Consider the formation of nitrogen dioxide (NO ) from nitric oxide (NO2) and oxygen. 2NO(g) + O2(g) → 2NO2(g)
Suppose initially, we take 8 moles of NO and 7 moles of O2.
To determine the limiting reagent, calculate the number of moles NO2 produced from the given initial quantities of NO and O2. The limiting reagent will yield the smaller amount of the product.
Starting with 8 moles of NO, the number of NO2 produced is, 8 mol NO × \(\frac{2\,molNO_2}{2\,molNO}\) = 8 mol NO2
Starting with 7 moles of O2, the number of moles NO2 produced is, 7 mol O2 × \(\frac{2\,molNO_2}{1\,molNO}\) = 14 mol NO2
Since, 8 moles NO result in a smaller amount of NO2, NO is the limiting reagent, and O2 is the excess reagent, before reaction has started.
1. The Blackman’s law of limiting factors states that when a process is conditioned as to its rapidity by a number of separate factors, the rate of the process is...