Question

Ammonia may be oxidised to nitrogen monoxide in the presence of catalyst according to the equation 4 NH3 + 5 O2 gives 4 NO and 6 H2O. If 27 litres of reactants are consumed , what volume of nitrogen monoxide is produced at the same temperature and pressure.

Answer 1

I think this may be the right answer

Answer 2

Answer: The volume of nitrogen monoxide produced is 12 L.

Explanation:

For the given chemical reaction:

$4NH_3+5O_2\rightarrow 4NO+6H_2O$

According to the mole concept:

1 mole of a gas occupies 22.4 L of volume.

So, 9 moles of reactants (which are gases) will occupy $9\times 22.4=201.6L$ of volume.

By Stoichiometry of the reaction:

201.6 L of volume of reactants produces $(4\times 22.4)=89.6L$ of nitrogen monoxide.

So, 27 L of reactants will produce = $\frac{89.6}{201.6}\times 27=12L$ of nitrogen monoxide.

Thus, the volume of nitrogen monoxide produced is 12 L.