We are given the following reaction:
SO2(g) + 2 H2S(g) ⇌ 3 S(s) + 2 H2O(g)
We are asked to do the following:
Find the equilibrium constant, k.
Recall that ΔG˚rxn and K are related to each other:
We can use the following equation to solve for ΔG˚rxn:
In determining k, we need to do the following steps:
Step 1: Calculate for ΔG˚rxn.
Step 2: Calculate for K.
Step 1: Calculate for ΔG˚rxn:
ΔG˚f, SO2(g) = – 300.4 kJ/mol
ΔG˚f, H2S(g) = – 33.01 kJ/mol
ΔG˚f, S(s) = 0 kJ/mol
ΔG˚f, H2O(g) = – 228.57 kJ/mol
The reaction SO2(g) + 2H2S(g) ⇌ 3S(s) + 2H2O(g) is the basis of a suggested method for removal of SO2 from power-plant gases. The standard free energy of each substance are
ΔGf°S(s) = 0 kJ/mol
ΔGf°H2O(g) = -228.57 kJ/mol
ΔGf°SO2(g) = -300.4 kJ/mol
ΔGf° H2S (g) = -33.01kJ/mol
What is the equilibrium constant for the reaction at 298K?
In principle, is this reaction a feasible method of removing SO2?
If Pressure of SO2 = Pressure of H2S and the vapor pressure of water is 26 torr, calculate the equilibrium SO 2 pressure in the system at 298 K.
Would you expect the process to be more or less effective at higher temperatures?
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 professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Fakhreddine's class at TEXAS.