Write the K expression for the following reaction

(1) One of the steps in the commercial process for converting ammonia to nitric acid involves the conversion of ammonia, NH3(g) to nitrous oxide, NO(g). 4 NH3(g )  +  5 O2(g)  → 4  NO(g)  +  6 H2O(l) Atomic weights (g/mol): N=14, H=1, O=16 a. Balance the above chemical equation that represents the conversion. b. How many moles of oxygen are needed to convert 2.5 moles of ammonia? c. How many grams of water will be produced from 2.5 moles of ammonia? d. If 150 grams of oxygen reacted 2.5 moles of ammonia, identify the limiting and excess reagents. e. How much of the excess reagent remains unreacted? f. If the reaction in (d) produces 10.0 grams of nitrous oxide, calculate the percent yield.

Hexamethylenediamine (CH16N2) is one of the starting materials for the production of nylon. It can be prepared from adipic acid (CH1004) by the following overall reaction: C6H1004(1) + 2 NH;(g) + 4 H2(g) – CH16N2(1) + 4 H,0()

Balance the cquation C,H18() + 0>(g)→ CO,(g) + H;O(g) CO,(g) + H,0(g)