(Solved): How much heat is transferred per mole of \( \mathrm{NH}_{3}(\mathrm{~g}) \) formed in the reaction ...

How much heat is transferred per mole of \( \mathrm{NH}_{3}(\mathrm{~g}) \) formed in the reaction shown below? Hint: Thermostoichiometry. \[ \mathrm{N}_{2}(\mathrm{~s})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_{3}(\mathrm{~s}) \quad \Delta H^{\circ}=-92.2 \mathrm{~kJ} \] \( 46.1 \mathrm{~kJ} \) \( +92.2 \mathrm{~kJ} \) \( -46.1 \mathrm{~kJ} \) \( +15.4 \mathrm{~kJ} \) \( -30.7 k J \) The enthalpy of reaction for \( \mathrm{H}_{2}(\mathrm{~g}) \) and \( \mathrm{Cl}_{2}(\mathrm{~g}) \) is listed below \[ \mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{HCl}(\mathrm{g}) \quad \Delta \mathrm{H}^{\circ}=-186 \mathrm{~kJ} \] What is the of \( \Delta \mathrm{H}^{\circ}{ }_{\mathrm{f}}(\mathrm{kJ} / \mathrm{mol}) \) for \( \mathrm{HCl}(\mathrm{g}) \) ? Given \[ \begin{array}{l} -1.27 \times 10^{2} \\ +186 \\ -3.72 \times 10^{2} \\ -93.0 \\ -186 \end{array} \] How much heat is absorbed/released when \( 20.00 \mathrm{~g} \) of \( \mathrm{NH}_{3}(\mathrm{~g}) \) reacts in the presence of excess \( \mathrm{O}_{2}(\mathrm{~g}) \) to produce \( \mathrm{NO}(\mathrm{g}) \) and \( \mathrm{H}_{2} \mathrm{O}(i) \) according to the following chemical equation? Hint: Thermostoichiometry. \[ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(\mathrm{~s}) \rightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \quad \Delta \mathrm{H}^{\circ}=+1168 \mathrm{~kJ} \] \( 342.9 \mathrm{~kJ} \) of heat is released. \( -546.39 \mathrm{~kJ} \) \( 1372 \mathrm{~kJ} \) of heat are absorbed. \( 342.9 \mathrm{~kJ} \) of heat are absorbed. \( 1372 \mathrm{~kJ} \) of heat is released.