Estimate the standard enthalpy change (Delta H_(rxn)^circ ) of the reaction D using reactions A-C A) NH_(3)arrow N_(2)+H_(2)Delta H_(rxn)^circ =+92kJ/mol B) H_(2)Oarrow H_(2)+O_(2)Delta H_(rxn)^circ =+572kJ/mol C) N_(2)+O_(2)-NO Delta H_(rxn)^circ =-180kJ/mol D) NH_(3)+O_(2)-gt NO+H_(2)O Delta H_(rxn)^circ -?

To estimate the standard enthalpy change $(\Delta H_{rxn}^{\circ })$ of reaction D using reactions A-C, we can manipulate the given reactions to match the products and reactants of reaction D.<br /><br />First, let's manipulate reaction A to obtain $NO$ as a product:<br />$NH_{3}\rightarrow N_{2}+H_{2}\quad \Delta H_{rxn}^{\circ }=+92kJ/mol$<br /><br />Next, let's manipulate reaction C to obtain $H_{2}O$ as a product:<br />$N_{2}+O_{2}\rightarrow NO\quad \Delta H_{rxn}^{\circ }=-180kJ/mol$<br /><br />Now, we can add the manipulated reactions A and C to obtain reaction D:<br />$NH_{3}+O_{2}\rightarrow NO+H_{2}O\quad \Delta H_{rxn}^{\circ }=+92kJ/mol + (-180kJ/mol) = -88kJ/mol$<br /><br />Therefore, the estimated standard enthalpy change $(\Delta H_{rxn}^{\circ })$ of reaction D is $-88kJ/mol$.