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15 Nov 2019
Stoichiometry of a gas producing reaction an getherunactions are mpassive or unchanging qualities. The unchanging reactants together under specific conditions, connect literally atoms, Chemical reactions can be thoug rearranging and new connections (bonds) bei ng made between atoms resulting in the formation o The evolution of a gas reactan process has occurred. Chemical reactions of this kind typican ets with hydrocho converted to products. In this experiment magnesium metai hydrogen gas and a salt. go to completion (all reactants are reacts with hydrochloric acid to form upon combining reactants is considered a clear indication that a chem Rinse a 50 mL Obtain a piece of magnesium metal ribbon graduated cylinder twice with distilled water. y sand remove any oxide by sanding the metal with a light grade sand emove any grit by wiping with a kimwipe, the magnesium metal. The mass should be in the range 0.030 g to 0.035 g. If the mass is ol the metal. Wind the metal into a tight coil which will fit into the mouth too great cut off some graduated cylinder. (not too tight do not want a ball) Insert a long stemmed funnel in the graduated cylinder and pour 4.0 mL (using a 10 mL graduated cylinder) of concentrated hydrochloric acid (12 M) in the bottom of the gradua cylinder. Add a 10 mL portion of distilled water to the graduated cylinder washing dow residual acid. Fill the mixing the water and acid as much as possible. the Avoid graduated cylinder completely to the top with distilled water. beaker of react with the acid in the Place the coil of magnesium in the graduated cylinder. Invert the cylinder into a large water (400- 800 mL) equipped with a thermometer. The metal shoul cylinder producing a gas which is trapped in the cylinder. After all the metal has reacted measure the volume of gas produced. Repeat the procedure. Pre-lab 1. 2. Write the balanced chemical equation. Calculate the volume of gas that can be produced if 0.0750 g of magnesium was reacted with 15.0 mL of 12 M HCI (Pay attention to the limiting reagent) Calculations 3. 4. 5. Calculate the moles of each reactant prior to the start of reaction. (moles of HCl and magnesium) Calculate the moles of gas produced using the limiting reactant and the balanced chemical equation. Use the ideal gas law to calculate the theoretical volume of gas produced based on the limiting reactant and determine the percent error. Lab Report Write a full lab report including Intro, Methods, Results and Conclusion. Be sure to address the following questions in the Conclusion Why is it important not to mix the concentrated HCl and water too much in the graduated cylinder? Why should the mass of magnesium not exceed 0.035 g? (What could happen?) 1) 2)
Stoichiometry of a gas producing reaction an getherunactions are mpassive or unchanging qualities. The unchanging reactants together under specific conditions, connect literally atoms, Chemical reactions can be thoug rearranging and new connections (bonds) bei ng made between atoms resulting in the formation o The evolution of a gas reactan process has occurred. Chemical reactions of this kind typican ets with hydrocho converted to products. In this experiment magnesium metai hydrogen gas and a salt. go to completion (all reactants are reacts with hydrochloric acid to form upon combining reactants is considered a clear indication that a chem Rinse a 50 mL Obtain a piece of magnesium metal ribbon graduated cylinder twice with distilled water. y sand remove any oxide by sanding the metal with a light grade sand emove any grit by wiping with a kimwipe, the magnesium metal. The mass should be in the range 0.030 g to 0.035 g. If the mass is ol the metal. Wind the metal into a tight coil which will fit into the mouth too great cut off some graduated cylinder. (not too tight do not want a ball) Insert a long stemmed funnel in the graduated cylinder and pour 4.0 mL (using a 10 mL graduated cylinder) of concentrated hydrochloric acid (12 M) in the bottom of the gradua cylinder. Add a 10 mL portion of distilled water to the graduated cylinder washing dow residual acid. Fill the mixing the water and acid as much as possible. the Avoid graduated cylinder completely to the top with distilled water. beaker of react with the acid in the Place the coil of magnesium in the graduated cylinder. Invert the cylinder into a large water (400- 800 mL) equipped with a thermometer. The metal shoul cylinder producing a gas which is trapped in the cylinder. After all the metal has reacted measure the volume of gas produced. Repeat the procedure. Pre-lab 1. 2. Write the balanced chemical equation. Calculate the volume of gas that can be produced if 0.0750 g of magnesium was reacted with 15.0 mL of 12 M HCI (Pay attention to the limiting reagent) Calculations 3. 4. 5. Calculate the moles of each reactant prior to the start of reaction. (moles of HCl and magnesium) Calculate the moles of gas produced using the limiting reactant and the balanced chemical equation. Use the ideal gas law to calculate the theoretical volume of gas produced based on the limiting reactant and determine the percent error. Lab Report Write a full lab report including Intro, Methods, Results and Conclusion. Be sure to address the following questions in the Conclusion Why is it important not to mix the concentrated HCl and water too much in the graduated cylinder? Why should the mass of magnesium not exceed 0.035 g? (What could happen?) 1) 2)