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Analytical chemistry

determination of the empirical formula of magnesium oxide

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Magnesium compounds
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Magnesium oxide
Crucible
Magnesium
Empirical formula

Determination of the Empirical Formula of Magnesium Oxide GOAL AND OVERVIEW The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal. Magnesium is reacted with oxygen from the air in a crucible, and the masses before and after the oxidation are measured. The resulting masses are used to calculate the experimental empirical formula of magnesium oxide, which is then compared to the theoretical empirical formula. A crucible and Bunsen burner will be used to heat magnesium metal to burning. Objectives of the Data Analysis: ? Determine the expected formula for the ionic oxide expected when Mg reacts with O2 ? Find the theoretical and actual yields of MgxOy

Chemistry 101 exam 1 key

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C10H14N2O3
C10H16N2O3

Chemistry 101 - Exam I Name _____________________ 27 September 2017 Show all work for credit. State any assumptions made to solve a problem. Give all numerical answers with the correct number of significant figures. All answers in scientific notation must be in correct scientific notation (i.e., 6.022?1023 not 6.022E23 or 6.022e23). All instances of incorrect scientific notation will result in the loss of 3 points each. All numbers that require units should have the units written. All instances of numbers without units will result in the loss of 3 points each. 1. (24 pts) Name the following organic compounds: a. O O propyl 4,4-dimethylheptanoate b. OH 2,5-dimethylphenol c. I 5-iodo-4-methyloct-2-ene

molarity and dilution

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Molarity Worksheet 1. Sea water contains roughly 28.0 g of NaCl per liter. What is the molarity of sodium chloride in sea water? 2. What is the molarity of 245.0 g of H2SO4 dissolved in 1.00 L of solution? 3. What is the molarity of 5.30 g of Na2CO3 dissolved in 400.0 mL solution? 4. What is the molarity of 5.00 g of NaOH in 750.0 mL of solution? 5. How many moles of Na2CO3 are there in 10.0 L of 2.0 M soluton? 6. How many moles of Na2CO3 are in 10.0 mL of a 2.0 M solution? 7. How many moles of NaCl are contained in 100.0 mL of a 0.20 M solution? 8. What weight (in grams) of NaCl would be contained in problem 7? 9. What weight (in grams) of H2SO4 would be needed to make 750.0 mL of 2.00 M solution? 10. What volume (in mL) of 18.0 M H2SO4 is needed to contain 2.45 g H2SO4?
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