# Question #4da79

May 12, 2017

The reaction produces 44 g of $\text{FeS}$.

#### Explanation:

Step 1. Write the chemical equation for the reaction

${M}_{\textrm{r}} : \textcolor{w h i t e}{m m} 256.52 \textcolor{w h i t e}{m} 87.91$
$\textcolor{w h i t e}{m m} \text{8Fe" + "S"_8 → "8FeS}$

Step 2. Calculate the moles of ${\text{S}}_{8}$

${\text{Moles of S"_8 = 16 color(red)(cancel(color(black)("g S"_8))) × "1 mol S"_8/(256.52 color(red)(cancel(color(black)("g S"_8)))) = "0.0624 mol S}}_{8}$

Step 3. Calculate the moles of $\text{FeS}$

$\text{Moles of FeS" = 0.0624 color(red)(cancel(color(black)("mol S"_8))) × "8 mol FeS"/(1 color(red)(cancel(color(black)("mol S"_8)))) = "0.500 mol FeS}$

Step 4, Calculate the mass of $\text{FeS}$

$\text{Mass of FeS" = 0.500 color(red)(cancel(color(black)("mol FeS"))) × "87.91 g FeS"/(1 color(red)(cancel(color(black)("mol FeS")))) = "44 g FeS}$