given the following equation: 8 fe + s₈ → 8 fes what mass of iron is needed to react with 16.0 grams of…

Answer:

43.9

Explanation:

Step1: Calculate molar mass of S₈

The molar mass of sulfur (S) is approximately 32.07 g/mol. For S₈, molar mass $M_{S_8}=8\times32.07\ g/mol = 256.56\ g/mol$.

Step2: Calculate moles of S₈

Given mass of S₈, $m_{S_8}=16.0\ g$. Moles of S₈, $n_{S_8}=\frac{m_{S_8}}{M_{S_8}}=\frac{16.0\ g}{256.56\ g/mol}\approx0.0624\ mol$.

Step3: Determine mole - ratio from the equation

From the balanced equation $8Fe + S_8\rightarrow8FeS$, the mole - ratio of $Fe$ to $S_8$ is 8:1. So, moles of $Fe$ needed, $n_{Fe}=8\times n_{S_8}=8\times0.0624\ mol = 0.4992\ mol$.

Step4: Calculate mass of Fe

The molar mass of iron (Fe) is approximately 55.85 g/mol. Mass of Fe, $m_{Fe}=n_{Fe}\times M_{Fe}=0.4992\ mol\times55.85\ g/mol\approx43.9\ g$.