he equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease (c) The volume of the reaction vessel is reduced by 50%.
Consider the following equilibrium for which H = -114.44:
4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g)
How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?
(a) O2(g)) is added to the system. which will happen?
the equilibrium will not shift
the equilibrium will shift toward product but Keq will not change
the equilibrium will shift toward reactant but Keq will not change
the equilibrium will shift toward product and Keq will increase
the equilibrium will shift toward reactant and Keq will decrease
(b) The reaction mixture is cooled.
the equilibrium will not shift
the equilibrium will shift toward product but Keq will not change
the equilibrium will shift toward reactant but Keq will not change
the equilibrium will shift toward product and Keq will increase
the equilibrium will shift toward reactant and Keq will decrease
(c) The volume of the reaction vessel is reduced by 50%.
(d) A catalyst is added to the reaction mixture.
(e) The total pressure of the system is increased by adding a noble gas.
(f) Cl2(g) is removed from the system.
Given reversible equation is
4 HCl(g) + O2(g) ----------> 2 Cl2(g) + 2 H2O(g)
Enthalpy of the reaction is H= -144.44
As H is negative, the reaction is an exothermic reaction.
Note: According to Q&A guidelines of Bartleby, we are supposed to answer only the first 3 sub-parts of the given question. Accordingly, I am answering only the first 3 sub-parts a), b) and c). Kindly repost the other question as the next question.
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