Stoichiometry How To
Calcium Carbonate + Nitric acid
Type of Reaction
HNO3= Nitric Acid
Ca(NO3)2= Calcium Nitrate
CO2= Carbon Dioxide
HNO3= 63.01 g/mol
CO2= 44.01 g/mol
H2O= 18.015 g/mol
To find the molar masses of the compound just add the masses of the compound elements together.
Mole To Mole Conversions
EX: You have 12.1 moles of H2O, but need to know the amount of moles HNO3 has.
When you look at the balanced equation the coefficients show us the ration.
We use this ratio to setup an equation. In this problem it would be 2/1.
This means for every H2O Mole there is, there is an extra HNO3 mole.
To get the answer just multiply(or divide in this case its multiply) the moles given by the ratio.
The answer would be 24.2 Moles of HNO3.
Mass To Mass Conversions
The fist half of this conversion if the same as the mole to mole conversion, with three extra steps.
After you get the ratio from the coefficients you set the mass of substance y over one mole.
Limiting and Excess Reactent
However you have to do this twice once for each given Reactant.
The lowest mass that can be produced will be your limiting reactant, and the highest will be your excess reactant.
Percentage Yield = Mass of Actual Yield x 100%
----------------------------Mass of Theoretical Yield
(Ignore the dashes i used them to center the equation)