how much energy is given off when 2.00 mol of CH4 are burned?
-444.2
To determine the amount of energy released when 2.00 mol of CH4 (methane) is burned, we need to use the concept of the heat of combustion of methane. The heat of combustion is the amount of energy released when one mole of a substance is completely burned.
The chemical equation for the combustion of methane (CH4) is as follows:
CH4 + 2O2 → CO2 + 2H2O
From the balanced equation, we can see that for every mole of methane burned, one mole of carbon dioxide (CO2) is produced. The heat of combustion of methane is approximately -890.3 kJ/mol.
To find the amount of energy released when 2.00 mol of CH4 is burned, we multiply the number of moles by the heat of combustion:
Energy released = 2.00 mol × -890.3 kJ/mol
Calculating this expression, the answer is -1780.6 kJ. The negative sign indicates that energy is being released, as in an exothermic reaction.
Therefore, when 2.00 mol of CH4 is burned, approximately 1780.6 kJ of energy is released.