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# 1.   Calculate the C ¾ H bond energy in methane at 25°C from the data. Heat of formation of methane is -17.9 kcal, heat of vaporization of carbon is 171.1 cal and heat of formation of hydrogen atoms is 52.1 kcal/mol.2.   The heats of combustion of hydrogen, ethane and ethylene are 68.4, 370.4 and 393.5 kcal per molecule respectively. Calculate the energy when ethylene is reduce to ethane.3.   The molar heat of formation of NH4NO­3 is 367.54 KJ and those of N2O(g) and H2O are 81.46 KJ and -285.78 KJ, respectively at 25°C and 1.0 atm pressure. Calculate ΔH and ΔE for the reaction.         NH4NO3(s) ———> N2O (g) + 2H2O(l)4.   Given that                                                                 N2(g) + l2 (g) ———> 2Hl(g)           ΔH = –12.46 kcal        l2(g)  ———> 2l(g)                        ΔH = 35.8 kcal         H2(g) ———> 2H(g)                       ΔH = 103.7 kcal            Calculate the bond energy of H – I5.   Calculate the maximum work done when pressure on 10 g of hydrogen is reduced from 20 to 1 atm at a constant temperature of 273 K. The gas behaves ideally. Calculate Q.6.   Standard heat of formation of HgO(s) at 298 K and at constant pressure is -90.8 kJ / mole. Excess of HgO(s) absorbs 41.84 kJ of heat at constant volume, calculate the amount of Hg that can be obtained at constant volume and 298 K, Atomic weight of Hg = 200.7.   Calculate the heat of formation of anhydrous Al2Cl6 from      2Al(s) + 6HCl (aq) ——> Al2Cl6(aq) + 3H2(g),               ΔH = –239.76 kcal      H2(g) + Cl2  ——> 2HCl(g)                                          ΔH = –44.0 kcal      HCl(g) + Aq  ——> HCl(aq.)                                       ΔH = –17.32 kcal      Al2Cl6(s) + Aq  ——> Al2Cl6(aq.)                               ΔH = –153.69 kcal8.   Calculate the heat of formation of Ag2O from following data:9.   Calculate resonance energy of from the following data if the observed heat of formation of is -439.7 kJ.      Bond Energy                             Heat of atomisation (kJ)      C – H = 413                                        C = 716.7      C – C = 348                                        H = 218.0      C = O = 732                                       O = 249.1      C – O = 351              O – H = 463        10.For a reaction, ΔH = 30 KJ mol-1 and ΔS = 0.07 KJ K-1 mol-1 at 1 atm. Calculate upto which temperature, the reaction would not be spontaneous.

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