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 DH = - 890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

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20 January, 17:06

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Damaris Tanner · Answer 1

94.56KJ

Explanation:

1.7 grams of CH4 contains 1.7/16 moles of CH4.

If 1 mole of CH4 give 890KJ

1.7/16 moles of CH4 gives 1.7/16*890 = 94.56KJ

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 DH = - 890.0 kJCalculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.