Answer:
Depending on the definition of "standard" conditions, the volume of O₂ required here will be either
Explanation:
Relative atomic mass data from a modern periodic table:
How many moles of iron Fe in that 35.8 gram of iron metal?
[tex]M(\mathrm{Fe}) = \rm 55.845\; g\cdot mol^{-1}[/tex].
[tex]\displaystyle n = \frac{m}{M} = \rm \frac{35.8\; g}{55.845\; g\cdot mol^{-1}} = 0.641060\; mol[/tex].
How many moles of oxygen gas will be required?
Consider the ratio between the coefficient of Fe and that of [tex]\mathrm{O_2}[/tex] in the equation:
[tex]\displaystyle \frac{n(\mathrm{O_2})}{n(\mathrm{Fe})} = \frac{3}{1} = 3[/tex].
As a result,
[tex]\displaystyle n(\mathrm{O_2}) = n(\mathrm{Fe}) \cdot \frac{n(\mathrm{O_2})}{n(\mathrm{Fe})} = \rm 0.641060\; mol \times 3 = 1.92318\; mol[/tex].
What's the volume of that [tex]\rm 1.92318\; mol[/tex] of oxygen gas under STP?
One mole of an ideal gas occupies a volume 22.4 Liters under STP (or 22.7 liters in certain textbooks.) The volume of an ideal gas is directly related to the number of moles of particles in this gas. Assume that oxygen acts like an ideal gas under STP. As a result, 1.92318 moles of oxygen will occupy a volume of either
[tex]\rm 1.92318\; mol \times 22.4\; L\cdot mol^{-1} = 43.1\; L[/tex] or
[tex]\rm 1.92318\; mol \times 22.7\; L\cdot mol^{-1} = 43.7\; L[/tex].
