Part A: Use the data given here to calculate the values of ΔG°_{rxn} (kJ/mol) at 25 °C for the reaction described by the equation:** **

A + B ⇌ C

A ΔG°_{f }= +387.7 kJ/mol

B ΔG°_{f }= +529.5 kJ/mol

C ΔG°_{f }= +402.0 kJ/mol

Part B: If ΔH°_{rxn} and ΔS°_{rxn} are both positive values, what drives the spontaneous reaction and in what direction at standard conditions?

a) enthalpy-driven to the left

b) entropy-driven to the left

c) entropy-driven to the right

d) enthalpy-driven to the right

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty of*Part A: Use the data given here to calculate the values of Δ...*as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 5 minutes and 36 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Addo-Mensah's class at TAMIU.