. 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.

With reference to the following equationN2(g) + 3 H2(g) 2 NH3(g)Heat of reaction = -92 kJ/molWhich statement is correct?92 kJ is the quantity of heat which isQuestion 6Select one:a.lost to the surroundings when 1 mol of hydrogen is consumedb.lost to the surroundings when 1 mol of ammonia is formedc.lost to the surroundings when 2 mol of ammonia are formedd.gained from the surroundings when 1 mol of hydrogen is formede.gained from the surroundings when 2 mol of ammonia are formed

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

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

For many purposes we can treat ammonia NH3 as an ideal gas at temperatures above its boiling point of −33.°C.Suppose the pressure on a 22.0g sample of ammonia gas at −9.00°C is doubled.