(Solved): In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon d ...

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: \[ \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{i}) \Delta \mathrm{H}=-890.0 \mathrm{~kJ} \] Calculate the value of \( q(\mathrm{~K}) \) in this exothermic reaction when \( 1.80 \mathrm{~g} \) of methane is combusted at constant pressure. \[ \begin{array}{l} -100.1 \mathrm{~kJ} \\ 0.0324 \mathrm{~kJ} \\ -0.0100 \mathrm{~kJ} \\ 30.9 \mathrm{~kJ} \\ -1.00 \times 10^{5} \mathrm{~kJ} \end{array} \]