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# 7.   Calculate the heat of following reaction      N2 + 3H2 —> 2NH3      Given the bond energies of N = N, H - H and N ¾ H bonds are 226, 104 and 93 kcal respectively.8.   When 2 moles of C2H6 are completely burnt 3129 KJ of heat is liberated. Calculate the heat of formation, ΔHf for C2H6; ΔHf for CO2­ and H2O are -395 and -286 KJ respectively.9.   Calculate the heat of formation of ethane at 25°C. The bond enthalpies for H - H, C - C and C -H bonds are 104.2 kcal, 80 kcal and 99.5 kcal respectively. Heat of vaporization of carbon is 171.7 kcal. 10. Define the following terms:      (a) Internal energy            (b) Endothermic reaction      (c) Hess law                    (d) Calorific value11.5 mole of an ideal gas expand isothermally & reversibly from a pressure of 10 atm to 2 atm at 300 K. What is the largest mass which can be lifted through a height of 1 mitre in this expansion?12.The equilibrium constant for the reaction:      CO2(g) + H2(g) ——> CO(g) + H2O at 298 K is 73. Calculate the value of the standard free energy change (R = 8.314 JK-1mol-1).13.An insulated container contains 1 mole of a liquid molar volumes 100 ml at 1 bar. When liquid is steeply passed to 100 bar, volume decrease t0 99 ml, find ΔH & ΔU for the process.

## 1 Answers

9 years ago

7.  1*226+3*104=638kcal gives total energy of the reactants

in NH3 3 N-H bonds are present

So, 3*93=279kcal

but there are 2 NH3 molecules

therefore

2*279=558kcal

net heat=558-638=-80kacl

which shows reaction is exothermic.

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