Respuesta :
Answer
Balanced equation: Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
The grams of iron produced = 335.07 grams
Explanation
Given:
The unbalanced equation is: Fe₂O₃ + H₂ → Fe + H₂O
The moles of hydrogen gas that reacted = 9 moles.
What to find:
The balanced question and the mass in grams of iron produced.
Solution
Step 1: Balance the equation.
The equation can be balanced by adding 3 as the coefficient of H₂ on the reactant side and 2 and 3 as the coefficients of Fe and H₂O respectively.
Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
Step 2: Determine the moles of Fe produced.
Using the mole ratio of H₂ and Fe in the balanced equation in step 1 and the given moles of H₂ that reacted; then the moles of Fe produced is
[tex]\begin{gathered} 3mol\text{ }H₂=2mol\text{ }Fe \\ \\ 9mol\text{ }H₂=x \\ \\ Cross\text{ }multiply\text{ }and\text{ }divide\text{ }both\text{ }sides\text{ }by\text{ }3mol\text{ }H₂ \\ \\ x=\frac{9mol\text{ }H₂}{3mol\text{ }H₂}\times2mol\text{ }Fe \\ \\ x=6\text{ }mol\text{ }Fe \end{gathered}[/tex]Step 3: Covert the 6 moles of Fe produced in step 2 to grams.
From the periodic table; the molar mass of Fe = 55.845 g/mol.
So, using the mole formula, the mass of Fe produced is
[tex]\begin{gathered} Moles=\frac{Mass}{Molar\text{ }mass} \\ \\ Mass\text{ }of\text{ }Fe=Moles\times Molar\text{ }mass \\ \\ Mass\text{ }of\text{ }Fe=6\text{ }mol\times55.845\text{ }g\text{/}mol \\ \\ Mass\text{ }of\text{ }Fe==335.07\text{ }grams \end{gathered}[/tex]Therefore, the grams of iron that will be produced from 9 moles of hydrogen gas is 335.07 grams
