The table shows the heat of combustion for four compounds - HSC - SSCE Chemistry - Question 11 - 2013 - Paper 1

To determine which compound produces the greatest amount of energy when burned, we need to consider the heat of combustion values provided in the table. The heat of combustion indicates the amount of energy released per mole of the compound when it is combusted.

1. Calculate the molar masses of each compound:

   • CO: 12.01 g/mol (C) + 16.00 g/mol (O) = 28.01 g/mol
   • CH₄: 12.01 g/mol (C) + 4(1.008 g/mol (H)) = 16.04 g/mol
   • C₂H₂: 2(12.01 g/mol (C)) + 2(1.008 g/mol (H)) = 26.04 g/mol
   • C₂H₆: 2(12.01 g/mol (C)) + 6(1.008 g/mol (H)) = 30.07 g/mol

2. Determine the energy released for 1.00 g of each compound:

   • For CO:

   • For CH₄:

   • For C₂H₂:

   • For C₂H₆:

3. Compare the energies produced per gram to identify the maximum:

   • Using the heat of combustion values:
     • CO:
     • CH₄:
     • C₂H₂:
     • C₂H₆:

Based on the calculations, C₂H₆ (Ethane) has the highest heat of combustion (1560 kJ/mol), and therefore is expected to produce the greatest amount of energy when 1.00 g is burned.