Problem: 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 kJCalculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.a. -94.6 kJb. 32.7 kJc. 0.0306 kJd. -9.46 × 104 kJe. -0.0106 kJ

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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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