Hydrogen Cyanide gas is produced industrially by this reaction: 2 CH4(g) + 3 O2(g) + 2 NH3(g) --> 2 HCN(g) + 6 H2O(g)

What volumes of O2(g) and NH3(g) are needed to react with 8.0 L of CH4(g) at STP?

Consider the following reactions. (note: (s) = solid, (l) = liquid, and (g) = gas.) mg(s) + ½o2(g) → mgo(s) + 146 kcal/mole h2(g) + ½o2(g) → h2o(g), δh = -57.82 kcal/mole what type of reaction is represented by the previous two examples?