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. 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 but Keq will will increase The equilibrium will shift toward reactant but Keq will decrease (b) The reaction mixture is cooled. (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.
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 but Keq will will increase
The equilibrium will shift toward reactant but Keq will decrease
(b) The reaction mixture is cooled.
(c) The volume of the reaction vessel is reduced by 50%.
Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on chemical equilibrium. This principle states that when any system is at equilibrium and if we change in concentration, temperature, or pressure, the system changes to a new equilibrium to cancel the change.
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