucible and the lead before heating is 25.08g. After heading, the mass of the crucible plus lead oxide formed is 25.05g. (Show all work!) a.) What is the mass of Pb in the lead oxide compound? b.) What is the mass of O in the lead oxide compound? c. Calculate the moles of Pb in the lead oxide compound. d. Calculate the moles of O in the lead oxide compound. e. Calculate the molar ratio of Pb: O and determine the empirical formula for the lead oxide compound. 3. A compound of only nitrogen and oxygen is 30.5% nitrogen. The molar mass of the molecular compound was found to be 92 g/mol. Find the empirical formula and molecular formula of the compound. (Show all work!)
REPORT FORM: Assume that a student followed the same procedure you have just outlined above and performed the experiment. Below is given some of their experimental data. Fill in any blanks in the data using your logic, then complete. 37.2 g 1. Mass of empty crucible and lid. 2. Mass of empty crucible, lid and magnesium ribbon Mass of magnesium used 3. Mass of crucible, lid, and MgO product 4. Show all work in your empirical formula calculation! Mass of magnesium oxide formed in experiment Mass of oxygen formed in experiment Moles of magnesium used: Moles of oxygen used: Ratio of Mg:0= I Experimental Empirical formula: 37.62 .g g 37.9 E bil g mol mol
1. What are some possible sources of error in this experiment? 2. What is the percent magnesium in the magnesium oxide compound based on your experimental data? (Remember % composition= [mass of element/mass of compound] x 100%) 3. 0.606 g of rust (iron oxide) is formed when 0.424 g of iron is burned in oxygen rich air. Find the empirical formula of the iron oxide. What is the name for this compound? (Show all work!)
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