Limiting Reactants (Section) One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of NH3 to NO: In a certain experiment, 2.00 g of NH3 reacts with 2.50 g of O2.: (a) Which is the limiting reactant? (b) How many grams of NO and H2O form? (c) How many grams of the excess reactant remain after the limiting reactant is completely consumed? (d) Show that your calculations in parts (b) and (c) are consistent with the law of conservation of mass.
Solution 80 The reaction given above is not a balanced reaction .so first we have to balance the reaction given in the question . 4NH3 (g)+5O2(g) 4NO2(g) + 6H2O(g). From the above balanced equation we know that 4 moles of ammonia =5 moles of oxygen . Molar mass is the mass of a given chemical element or chemical compound (g) divided by the amount of substance (mol). The molar mass of a compound can be calculated by adding the standard atomic masses (in g/mol) of the constituent atoms. Molar mass of NH3=17 g Molar mass of oxygen =32g. Initial amount of NH3=2.00g Initial amount of oxygen =2.50g. Let us calculate the number of moles of reactants for the given reaction Step 1 of 4