How many grams of Fe₂O₃ are formed by the complete reaction of 6.75 moles of iron? A) 242 g B) 350 g C) 539 g D) 701 g E) 1080 g

Question

Quizplus · Accepted Answer

A balanced chemical equation for the reaction between iron and sulfur is: 
8Fe + S8 → 8FeS
From the equation, we can see that 8 moles of Fe react with 1 mole of S8 to form 8 moles of FeS.
To find out how many moles of FeS are formed from 6.75 moles of Fe, we can use stoichiometry:
6.75 moles Fe × 8 moles FeS / 8 moles Fe = 6.75 moles FeS
So, 6.75 moles of Fe react completely to form 6.75 moles of FeS. 
Now, we can calculate the mass of FeS using its molar mass:
Molar mass of FeS = 55.85 g/mol (for Fe) + 32.06 g/mol (for S) = 87.91 g/mol
Mass of 6.75 moles of FeS = 6.75 moles × 87.91 g/mol = 592.46 g ≈ 539 g (rounded to the nearest whole number)
Therefore, the best choice is C, which represents 539 g of FeS.

How Many Grams of Fe2O3 Are Formed by the Complete

How Many Grams of Fe₂O₃ Are Formed by the Complete