Question

If 8.00 moles of NH₃ of and 10.00 moles of O₂ react in the following reaction, how many moles of which reactant will be left over? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)

A) 2.00 mol O₂
B) 2.00 mol NH₃
C) 8.00 mol NO
D) no moles will be left over of either reactant because both are limiting.

Answer 1

Option (D) no moles will be left over of either reactant because both are limiting

Step-by-step explanation:

The balanced equation for the reaction is given below:

4NH₃(g) + 5O₂(g) → 4NO(g) + 6H₂O(g)

From the balanced equation above,

4 moles of NH₃ reacted with 5 moles of O₂.

Next, we shall determine the excess reactant. This can be obtained as follow:

From the balanced equation above,

4 moles of NH₃ reacted with 5 moles of O₂.

Therefore, 8 moles of NH₃ will react with = (8 × 5)/4 = 10 moles of O₂.

From the calculations made above, we see clearly that 10 moles of O₂ reacted completely with 8 moles of NH₃. This implies that both reactant are limiting reactant and there is no excess reactant.

Thus, no reactant is left over.