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(a) Distinguish clearly between the terms mean bond energy and bond dissociation energy.
Use the following reactions in your answer:
H2O(g) H(g) + OH(g)
OH(g) H(g) + O(g) (3 marks)
(b) From the mean bond enthalpy data given below, estimate the enthalpy change for the complete combustion of two moles of C2H6 (g) at 298 K. (The molar enthalpy of vaporization of water is 45.0 kJ mol-1 at 298K).
2C2H6 + 14 O2 --------------------- 4CO2 + 6H2O
Reactants - Products
Bond CH O=O OH C=O CC
Bond enthalpy/kJ mol1 414 499 460 799
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(c) A sample of naphthalene C10H8 (s), is completely burned in a bomb calorimeter at 298K. The calorimeter constant (heat capacity) is 70.5 J K1. The standard molar enthalpy of combustion of naphthalene is ΔcHo = – 5157 kJ mol1.
(i) Write a balanced chemical equation for the combustion reaction.
C10H8 + 7O2 5CO2 + 4H2O
(ii) Calculate DeltaUo for the reaction.
(iii) If the sample contains 200 mg naphthalene, calculate the heat released during the reaction, and hence calculate the temperature change of the calorimeter.
(d) Calculate the heat required to melt 500 kg of potassium metal at 336 K.
The enthalpy of fusion of potassium is 2.35 kJ mol1.