We’re being asked to determine the relationship of spontaneity or standard free energy change (ΔG) and high temperature (635 K) for the reaction:
Fe2O3(s) + 3 H2(g) ⇌ 2 Fe(s) + 3 H2O(g), ΔG° = 53 kJ at 25 °C and ΔH° = 100 kJ
In this case, we can determine ΔS and use the relationship between ΔS and ΔH.
We can calculate for ΔS using the following equation:
For the reaction, Fe2O3(s) + 3 H2(g) <=> 2 Fe(s) + 3 H2O(g), ΔG° = 53 kJ at 25 °C and ΔH° = 100 kJ. Which of the following is completely true about the relationship between ΔG and T for this reaction?
a. ΔG < 0 when T > 635 K
b. ΔG < 0 when T < 635 K
c. ΔG < 0 at all temperature
d. ΔG = 0 when T < 635 K
e. ΔG = 0 when T > 635 K
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 ofFor the reaction, Fe2O3(s) + 3 H2(g) <=> 2 Fe(s) + 3 H...as medium difficulty.