Reaction equation:

NH3(g) + O2(g) → NO(g) + H2O(g)

Given:

Amount of gas taken initially = 13.6 moles

Steps to solve the problem:

1. Determine the limiting reactant:

The limiting reactant is the reactant that is completely consumed in the reaction and limits the amount of product that can be formed. To determine the limiting reactant, we need to compare the number of moles of each reactant with their stoichiometric coefficients in the balanced equation.

The stoichiometric coefficients of NH3 and O2 are 1 and 1, respectively. Therefore, the number of moles of NH3 and O2 taken initially are both 13.6 moles.

NH3(g) + O2(g) → NO(g) + H2O(g)

Since the stoichiometric coefficients of NH3 and O2 are equal, they are both the limiting reactants.

2. Calculate the amount of product formed:

Since both NH3 and O2 are limiting reactants, we need to calculate the amount of product formed from each of them and choose the smaller value as the actual yield.

From the balanced equation, we can see that 1 mole of NH3 produces 1 mole of NO. Therefore, the amount of NO produced from 13.6 moles of NH3 is also 13.6 moles.

From the balanced equation, we can see that 1 mole of O2 produces 1 mole of NO. Therefore, the amount of NO produced from 13.6 moles of O2 is also 13.6 moles.

Therefore, the actual yield is 13.6 moles of NO.

Answer:

The amount of NO produced when 13.6 moles of NH3 and O2 are taken initially is 13.6 moles.

A