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ivann1987 [24]
4 years ago
11

PLEASE HELP!

Chemistry
2 answers:
Arturiano [62]4 years ago
8 0

Answer: A. 1.333 mol

Explanation:

4Fe+3O_2\rightarrow 2Fe_2O_3

To calculate the moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}

\text{Number of moles}=\frac{63.98g}{32g/mol}=2.0moles

As oxygen is completely consumed, it is the limiting reagent and will limit the formation of Fe_2O_3.

According to stochiometry,

3 mole of O_2 produces 2 moles of Fe_2O_3

Thus 2 moles of O_2 will produce=\frac{2}{3}\times 2= 1.333 moles of Fe_2O_3

Thus the correct answer is 1.333 moles

adelina 88 [10]4 years ago
7 0
<span>he balanced equation for the reaction is
4Fe + 3O</span>₂ ---> 2Fe₂O₃<span> 
stoichiometry of O</span>₂ to Fe₂O₃  is 3:2
                   
number of O₂ moles used up - mass present / molar mass of O₂
number of O₂ moles = 63.98 g / 32 g/mol = 1.999 mol
 
if 3 mol of O₂ forms 2 mol of Fe₂O₃  
then 1.999 mol of O₂ forms - 2/3 x 1.999 mol = 1.333 mol
answer is A) 1.333 mol of Fe₂O₃  are formed
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