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

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 1.00 g of methane is combusted at constant pressure.

a. -55.6 kJ
b. -5.56 × 104kJ
c. -0.0180 kJ
d. 55.6 kJ
e. 0.0180 kJ

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Expert Solution

queen_honey_blossom answered 2 years ago
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