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

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

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