Consider the reaction below. If 8.75 g of CH4 reacts with 18.95 g of O2 and 6.85 g of H2O is collected, what is the percent yield of H2O? Show clear work. [Atomic masses: C = 12.01 g, H = 1.008 g, O = 16.00 g] CH4 + O2 _ CO2 + H2O (unbalanced).

Liquid ammonia is produced at high temperatures and under great pressure in a tank by passing a mixture of nitrogen gas and hydrogen gas over an iron catalyst. the reaction is represented by the following equation. n2(g) + 3h2(g) → 2nh3(g) changing all but one experimental condition will affect the amount of ammonia produced. that condition is a) increasing the concentration of both reactants b) changing the temperature within the tank c) decreasing the pressure within the tank. d) increasing only the amount of nitrogen present.