Sodium sulphate is used in detergents and can be synthesized by the following unbalanced reaction:
NaCl + H₂SO₄ $\rarr$ Na₂SO₄ + HCl
How much sulphuric acid (in kg) would be required to consume 5.0 x 10³kg of NaCl?

Question

Sodium sulphate is used in detergents and can be synthesized by the following unbalanced reaction:
NaCl + H₂SO₄

\rarr

Na₂SO₄ + HCl
How much sulphuric acid (in kg) would be required to consume 5.0 x 10³kg of NaCl?

Quizplus · Accepted Answer

The balanced chemical equation for the synthesis of sodium sulfate from sodium chloride and sulfuric acid is: $2NaCl + H_2SO_4 \rightarrow Na_2SO_4 + 2HCl$. This shows that 1 mole of $H_2SO_4$ reacts with 2 moles of $NaCl$. Given that the molar mass of $NaCl$ is approximately 58.5 g/mol and that of $H_2SO_4$ is approximately 98 g/mol, for every 117 g (2 moles) of $NaCl$, 98 g (1 mole) of $H_2SO_4$ is required. Given 5.0 x $10^{3}$ kg (or 5.0 x $10^{6}$ g) of $NaCl$, the mass of $H_2SO_4$ required can be calculated as follows: $(5.0 x 10^{6} g \, NaCl) \times (98 g \, H_2SO_4 / 117 g \, NaCl) = 4.2 x 10^{6} g$, or 4.2 x $10^{3}$ kg of $H_2SO_4$.

Sodium Sulphate Is Used in Detergents and Can Be Synthesized →\rarr→

Sodium Sulphate Is Used in Detergents and Can Be Synthesized $\rarr$