Question

15.   Consider the following reaction: 2 2 eqH O (g)   + Cl O (g)      2 HClO (g)        ÄH = 3.00 kcal    K = 0.0900 at 25°C
a. Does the equilibrium favor products or reactants at 25°C? The equilibrium favors reactants (K < 1)

b. Would the equilibrium shift in the favor of reactants (left) or products (right) if:
a. The temperature was lowered?
b. H2O was added to the reaction mixture?
c. The volume was increased?

d. HClO was removed from the reaction mixture?

Answer 1

Ans 15 :

a) The value of K is less than 1 , so the equillibrium favors reactants.

b) : a) The reaction is endothermic reaction. So if the temperature is lowered , the equillibrium shift in the favor of reactants.

b) H2O is a reactant here , so if H2O is added to the reaction mixture , the equilibrium shifts in the favor of products.

c) If volume is increased , the pressure reduces so equilibrium shifts in the favor of reactants .

d) HClO is a product here , so if it is removed from the reaction mixture , the equilibrium shifts in the favor of products.