Answer:
First line of the table:
FeS: 1.2mol
[tex]O_{2}[/tex]: 1.8moles
FeO: 1.2moles
[tex]SO_{2}[/tex]: 1.2moles
Second line of the table:
FeS: 5.2mol
[tex]O_{2}[/tex]: 7.8moles
FeO: 5.2moles
[tex]SO_{2}[/tex]: 5.2moles
Explanation:
1. Take as reference the balanced chemical equation:
[tex]_{2}FeS(s)+_{3}O_{2}(g)=_{2}FeO(s)+_{2}SO_{2}(g)[/tex]
2. Take the first quantity given in the table to calculate the quantities of the other compounds using stoichiometry:
- Calculate the number of moles of [tex]O_{2}[/tex]:
[tex]1.2molesFeS*\frac{3molesO_{2}}{2molesFeS}=1.8molesO_{2}[/tex]
- Calculate the number of moles of FeO:
[tex]1.2molesFeS*\frac{2molesFeO}{2molesFeS}=1.2molesFeO[/tex]
-Calculate the number of moles of [tex]SO_{2}[/tex]:
[tex]1.2molesFeS*\frac{2molesSO_{2}}{2molesFeS}=1.2molesSO_{2}[/tex]
3. Take the second quantity given in the table to complete the other quantities using stoichiometry:
- Calculate the number of moles of FeS:
[tex]5.2molesSO_{2}*\frac{2molesFeS}{2molesSO_{2}}=5.2molesFeS[/tex]
- Calculate the number of moles of [tex]O_{2}[/tex]:
[tex]5.2molesSO_{2}*\frac{3molesO_{2}}{2molesSO_{2}}=7.8molesO_{2}[/tex]
- Calculate the number of moles of FeO:
[tex]5.2molesSO_{2}*\frac{2molesFeO}{2molesSO_{2}}=5.2molesFeO[/tex]
