Answer :
Final answer:
In a chemical reaction 1.57 mol of sodium hydroxide would produce approximately 111.5 g of sodium sulfate.
Explanation:
The student's question asks, "What mass of sodium sulfate is produced from 1.57 mol of sodium hydroxide?" This is a stoichiometry problem involving a chemical reaction between sodium hydroxide (NaOH) and sulfuric acid (H2SO4) to produce sodium sulfate (Na2SO4) and water (H2O). The reaction is balanced as follows:
2NaOH + H2SO4 -> Na2SO4 + 2H2O
In this reaction, two moles of sodium hydroxide react with one mole of sulfuric acid to produce one mole of sodium sulfate. As such, if we have 1.57 moles of sodium hydroxide, we would expect to produce approximately 0.785 mol of sodium sulfate.
Next, we need to convert this amount in mol to grams. The molar mass of sodium sulfate is 142.04 g/mol. So, the mass of sodium sulfate produced would be:
0.785 mol x 142.04 g/mol = 111.5 g
In conclusion, 1.57 mol of sodium hydroxide would produce approximately 111.5 g of sodium sulfate.
Learn more about Stoichiometry here:
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