posted by Angie on .
What is the amount of H2O that can be produced by combining 89.7 of each reactant in the following equation:
4NH3(g) + 5O2 (g)----> 4NO(g) + 6 H2O(g)
A limiting reagent problem; you know that because amounts are given for BOTH reactants.
mols NH3 = grams/molar mass.
mols O2 = grams/molar mass.
Using the coefficients in the balanced equation, convert mols NH3 to mols H2O.
Do the same for mols O2.
It is likely these two values will not be the same which means one of them is wrong. The correct value in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.
Now convert mols to grams. g = mols x molar mass