Two moles of ammonia is introducedi in an evacuated 500 ml vessel at high temperature. The decomposition reaction is : 2NH3 ->N2 +3H2 at the equillibrium NH3 becomes 1 mole then the 'K' would be:

4. Give the thermochemical equation for the decomposition of ammonia, NH3.NH3 (g) —> 3/2 H2 (g)  + 1/2 N2 (g)                    ΔH = 29.61 kJ*3 pointsNH3 (g) —> 3/2 H2 + 1/2 N2 (g) + 29.61 kJNH3 (g) + 29.61 kJ —> 3/2 H2 + 1/2 N2 (g)NH3 (g) —> 3/2 H2 + 1/2 N2 (g) - 29.61 kJNH3 (g) - 29.61 kJ —> 3/2 H2 + 1/2 N2 (g)Is the reaction in no. 4  endothermic or exothermic?*2 pointsendothermicexothermic

. The thermochemical equation showing the formation of ammonia, NH3 from its elements is:N2 (g) + 3 H2 (g) —> 2 NH3 (g)            ΔH = -92 kJThis equation shows that 92 kJ of heat is ____.*2 pointsabsorbed from the surroundings.released to the surroundings.

Q2How many moles of ammonia are produced from 0.60 moles of nitrogen? N2 (g) + 3 H2 (g) yields 2 NH3 (g)2 marks0.60.21.20.3

When ammonia burns in air, nitrogen dioxide and water are produced according to the reaction below:4 NH3(g) + 7 O2(g) → 4 NO2(g) + 6 H2O(l)At 0 °C and 1 atm pressure, burning 44.8 L of ammonia requires:A.6/7 moles O2.B.8/7 moles O2.C.7/4 moles O2.D.7/2 moles O2.

The enthalpy of formation of NH3 is – 46. The enthalpy change for the reaction: 2NH3 → N2 + 3H2 is ?46 KJ92 KJ–23 KJ     –92 KJ