Question

Indicate how each of the following will affect the equilibrium concentration of NH3 in the following reaction: 4NH3(g)+5O2(g)?4NO(g)+6H2O(g)+906kJ

Part A

adding more O2(g)

a. The equilibrium concentration of NH3 will decrease.

b. The equilibrium concentration of NH3 will increase.

c. The equilibrium concentration of NH3 will not change.

Part B

increasing the temperature of the reaction

a. The equilibrium concentration of NH3 will increase.

b. The equilibrium concentration of NH3 will decrease.

c. The equilibrium concentration of NH3 will not change.

Part C

decreasing the volume of the container

a. The equilibrium concentration of NH3 will increase.

b.The equilibrium concentration of NH3 will decrease.

c. The equilibrium concentration of NH3 will not change.

Part D

adding more NO(g)

a.The equilibrium concentration of NH3 will decrease.

b.The equilibrium concentration of NH3 will increase.

c.The equilibrium concentration of NH3 will not change.

Part E

removing some H2O(g)

a. The equilibrium concentration of NH3 will increase.

b.The equilibrium concentration of NH3 will decrease.

c. The equilibrium concentration of NH3 will not change.

Answer 1

4NH3(g) + 5O2(g) = 4NO(g) + 6H2O(g) DELTA H = 906 KJ (endothermic)

according to le chatelier's principle when a system experiences it maintains itself to gain equilibrium accordingly.

1. adding more O2 gas reaction will go forward and the equilibrium concentration of NH3 will decrease.

2. reaction is endothermic hence increasing the temperature reaction will shift forward (product side). NH3 will decrease

3. decreasing the volume of the container will shift reaction backward (less number of moles of gas side). NH3 will increase

4. adding more NO will shift reaction backward concentration of NH3 will increase.

5. removing some H2O reaction move forward and NH3 will decrease.

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