In the Presence of Excess Oxygen, Methane Gas Burns in a Constant-Pressure

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH₄ (g) + 2O₂ (g) → + CO₂(g) + 2H₂O (l) Δ_rH = -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) -105.7 kJ mol^-1
B) 0.0342 kJ mol^-1
C) -0.0095 kJ mol^-1
D) 29.3 kJ mol^-1
E) -1.06 × 10⁵ kJ mol^-1