Question

In the reaction BaCO3 + 2HNO3 + Ba(NO3)2 + CO2 + H2O, what mass of Ba(NO3)2 can be formed by combining 55 g BaCO3 and 26 g HNO3

Answer 1

From the stoichiometry of the reaction, the mass of barium nitrate produced is 54.9 g.

Stoichiometry

The term stoichiometry refers to mass - volume relationships. Stoichiometry can be used to calculate the amount, mass or volume of reactants and products from the balanced reaction equation.

The equation of the reaction is written as follows;

BaCO3 + 2HNO3 ------>  Ba(NO3)2 + CO2 + H2O

Number of moles of BaCO3  = 55 g/197.34 g/mol = 0.28 moles

Number of moles of HNO3 = 26 g/63.01 g/mol = 0.41 moles

From the reaction equation;

1 mole of BaCO3 reacts with 2 moles of HNO3

0.28 moles of BaCO3 reacts with 0.28 moles ×  2 moles/1 mole = 0.56 moles

There is not enough HNO3 hence it is the limiting reactant.

Number of moles of Ba(NO3)2 produced  is obtained from;

2 moles of HNO3  yields 1 mole of Ba(NO3)2

0.41 moles of HNO3  yields 0.41 moles × 1 mole/2 moles

= 0.21 moles of Ba(NO3)2

Mass of  Ba(NO3)2  = 0.21 moles  × 261.337 g/mol = 54.9 g

Learn more about stoichiometry: brainly.com/question/9743981