Name: Stoichiometry
Uploaded: 2019-07-19
Duration: 10 min 8 s
Description: Watch this video to learn the calculations of reactants or products with the help of a balanced chemical equation. It is termed stoichiometry.

Question

What mass of barium sulfate would be produced when $10 g$ of barium chloride is completely consumed in the following reaction?

${BaCl}_{2} (aq) + H_{2} {SO}_{4} (aq) \to {BaSO}_{4} (aq) + 2 HCl (aq)$

Accepted Answer

The given mass, $m$ of barium chloride $= 10 g$
The molar mass of barium chloride $({BaCl}_{2}), M_{r}$ $= [137 + (2 \times 35.5)] = 208 g {mol}^{- 1}$

The number of moles, $n = \frac{Given mass m}{Molar mass M_{r}} = \frac{10}{208} = 0.048 mol$

${BaCl}_{2} (aq) + H_{2} {SO}_{4} (aq) \to {BaSO}_{4} (aq) + 2 HCl (aq)$

From the above equation, it is clear that the number of moles of barium sulphate formed is the same as the number of moles of barium chloride taken. Therefore, $0.048 mol$ of barium sulphate will be formed.
Hence, the mass of barium sulphate produced from $10 g$ barium chloride is $= 0.048 \times$ molar mass of ${BaSO}_{4}$
$= 0.048 \times [137 + 32 + (4 \times 16)] = 0.048 \times 233 = 11.18 g$

What mass of barium sulfate would be produced when $10 g$ of barium chloride is completely consumed in the following reaction?

${BaCl}_{2} (aq) + H_{2} {SO}_{4} (aq) \to {BaSO}_{4} (aq) + 2 HCl (aq)$

Important Questions on Function

Learn and Prepare for any exam you want !

What mass of barium sulfate would be produced when 10 g of barium chloride is completely consumed in the following reaction? BaCl2 (aq) + H2SO4 (aq) → BaSO4 (aq) + 2HCl(aq)

Important Questions on Function

Learn and Prepare for any exam you want !

What mass of barium sulfate would be produced when $10 g$ of barium chloride is completely consumed in the following reaction?

${BaCl}_{2} (aq) + H_{2} {SO}_{4} (aq) \to {BaSO}_{4} (aq) + 2 HCl (aq)$