1. Sodium Bicarbonate Decomposition Edward A. Mottel Department of Chemistry Rose-Hulman Institute of Technology

2. Resources Available  Exp. F: Quantifying a Chemical Reaction

3. Limestone  Limestone is a naturally occurring material consisting principally of calcium carbonate.  Upon heating (roasting) at >1000  C, it decomposes into calcium oxide and carbon dioxide.  You are the chief engineer. How could you determine when this roasting process is completed?

4. Sodium Bicarbonate Thermal Decomposition  Sodium bicarbonate decomposes when heated to form solid sodium carbonate, water vapor and carbon dioxide. If 2.00 grams of sodium bicarbonate is heated and completely decomposed, what will be the mass of the remaining solid?  Decide on the sequence of steps needed to solve this problem.

5. Sodium Bicarbonate Thermal Decomposition  Process Balance equation Identify a pathway to go from mass of reactant to mass of product. Calculate the answer. Check your answer -- does it seem reasonable?

6. Sodium Bicarbonate Thermal Decomposition  Sodium bicarbonate decomposes when heated to form solid sodium carbonate, water vapor and carbon dioxide. If 2.00 grams of sodium bicarbonate is heated and is 60% decomposed, what will be the mass of the remaining solid?  Decide on the sequence of steps needed to solve this problem.

7. Sodium Bicarbonate Thermal Decomposition Na 2 CO 3 60% NaHCO 3 40% 2.00 g 0.80 g 0.76 g 1.56 g

8. Sodium Bicarbonate Thermal Decomposition  A little harder problem If 2.00 gram sample of sodium bicarbonate is heated and has a mass of 1.56 grams after heating, what is the percentage converted (percentage yield)? Hint: How many moles of CO 2 and H 2 O are produced? How many moles of NaHCO 3 have decomposed?

10. 6/10/2015