89.1k views
2 votes
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)

1 Answer

1 vote

Final answer:

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.

User Zeroboo
by
8.4k points
Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.