Answer:
600.6L
Explanation:
Step 1:
The balanced equation for the reaction.
3CO + Fe2O3 --> 2Fe + 3CO2
Step 2:
Determination of the number of moles in 1001g of Fe.
This is illustrated below:
Mass of Fe = 1001g
Molar Mass of Fe = 56g/mol
Number of mole =?
Number of mole = Mass/Molar Mass
Number of mole of Fe = 1001/56
Number of mole of Fe = 17.875 mole
Step 3:
Determination of the number of mole of CO that reacted during the process.
This is illustrated below:
3CO + Fe2O3 --> 2Fe + 3CO2
From the balanced equation above,
3 moles of CO produced 2 moles of Fe.
Therefore, Xmol of CO will produce 17.875 moles of Fe i.e
Xmol of CO = (3 x 17.875)/2
Xmol of CO = 26.8125 moles
Step 4
Determination of the volume occupied by 26.8125 moles of CO at stp.
1 mole of a gas occupy 22.4L at stp.
Therefore 26.8125 moles of CO will occupy = 26.8125 x 22.4 = 600.6L
Therefore, 600.6L of CO is needed to produce 1001g of Fe
Answer:
[tex]V=602L[/tex]
Explanation:
Hello,
In this case, for the given chemical reaction:
[tex]3 CO + Fe_2O_3 \rightarrow 2 Fe + 3 CO_2[/tex]
In such a way, for the 1,001 g of iron, we compute the required moles of carbon monoxide by using the 2:3 mole ratio:
[tex]n_{CO}=1,001gFe*\frac{1molFe}{55.845gFe}*\frac{3molCO}{2molFe} \\\\n_{CO}=26.89molCO[/tex]
Finally, we use the ideal gas equation to compute the volute at STP conditions (1atm and 273K):
[tex]V=\frac{nRT}{P}=\frac{26.89mol*0.082\frac{atm*L}{mol*K}*273K}{1atm} \\\\V=602L[/tex]
Best regards.
