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Ok, so I'm working on a problem that is asking me to find the heat of formation of Acetylene. I'm given the heat of formation of both CO2 and O2. From that I'm assuming I am suppose to use the heat of combustion of acetylene (given) to determine the heat of formation of acetylene. I got it up to there.
My problem is when you balance the equation, you get:
C2H2 + 2.5O2 --> 2CO2 + H2O
That too makes sense, but why do you not balance it out so that all the coefficients are whole numbers? For example why wouldn't it be:
2C2H2 + 5O2 --> 4CO2 +2H2O
Solving for the heat of formation gives different results depending on which equation you use. The book I'm using uses the first equation with the 2.5O2 coefficient.
My problem is when you balance the equation, you get:
C2H2 + 2.5O2 --> 2CO2 + H2O
That too makes sense, but why do you not balance it out so that all the coefficients are whole numbers? For example why wouldn't it be:
2C2H2 + 5O2 --> 4CO2 +2H2O
Solving for the heat of formation gives different results depending on which equation you use. The book I'm using uses the first equation with the 2.5O2 coefficient.