Consider the reaction at equilibrium: 2H2O(g) -----> 2H2(g) + O2(g) Hrxn > 0 Pre

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.

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