
Hydrogen sulfide (H2S) is a contaminant commonly found m natural gas. It is removed by reaction with oxygen to produce elemental sulfur.
For each of the following scenarios, determine whether the equilibrium will shift to the right, shift to the left, or neither: (a) addition of O2(g), (b) removal of H2S(g), (c) removal of H2O(g), and (d) addition of S(s).

Interpretation:
The equilibrium directions should be identified for the given Hydrogen Sulfide (H2S) equilibrium reaction with different conditions.
Concept Introduction:
Concept of equilibrium process: Any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed. This equilibrium can be explained in a simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.
Le Chatelier's Principle: A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change. In other words the closed system is an increase in pressure; the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.
Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions.
Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.
Homogeneous equilibrium: A homogeneous equilibrium involved has an everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.
Answer to Problem 15.15WE
The equilibrium directions for given the statements of addition, removal and temperature reactions are given below.
Explanation of Solution
To Identify: Given the equilibrium reactions (a and b) addition, removal of (O2 and H2S) should be analyzed.
Given both reactions (a and b) equilibrium directions must be analyzed.
Before identification of equilibrium directions we writing the reaction quotient (Qc) expression fallowed.
Here (S) will not appear in the expression, because sulfur is solid.
Let us consider the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.
The given equilibrium reaction (
Analyzing for reaction (a): The given reaction if we addition of sufficient amount (O2) this process will undergoes for right side, process will be re-established in such a way that Qc is again to the equilibrium constant, highest mole amount of product (S) will form. Hence the system of equilibrium shifted to the right side to established concentration equilibrium.
Analyzing for reaction (b): The given reaction if we addition of sufficient amount hydrogen sulfide this process will undergoes for left side, process will be re-established in such a way that Qc is again to the equilibrium constant, lowest amount of product (S) will form. Hence the system of equilibrium shifted to the left side to established concentration equilibrium.
Explanation:
To Identify: Given the equilibrium reactions (c and d) addition, removal of (
Given both reactions (c and d) equilibrium directions must be analyzed.
Here also we will identify given the reaction process, Le Chatelier's Principle to determine which of the following process will cause the equilibrium shift to the right or left.
Reaction (c): Above the removal process of (
Reaction (b): The given reaction if we addition of sufficient amount (
The equilibrium directions were identified given the hydrogen sulfide (H2S) addition and removal reaction with respective conditions.
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Chapter 15 Solutions
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