In the Presence of Excess Oxygen,methane Gas Burns in a Constant

In the presence of excess oxygen,methane gas burns in a constant pressure system to yield carbon dioxide and water: $\mathrm { CH } _ { 4 }$ (g) + $2 \mathrm { O } _ { 2 }$ (g) ? $\mathrm { CO } _ { 2 }$ (g) + $2 \mathrm { H } _ { 2 }$ O (l) $\Delta _ { \mathrm { r } }$ H = -890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure.

A) -0.00946 kJ $\mathrm { mol } ^ { - 1 }$
B) 0.0342 kJ $\mathrm { mol } ^ { - 1 }$
C) -1.06 × $10 ^ { - 5 }$ kJ $\mathrm { mol } ^ { - 1 }$
D) 29.3 kJ $\mathrm { mol } ^ { - 1 }$
E) -106 kJ $\mathrm { mol } ^ { - 1 }$