Friday
November 28, 2014

Homework Help: Chemistry

Posted by Jenny on Monday, March 28, 2011 at 10:02pm.

Suppose that 0.650 mol of methane, CH4(g), is reacted with 0.800 mol of fluorine, F2(g), forming CF4(g) and HF(g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?

Substance & Enthalpy of Form. (kJ/mol)
C(g) 718.4
CF4(g) -679.9
CH4(g) -74.8
H(g) 217.94
HF(g) -268.61

I have figured out the equation:
CH4(g)+4F2(g) -> CF4(g)+4HF(g)

I also figured out the enthalpy of reaction:
Delta H = -1679.54kJ

I realize that I must figure out which of the reactants are limiting. How do I do that? What do I do after I find the limiting reactant?

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