# Calcium Carbonate + HNO3

## Types of Reaction

Calcium Carbonate + HNO3 is a double replacement. Ca(CO3) + HNO3 ~Ca(NO3)2 + H2CO3
Calcium Carbonate and Hydrogen Nitrate is aqueous. Calcium Nitrate and Hydrogen Carbonate is aqueous too.
Balanced equation
Ca(CO3) + 2 HNO3 Ca(NO3)2 + H2 CO3

## Molar mass of each reactant and products.

Ca(CO3) Ca=12.011+ C=12.011+ O=15.999(3) = 100.086g/mole
HNO3 H= 1.008+ + N=14.007+ O=15.999(3)= 47.997g/mole
Ca(NO3)2 Ca=40.078+ N=14.007(2) + O=15.999(6) = 164.086g/mole
H2CO3 H=1.008(2)++ C=12.011+O=15.999(3) =47.997g/mole
Mole to Mole conversions
3.21 mole Ca(CO3) times 1 mole H2CO3 divided by
_ 1mole Ca(CO3) 1 Mole Ca(CO3) = 3.21 mole H2CO3
Mass to Mass conversion
12.1g Ca(CO3) 1 mole Ca(CO3) 2mole HNO3 63.012 mole HNO3 = 15.22g HNO3
_ 100.086gCa(CO3) 1 mole Ca(CO3) 1 mole HNO3
Limiting and excess reactants

12.3g Ca(CO3) times 1 mole Ca(NO3)2 times 1 mole H2CO3 times 62.012 mole HNO3 divided by

_ times 100.086 g Ca(CO3) times 1 mole Ca(CO3)2 times 1 mole HNO3

7.62g H2CO3

12.3 g HNO3 times 1 mole HNO3 times 1 mole H2CO3 times 62.024 g H2CO3 divided by

_ 63.012 HNO3 times 2 mole HNO3 times 1 mole H2CO3

6.05g H2CO3

12.3g Ca(CO3) is excess. 12.3 g HNO3 is limited because 6.05 is less then 7.62

Theoretical yield

The theoretical yield is the amount predicted by a stoichiometric calculation based on the number of moles of all reactants present. This calculation assumes that only one reaction occurs and that the limiting reactant reacts completely.

6.05g H2CO3

Percent yield

defined as the actual yield/theoretical yield x 100

4.87 divided by 6.05 = .804 times 100 = 80.49%

Mole-to-mole and Mass-to-mass Conversions