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.

Gaseous ammonia chemically reacts with oxygen O2 gas to produce nitrogen monoxide gas and water vapor. Calculate the moles of nitrogen monoxide produced by the reaction of 0.10mol of oxygen. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

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.

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

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