Question

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.

Answer 1

94.56KJ

Step-by-step 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