Using this equation for the decomposition of sodium bicarbonate upon heating, answer the following questions.
2NaHCO3 (s) + heat ------> Na2CO3 (s) + H2O (g) + CO2 (g)
a. How many moles of sodium bicarbonate are required to produce one mole of sodium carbonate?
b. Describe the flame used when doing the strong heating portion of the reaction.
c. You determine that the mass of the crucible plus sodium bicarbonate used in
the reaction is 34. 929 grams, what is the theoretical yield of sodium carbonate given that the molecular weight of sodium bicarbonate is 84. 0 grams/mole, the molecular weight of sodium carbonate is 106. 0 grams/mole, and the original mass of the crucible was 31. 033 grams. REMEMBER THAT THE MOLE RATIO IS NOT 1.1 this time!!
d. Given the same starting mass of sodium bicarbonate how many moles of carbon dioxide are produced?
e. Just for practice, let's say that liquid water was produced. Given the same starting mass of sodium bicarbonate, how much liquid water (in mL) would be produced? Remember that the density of water is 1 g/mL.
f. You determine that you have produced 4. 292 grams of sodium carbonate. Determine the percent yield.
g. Based off your percent yield, does it indicate any problems with the reaction? Suggest one possible source.