# Stoichiometry How To

### Calcium Carbonate + Nitric acid

## Type of Reaction

## Reactants

## Products

## Balanced Equation

## IUPAC NAMING

HNO3= Nitric Acid

Ca(NO3)2= Calcium Nitrate

CO2= Carbon Dioxide

H2O= Water

## Molar Masses

HNO3= 63.01 g/mol

Ca(NO3)2=164.088 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.

## Theoretical Yeild

## Percent Yeild

**Percentage Yield = Mass of Actual Yield x 100%**

**----------------------------Mass of Theoretical Yield**

**(Ignore the dashes i used them to center the equation)**