Consider the combustion of liquid octane (molar mass = 114.23 g/mol) and the associated enthalpy change: 2 C8H18 (L) + 25 O2 (g) -> 16 CO2 (g) + 18 H2O ΔH = 10860 kJ What mass (in g) of octane needs to be burned to provide 4225.8 kJ of energy?
Added by Deborah C.
Step 1
First, we need to understand that the enthalpy change given is for the combustion of 2 moles of octane. This means that 10860 kJ of energy is released when 2 moles of octane are burned. Show more…
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