Question 1

Why is the enthalpy of formation of an element zero?

Accepted Answer

The standard enthalpy of formation is the energy change to form one mole of a substance from its elements in their standard states. To 'form' an element like O₂(g) from its standard state (which is O₂(g)), there is no change, so the enthalpy change is zero by definition.

Question 2

What's the difference between the cycles for formation and combustion data?

Accepted Answer

For formation data, the cycle's intermediate step is the constituent elements, and the arrows point 'up' from the elements to the reactants and products. For combustion data, the intermediate step is the combustion products (CO₂ and H₂O), and the arrows point 'down' from the reactants and products to these products.

Question 3

Can I use a mix of formation and combustion data in one calculation?

Accepted Answer

While theoretically possible if you construct a very complex cycle, it is not a standard method and is highly prone to error. For A-Level Chemistry, you will always be given a consistent set of data – either all formation or all combustion values needed for the calculation.

Question 4

What if a substance in the equation is an element, like in the hydrogenation of ethene?

Accepted Answer

When using formation data ($\Delta H_f^\ominus$), the value for the element (e.g., H₂(g)) is zero. When using combustion data ($\Delta H_c^\ominus$), the element will have a non-zero value (e.g., the enthalpy of combustion of hydrogen is -286 kJ mol⁻¹), which you must include in your calculation.

Hess's law

What you need to know

The Chemical Detour