Assuming all volume change is due to gases, calculate the work
for combustion of 1 mol of octane producing gaseous water.
Determine the work per liter of octane (density = 0.6986
g/cm3).
____L*atm
2 C8H18 + 25 O2 ---------------------> 16 O2 + 18 H2O
we know that 1 mol of gas can occupy 22.4 L volume
2 mol C8H18 require = 25 mol O2
= 25 x 22.4 L
= 560 L
so initial volume (V1) = 560 L
increases on product side . this can be considered as V2
2 mol C8H18 = 16 moles of CO2
= 16 x 22.4
= 358.4 L
2 mol C8H18 = 18 mol H2O
= 18 x 22.4 L
= 403.2 L
total volume on products side = 358.4 + 403.2 = 716.6 L
V2 = 716.6 L
work = P (V2-V1)
= 1 x (716.6-560 )
= 201.6 L-atm
for 2 mol C8H18 work = 201.6
for 1 mol C8H18 work = 100.8 L-atm
work = 100.8 L-atm ------------------------> answer
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