Balance the equation.
dHrxn = (n*dHf products) - (n*dHf reactants) in units of kJ/mol
q = dHrxn x (578/2*molar mass tristearin) = ?
If you have a 578 g of fat (tristearin) stored in your body, how much heat will be produced when it is metabolized?
tristearin is C57H110O6
The chemical reaction:
C57H110O6(s) + O2(g) --> CO2(g) + H2O (l)
DHf:
C57H110O6(s) -390.70
O2(g) 0
CO2(g) -393.5
H2O(l) -285.840
I don't know how to figure this one out.
5 answers
-11385 J
I don't get that. The best way you can do this is to show the balanced equation, then show step by step what your math is like and I can find the error if you've made one. I think we're wasting time with your multiple answers and my no that isn't right.
-75520 (578 / 2(891.4468)g = -24483 J
Note here that you obtained 75520 for dHrxn but on page 1 you are not using half of that if you are doing for 1 mole. And the 75520 agrees with the number I had (before dividing by 2) for 1 mole.
Here, I obtained 890 for the molar mass but I used 12 for C, 16 for O and 1 for H. Those large numbers probably make the difference between 890 and 891.4468 Anyway, the set up is ok and the answer is ok.
Here, I obtained 890 for the molar mass but I used 12 for C, 16 for O and 1 for H. Those large numbers probably make the difference between 890 and 891.4468 Anyway, the set up is ok and the answer is ok.