Consider the reaction at equilibrium: 2H2O(g) -----> 2H2(g) + O2(g) Hrxn > 0 Pre
ID: 713182 • Letter: C
Question
Consider the reaction at equilibrium: 2H2O(g) -----> 2H2(g) + O2(g) Hrxn > 0 Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance.
(a) adding O2(g) makes the equilibrium __________?
(b) adding a solid phase calalyst makes the equilibrium ____________?
(c) increasing the volume of the container makes the equilibrium ___________?
(d) decreasing the temperature at constant pressure makes the equilibrium _________?
(e) adding an inert gas, He, makes the equilibrium__________?
Explanation / Answer
2H2O (g) --------------> 2H2(g) + O2(g)
Given delta H > 0 , that is endothermic reaction.
a) adding O2., a product shifts the equilibrium left (backwards)
b) addition of catalyst does not change the equilibrium.
c) increasing the volume of container , shifts the equilibrium towards more number of molecules , that is twards right side.
d) decreasing temperature favors backward reaction(exo) , that is shifts left.
e) adding inert gas
at constant volume does not change equilibrium.
at constant pressure shift right side ,w here more moles are present.