NH3 + O2 ? NO + H2O Unbalanced If at the beginning of the reaction you used 6.89

Question

NH3 + O2 ? NO + H2O

Unbalanced

If at the beginning of the reaction you used 6.89 g NH3 and 15.76 g O2, what is the theoretical yield (in grams) of NO (you will need to find the limiting reagent and then the theoretical yield of NO from this reagent)?

Explanation / Answer

example First, we balance the chemical equation. 4NH3 + 5O2 --> 4NO + 6H2O We then find the limiting reactant. For NH3: reactant = (mass / molar mass) / coefficient reactant = (4.30 g / 17.03 g/mol) / 4 reactant = 0.063 For O2: reactant = (mass / molar mass) / coefficient reactant = (15.76 g / 32.00) / 5 reactant = 0.0985 Since 0.063 < 0.0985, NH3 is the limiting reactant. Calculate for the theoretical yield. The product takes x, and the limiting reactant takes y. t.yield = (mole of y) * (coeff of x / coeff of y) * (molar mass of x) t.yield = (0.252495596) * (4 / 4) * (30.01) t.yield = 7.58 g NO (Answer)

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