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Data: Find: Tf: ? of the water
Benzene (C6H6) : 7.800 g
H2O : 2.387 Kg
Ti : 21.0 *C
Specific heat of water : 4.184 J/g . C
1) First we have to find the amount of heat released by the burning of 7.800 g of benzene. To find the it, we need to first write down the balanced equation for the combustion of benzene. Then use the ∆hf* of the reactants and products to find the ΔH°rxn using Hess' Law:
ΔH°rxn = Σ ΔH°f (products) - Σ ΔH°f (reactants)
2 C6H6(l) + 15 O2(g) ----> 12CO2(g) + 6H2O(g) ΔH°rxn = - 6271 K
ΔH°rxn = 12(CO2)
+ 6( H2O) – 2(C6H6) + 15(O2)
ΔH°rxn = 12(-393.5 KJ/mol) + 6 ( -241.8 KJ/ mol) – 2(49.1 KJ/ mol)
+ 15 (0 KJ/ mol) = -6271 KJ
2) Once we have the ΔH°rxn for the balanced equation of the combustion process, we can find the amount of heat released by the burning of 7.800 g of C6H6 by simply converting from grams to moles of benzene and calculating the heat produced by the burning of that many moles of reactant.
7.800 g C6H6 x
(1 mol C6H6 / 78.108 g) =
0.09986173 mol C6H6
(-6271 KJ / 2 mol C6H6 ) x 0.09986173 mol C6H6 = - 313.1165 KJ
q = m x Cs x ∆T
313116.5 J = (2387 g) x (4.184 J/ g . °C) x ∆T
313116.5
J/ (2387 g) x (4.184 J/ g . °C) = ∆T
∆T = 31.35 °C
∆T
= Tf - Ti
∆T
+ Ti = Tf
Tf = 31.35 °C + 21.0 °C = 52.35 °C
- http://www.mychemistrytutor.com/questions/calculating-delta-hrxn-combustion-benzene-using-enthalpy-formation-values
- http://www.saplinglearning.com/ibiscms/mod/ibis/view.php?id=492792
- https://sites.google.com/site/chempendix/thermo
- http://www.chemteam.info/Thermochem/HessLawIntro2.html
- Tro, Nivaldo J. “Chemistry A Molecular Approach.”Pearson. 2nd Ed. pp. 612-655.Print.2008.
Very well done!
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