We’re being asked to determine which of the is completely true about the relationship between ΔG° and T for the reaction below:
Fe2O3 (s) + 3 H2(g) ⇌ 2 Fe(s) + 3 H2O(g)
ΔG° = 53 kJ at 25 °C
ΔH° = 100 kJ
The relationships given describe the spontaneity of the reaction at different temperatures. Recall that when ΔH and ΔS are given, we can determine the spontaneity of the reaction based on their signs.
We can use the Punnett square shown below:
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 when T < 635 K
d. ΔG° > 0 when T > 635 K
e. ΔG° < 0 when T > 635 K
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What scientific concept do you need to know in order to solve this problem?
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