# From the equation below, how many grams of barium sulfate can be produced from 20.8 g of barium...

## Question:

From the equation below, how many grams of barium sulfate can be produced from {eq}20.8\ g {/eq} of barium chloride?

{eq}\rm BaCl_2 + Na_2SO_4 \to BaSO_4 + 2NaCl {/eq}.

## Molar Mass:

We know the total mass of a reagent by multiplying the required number of moles by the molar mass of the reagent. The molar mass used in more applications than this. We can determine the number of moles given the mass of reagent by dividing the mass by the molar mass of the substance.

## Answer and Explanation:

Determine the mass of the produced {eq}\displaystyle BaSO_4 {/eq} from the given mass of reagent by first assuming the abundance of {eq}\displaystyle Na_2SO_4 {/eq} and then finding the number of moles in the given reagent, and then multiplying the ratio of the coefficients of the product and the reactant from the chemical reaction and finally multiplying the molar mass of the product. We proceed with the solution.

{eq}\begin{align} \displaystyle 20.8\ g\ BaCl_2\times \frac{1}{208.23}\ \rm{mol/g}\times \frac{1\ mol\ BaSO_4}{1\ mol\ BaCl_2}\times 233.38\ \rm{g/mol} = 23.3\ g\ BaSO_4 \end{align} {/eq}