Answer to Question #313854 in General Chemistry for soidq

Question

Consider the reaction that has reached a state of equilibrium at 200^oC:

2HCl_(g) + O_2(g) ⇌ 2Cl_2(g) + 2H₂O_(g)      exothermic

 

Determine whether each of the following will increase the equilibrium concentration of Cl₂ product. Explain your reasoning.

a.   Remove H₂O gas

 

 

b.   Remove HCl gas

 

 

c.    Removing Cl₂ gas.

 

 

d.   Increasing the temperature of the system:

 

 

e.   Decreasing the pressure in the reaction vessel:

 

 

Answer 1

2HCl_(g) + O_2(g) ⇌ 2Cl_2(g) + 2H₂O_(g)      exothermic

a. Removing H₂O gas will increase the equilibrium concentration of Cl₂ product (removing one of the products shift equilibrium to the right to relieve the stress).

b. Removing HCl gas will decrease the equilibrium concentration of Cl₂ product (removing one of the reactants shift equilibrium to the left to relieve the stress).

c. Removing Cl₂ gas will increase the equilibrium concentration of Cl₂ product (removing one of the products shift equilibrium to the right to relieve the stress).

d. If reaction is exothermic heat is released. Thats why increasing the temperature of the system will shift equilibrium to the left (decrease the equilibrium concentration of Cl₂ product).

e. The equilibrium will move in such a way that the pressure increases again. It can do that by producing more gaseous molecules. In our case, the position of equilibrium will move towards the right-hand side of the reaction (increase the equilibrium concentration of Cl₂ product).