Problemas
Given the following equation: underline ( )Fe+underline ( )Ssarrow underline ( )FeS (Balance this equation first) 6. How many grams of FeS are produced from 5 moles of sulfur?
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Lourdes
professionell · Tutor durante 6 años
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(263 Votos)
Respuesta
To balance the chemical equation, we need to ensure that the number of atoms of each element is the same on both sides of the equation. In this case, we have:Fe + S → FeSTo balance this equation, we need to add a coefficient of 1 in front of each compound:1Fe + 1S → 1FeSNow, the equation is balanced, and we can proceed to the next step.To determine how many grams of FeS are produced from 5 moles of sulfur, we need to use the stoichiometry of the balanced equation.According to the balanced equation, 1 mole of sulfur reacts with 1 mole of iron to produce 1 mole of FeS.Therefore, if we have 5 moles of sulfur, we can expect to produce 5 moles of FeS.To convert moles of FeS to grams, we need to use the molar mass of FeS. The molar mass of FeS is approximately 87.87 g/mol.So, the mass of FeS produced from 5 moles of sulfur is:5 moles of FeS × 87.87 g/mol = 439.35 grams of FeSTherefore, 439.35 grams of FeS are produced from 5 moles of sulfur.