How much heat is required to raise the temperature of 1.50 g of water from 25 de

Question

How much heat is required to raise the temperature of 1.50 g of water from 25 degree C to 100 degree C? The propane fuel (C_3H_8) used in gas barbeques burn according to the thermochemical equation C_3H_8 (g) + 5O_2 (g) rightarrow 3CO_2 (g) + 4 H_2O (g) Delta H = -2217 kJ How much heat would be released by the combustion of 155.5 g of propane? When 1 mole of a gas fuel is burned at constant pressure, it produces (releases) 3452 kJ heat and does 11 kJ of work. What are the values of the Delta E and Delta H for the combustion of the fuel? Is the combustion of the fuel in (a) an exothermic or endothermic process?

Explanation / Answer

deltaU= Q+W

W = Work done. it is +ve when done on the system and -ve when done by the system

Q= heat is relased means it is -ve

deltaU= -3452-11= -3463 KJ

H= U+PV

deltaH= deltaU + PdV ( since P is constant)= deltaU-11 = -3463-11= 3474 KJ

since enthalpy is -ve, combustion of fuel is exothermic.

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