The following sequence of reaction occurs in commercial production of aqueous nitric acid.

$$\begin{gathered} 4N{H}_3\left(g\right)+5O_2\left(g\right)\stackrel{ }{\to }4NO\left(g\right)+6H_{2}O\left(l\right)\Delta H=-904KJ\mathrm{........}\left(1\right) \\ 2NO\left(g\right)+O_2\left(g\right)\stackrel{ }{\to }2N{O}_2\left(g\right)\Delta H=-112KJ\mathrm{........}\left(2\right) \\ 3N{O}_2\left(g\right)+H_{2}O\left(l\right)\stackrel{ }{\to }2HN{O}_3\left(aq\right)+NO\Delta H=-140KJ\mathrm{........}\left(3\right) \end{gathered}$$

Determine the total heat liberated (in KJ/mol) at constant pressure for the production of  exactly 1 mole of aqueous nitric acid from  $N{H}_3$ by this process.