equilibrium expression for the combustion of octane?
My project is due today =/ (it's 1:30 now, and I really need someone to clarify this last one question. Thanks!
This is what I got for the combustion of octane. ^denotes a superscript/exponent.
[H2O]^18[CO2]^16
-----------------
[C8H18]^2[O2]^25
Thanks! Please respond as QUICKLY as possible
please? I'm going to have to leave it like this =/
The equilibrium expression for the combustion of octane can be derived from the balanced equation for the reaction. The balanced equation for the combustion of octane is as follows:
C8H18 + 12.5 O2 → 8 CO2 + 9 H2O
The coefficients in the balanced equation give us the stoichiometry of the reaction. To write the equilibrium expression, we consider the molar concentrations or partial pressures of the reactants and products at equilibrium.
The equilibrium expression for the combustion of octane can be written as:
K = ([CO2]^8[H2O]^9) / ([C8H18][O2]^12.5)
Here, the square brackets denote molar concentrations if you are using concentrations or partial pressures if you are using pressures. The exponents represent the stoichiometric coefficients from the balanced equation.
In your given expression:
[H2O]^18[CO2]^16
-----------------
[C8H18]^2[O2]^25
It seems that the stoichiometric coefficients are not accurately represented. The coefficients in the expression should correspond to the stoichiometry in the balanced equation. Hence, the correct equilibrium expression would be:
[H2O]^9[CO2]^8
-----------------
[C8H18][O2]^12.5
I hope this clarification helps. Good luck with your project!