# Problem: Nitric axide (NO) reacts with oxygen gas to form nitrogen dioxide (NO 2) a dark brown gas:2NO(g) + O2(g) → 2NO2(g)In one experiment. 0.893 mol of NO is mixed with 0.519 mol of O 2. Determnine which of the two reactants is the limiting reactant. Calculate also the number if moles NO2 produced.(A) Limiting reactant(B) moles of NO2 produced

###### FREE Expert Solution

We´re asked to determine the limiting reactant in the reaction of 0.893 moles of NO with 0.519 moles of O2, and the number of moles of NO2 produced.

Consider that the limiting reactant is the one that’s consumed completely in the reaction and forms the less amount of product, and the excess reactant is the one that remains after the reaction is completed and forms the most amount of product.

The problem can be solved in 2 steps:

Step 1: Calculate the number of moles of NO2 produced by each reactant.

###### Problem Details

Nitric axide (NO) reacts with oxygen gas to form nitrogen dioxide (NO 2) a dark brown gas:

2NO(g) + O2(g) → 2NO2(g)

In one experiment. 0.893 mol of NO is mixed with 0.519 mol of O 2. Determnine which of the two reactants is the limiting reactant. Calculate also the number if moles NO2 produced.

(A) Limiting reactant

(B) moles of NO2 produced