Compare the amount of oxygen required to oxidize methane and ethane completely. Give your answer two ways: gO2/g compound and gO2/gC.
Combustion of methane
CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
1 mol of CH4 reacts with = 2 moles of O2
16 g of CH4 reacts with = 64 g of O2
gO2/gCH4 = 64/16 = 4
gO2/gC = 64/12 = 5.333
combustion of ethane
C2H6(g) +7/2 O2(g) → 2CO2(g) + 3H2O(l)
1 mol of C2H6 reacts with = 3.5 moles of O2
30 g of C2H6 reacts with = 3.5*32 = 112 g of O2
gO2/gC2H6 = 112/30 = 3.733
gO2/gC = 112/24 = 4.666
In the combustion of ethane gO2/g compound and gO2/gC are required less than combustion of methane.
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