C6H6 (l) + O2 (g) 6 CO2 (g) + 3 H2O (g)
Hcomb = [6* Hf (CO2) + 3*Hof H2O (g) ] - [ Hfo(C6H6) + H(O2)]
= [6*(-393.5) + 3*(-245.15) ] - [ 49.2+ 0]
= -2361 -735.45 - 49.2
= -3096.45 - 49.2
= -3145.65 KJ/mole
Note:
[ Enthalpy of Formation of H2O (l) = -285.8 KJ/mole
and, H2O (l) H2O (g)
then, Enthalpy of formation of H2O (g) = Enthalpy of evaporation + Enthapy of formation of H2O (l) = 40.65 +(-285.8) = - 245.15 KJ ]
Enthalpy of formation of CO2 , H2O (l) , C6H6 (l) , O2 (g) are taken from literature.
Marks Calculate the enthalpy of combustion of benzene in which the water produced is a gas rather than a liquid. You ma...
2) Consider the combustion reaction of ethylene at 25 °C and 1 bar, but in the case that H20 is produced as a gas rather than a liquid: C2Halg)+3 O2(g)>2 CO2(g) + 2 H20(g) What is the standard enthalpy of the reaction? Information that may be useful for the calculation is given below (at the same temperature and pressure): C2H4(g)3 O2(g) -»2 CO2(g)+ 2 H2O(liq) AtusH(H20) 6.008 kJ mol-; AvaphH°(H2O) = 44.016 kJ mol-; AtH°(H20,g) = -241.82 kJ mol- (A)-1410.0...
Calculate the standard combustion enthalpy of propylene at 25 ° C using the standard formation enthalpy of liquid water (-286 kJ mol-1) and the following reactions: 1) CH2CHCH3 (g) + H2 (g) → CH3CH2CH3 (g); Δ? (1) = -125 kJ mol-1 2) CH3CH2CH3 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l); Δ? (2) = -2220 kJ mol-1 3) H 2 (g) + 0.5O2 (g) → H2O (l);Δ? ((3) = -286 kJ mol-1
2. Given the enthalpy of hydrogenation of benzene (C.He reacts with Hy forming C u) (4,H"=+215 k/mol), the enthalpy of combustion of benzene (CHs reacts with O, forming Co, and H.0) (A_H" = -3268 kJ/mol and the reaction enthalpy of water decomposition (liquid H2O becomes Hy and Orgases) (A,Hº = +286 kJ/mol, what is the enthalpy of combustion of cyclohexane (4 H°). (hint: write all balanced equations, use Hess' Law) (15 pts)
Self-test 3.7 Use standard enthalpies of formation to calculate the enthalpy of combustion of propane gas to carbon dioxide and water vapour. Answer: -2220 kJ mol-1
Example Problem Calculate the enthalpy (AH°, ) of combustion of Benzene, CH6. rxn C6H615/2 O2 (8)6CO2 (g) + 3H2O AH°, [C6H6= 49.0 kl/mol AH°% [CO2(@)= -393 .5 kJ/mol AHO, [H20 = -285.8 kl/mol AH', [O2@= 0 kl/mol
A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184...
Calculate the enthalpy change, Delta H process in which 32.5 g water is converted from liquid at 18.9 C to vapor 25.0 degrees C. For water Delta H vap =44.0 kJ/mol at 25.0 °C and Cs=4.18 J/(g*^ C) for H2O (l)
the complete combustion of candle wax (C31H64) in oxygen produced co2 and liquid water. calculate the work associated with this combustion reaction at 298k in kj/mol
The heat of combustion of liquid C2H60 is -1460.4 kJ/mol at 298K. Thermodynamic tables Note, tolerance on this problem is set to 1% so maintain all decimal digits as given or found in Thermodynamic Table. What is the combustion reaction to which this number applies? Instructions: • Write balanced reaction in the order: fuel + oxygen -> carbon dioxide + water (H20) • Use -> (hyphen + greater than) for yields • Do not include the states, i.e., no (s),...
Part A Calculate the enthalpy change, ΔH, for the process in which 42.4 g of water is converted from liquid at 15.3 ∘C to vapor at 25.0 ∘C . For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and Cs = 4.18 J/(g⋅∘C) for H2O(l). How many grams of ice at -16.2 ∘C can be completely converted to liquid at 25.5 ∘C if the available heat for this process is 4.77×103 kJ ? For ice, use a specific heat of...