For the combustion of ethane, beginning with 3.21 mol of CH3CH3, 2CH3CH3(g) + 7O2(g) → 4CO2(g) + 6H2O(g)?
a. how many moles of O2 are required to completely consume the CH3CH3?
b. how many moles of CO2 are obtained when the CH3CH3 is completely combusted?
c. how many moles of H2O are obtained when the CH3CH3 is completely combusted?
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2CH3CH3(g) + 7O2(g) → 4CO2(g) + 6H2O(g)
(a) From the balanced equation:
the mole ratio CH3CH3 : O2 = 2 : 7
so 1 mol CH3CH3 reacts with 3.5 mol O2
so 3.21 mol CH3CH3 will be consumed completely by 3.21 x 3.5 = 11.235 mol O2
(b) The mole ratio CH3CH3 : CO2 = 2 : 4 = 1 : 2
so when 3.21 mol CH3CH3 is completely combusted 3.21 x 2 = 6.42 mol CO2 are obtained
(c) The mole ratio CH3CH3 : H2O = 2 : 6 = 1 : 3
so when 3.21 mol CH3CH3 is completely combusted 3.21 x 3 = 9.63 mol H2O are obtained