A theoretical recipe and an actual recovered product — Physical Science: Chemistry

A balanced equation supplies a relative-amount recipe. With 2.00 mol N₂ and 3.00 mol H₂ in the selected complete ammonia model, hydrogen supports only 2.00 mol NH₃ while 1.00 mol N₂ remains. Choosing a limiting reactant by smaller starting mass ignores molar mass and the coefficient ratio. Compare each starting amount through its capacity to form the same product.

If the recovered ammonia is 1.60 mol, the selected yield is 80.0% of the 2.00 mol theoretical amount. That does not prove exactly twenty percent of every reactant stayed unchanged. Incomplete conversion, side products and isolation losses are different explanations. Analyze composition before isolation and the purity/amount recovered afterward to distinguish them.

Solutions add another conversion rather than a different conservation principle. Concentration times liters gives the specified solute amount; dissociation can supply several reacting ions per formula unit. Apply the reaction ratio, determine leftovers, then divide by final mixture volume if a concentration is requested. Keep assumptions about purity, extent and volume addition visible.