chem. lab report - Lab: Molar Volume of a Gas Kasey...

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Lab: Molar Volume of a Gas Kasey Remillard 4-18-08 Purpose: After completing this experiment, you should be able to compare the volume of gas generated in lab to the accepted value of 22.414 liters per mole of STP. Apparatus: 400 mL Beakers Thermometer 100 mL graduated cylinder ring stand Thread Centimeter rule Rubber stopper (one-hole, #00) 50 mL Buret clamp Eudiometer Data Table: Mass of Mg used .04 g Moles of Mg consumed .002 moles Moles of H2 produced .002 moles Temperature 28 c (301 k) Barometeric Pressure 1.011 atm Partial Pressure of H20 28.349 mm Hg Partial Pressure of H2 739.75 mm Hg Volume of dry H2 44.08 mL Calculations: 1. Write the balanced equation for the reaction, include the phases. Mg(s) + 2 HCl(aq) ---> MgCl 2 (aq) + H 2 (g) 2. Find the mass of the magnesium. .04 g 3. Calculate the moles of magnesium reacted for the mass reacted. .04g of Mg 1 mole = .002 moles of Mg 24.3 g of Mg Materials: Magnesium ribbon, untarnished Hydrochloric acid, 6M
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chem. lab report - Lab: Molar Volume of a Gas Kasey...

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