Question #4da79

1 Answer
May 12, 2017

Answer:

The reaction produces 44 g of #"FeS"#.

Explanation:

Step 1. Write the chemical equation for the reaction

#M_text(r): color(white)(mm)256.52color(white)(m)87.91#
#color(white)(mm)"8Fe" + "S"_8 → "8FeS"#

Step 2. Calculate the moles of #"S"_8#

#"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 #"FeS"#

#"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 #"FeS"#

#"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"#