How do I solve this, please be detailed

Question

If 25.0g of NH₃ and 45.0 g of O_{2 react in the following reaction, what is the mass in grams of NO that will be formed?}

4NH_3(g) + 5O_{2 (g) = 4}NO (g) + 6H₂O(g)

Answer 1

4NH_3(g) + 5O_{2 (g) ==>} 4NO (g) + 6H₂O(g) ... balanced equation

Looking at the balanced equation we see that 4 MOLES of NO can be produced from 4 MOLES NH₃ and from 5 MOLES of O_2. Whenever you are given the quantities of BOTH reactants, you will be dealing with a limiting reactant problem. We must find out which, if any, reactant is limiting.

For NH3: 25.0 g NH₃ x 1 mol NH₃/17 g x 4 mol NO/4 mol NH₃ x 30 g NO/mol = 44.1 g NO produced

For O₂: 45.0 g O₂ x 1 mol O₂/32 g x 4 mol NO/5 mol O₂ x 30 g NO/mol = 33.8 g NO produced

In this case, O₂ is limiting and 33.8 g of NO will be produced