Question

In a previous le, you calculated the standard entropy change for the combustion of 1 mole of diamond at room temperature. What is the standard free energy change for the same process? Please answer in kJ/mol and report your answer to one place past the decimal. C (s, diamond) + O₂ (g) → CO₂ (g)

Answer 1

The standard free energy change for the combustion of diamond cannot be directly calculated without the standard enthalpy change value.

Step-by-step explanation:

The standard free energy change, ΔG°, for a process can be calculated using the equation ΔG° = ΔH° - TΔS°, where ΔH° is the standard enthalpy change, T is the temperature in Kelvin, and ΔS° is the standard entropy change.

For the combustion of 1 mole of diamond at room temperature, the standard entropy change, ΔS°, was calculated previously. To determine the standard free energy change, we need the standard enthalpy change, ΔH°. Unfortunately, the given information does not include the value of ΔH°.

Therefore, it is not possible to directly calculate the standard free energy change for the combustion of diamond using the given information.