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.

Answer 1

To calculate the standard free energy change for the combustion of 1 mole of diamond at room temperature, you need to know the standard enthalpy change. Using the equation ∆G° = ∆H° - T∆S°, where ∆H° is the standard enthalpy change and ∆S° is the standard entropy change, you can find the standard free energy change.

Step-by-step explanation:

The student wants to know the standard free energy change for the combustion of 1 mole of diamond at room temperature. The standard free energy change (∆G°) can be determined using the equation: ∆G° = ∆H° - T∆S°, where ∆H° is the standard enthalpy change and ∆S° is the standard entropy change. If we have already calculated the standard entropy change for the combustion of 1 mole of diamond at room temperature, we can use that information to calculate the standard free energy change.

Let's assume that the standard entropy change (∆S°) for the combustion of 1 mole of diamond at room temperature is -10 J/(mol·K). We can use the equation ∆G° = ∆H° - T∆S°, where T is the temperature in Kelvin. At room temperature, T is approximately 298 K.

So, if we have the enthalpy change, we can calculate the standard free energy change (∆G°). However, the question doesn't provide the enthalpy change, so we cannot provide a specific value for the standard free energy change.