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

To find the energy produced by burning 1.00 g of C₂H₆, we first need the molar mass of C₂H₆:

• Molar mass of C₂H₆ = 2(12.01 g/mol for C) + 6(1.008 g/mol for H) = 30.07 g/mol.

Next, we calculate the moles in 1.00 g of C₂H₆:

$ext{moles of C₂H₆} = \frac{1.00 ext{ g}}{30.07 ext{ g/mol}} \approx 0.0332 ext{ mol}$

Finally, we calculate the total energy produced:

$ext{Energy} = ext{moles} \times \text{heat of combustion} = 0.0332 ext{ mol} \times 1560 ext{ kJ/mol} \approx 51.79 ext{ kJ}$

Thus, burning 1.00 g of C₂H₆ would produce approximately 51.79 kJ of energy.