3rd Six Weeks Project
By:Glory Russell 1st period
Baking Soda (NaHCO3) and Hydrochloric Acid (HCl)
Double Displacement Sodium Bicarbonate and HCl
This reaction is a double replacement and decomposition
Balanced Equation
NaHCO3(aq)+HCl(aq)->CO2(g)+H2O(l)+NaCl(s)
Baking soda and Hydrochloric Acid makes Carbon Dioxide and Water and Sodium Chloride
Molar Mass of Reactants and Products
NaHCO3=84.0006 g/mole
HCl=36.461 g/mole
CO2=43.991 g/mole
H2O=18.015 g/mole
NaCl=58.443 g/mole
Mole to Mole Conversion
You start out with Mole A/ the given (In this case it is NaHCo3) on top. Then you put one mole on the bottom of Mole A. Then you want to end up with Mole B in the end so you put Mole B(NaCl) on top. The ratio will depend on the coefficients in the balanced equation(In this case they both had a coefficient of one). Then you multiply across the top and divide by the bottom.
Mass to Mass Conversions
You start with 12.1 grams of NaHCO3(Mole A) then you put the molar mass of NaHCO3 on the bottom, which is 84.006 grams. Then you put one mole on top (because 84.006 grams of NaHCO3 is equal to one mole of NaHCO3). Then you use the coefficient ratio, which in this case is one to one. One mole of NaHCO3 on bottom and one mole of HCl on the top. Then to get rid of moles you put one mole of HCl on the bottom. Then you put the molar mass of HCl (you get it from the periodic table). Then you multiply across the top and divide by the bottom and you should get 5.25 grams of HCl.
Limiting and Excess Reactant
Limiting Reactant
You first do a mass to mass conversion. Then in this case you can only make 8.56 grams NaCl, which is less than 19.72 grams NaCl. The limiting reactant is the 12.3 grams of NaHCO3.
Excess Reactant
You first do a mass to mass conversion. Then in this case you can make 19.72 grams NaCl, which is more than 8.56 grams NaCl. The excess reactant is the 12.3 grams of HCl.
Theoretical Yield
The theoretical yield is the how much of something (NaCl) the limiting reactant can make.
Percent Yield
You can find percent yields by dividing the actual yield by the theoretical yield, then multiplying by 100.