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) ΔH = -890.0 kJ
Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.
a. -94.6 kJ
b. 32.7 kJ
c. 0.0306 kJ
d. -9.46 × 104 kJ
e. -0.0106 kJ
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