6. The pressure on each of the following systems is increased by decreasing the

Question

6. The pressure on each of the following systems is increased by decreasing the volume of the container. Explain whether each system would shift left, right, or stay the same.

a. 2 SO2 (g) + O2 (g) 2 SO3 (g) (1 mark)

b. H2 (g) + I2 (g) 2 HI(g) (1 mark)

c. CaCO3 (s) CaO(s) + CO2 (g) (1 mark)

d. AgCl(s) Ag1+(aq) + Cl1- (aq) (1 mark)

How could you alter the following to make the equilibrium below shift to the left:

2CO(g) + O2(g) 2CO2(g) + 566 kJ

a) [CO]  

b) pressure

c) temperature>2NH(G)

Changing the volume of the system alters the equilibrium position of this equilibrium:N2(G)+3H2(G)------ But a similar change has no effect on this equilibrium: H2(G)+ Cl2(G)----> 2HCl (g) Explain

Explanation / Answer

6)

a)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here product has less gaseous molecule

So equilibrium will move to right

So, Equilibrium moves to product side

Answer: right

b)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is same on both side

So equilibrium will not be effected

So, No effect on equilibrium

Answer: stay the same

c)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here reactant has less gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

Answer: left

d)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here, number of gaseous molecules is 0 on both side

So equilibrium will not be effected

So, No effect on equilibrium

Answer: stay the same

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