I2 + Cl2 →2ICl Kp=81.9. A reaction mixture initially P(I2)=P(Cl2)=P(ICl)= 0.1 atm. How to determine the direction of the reaction will proceed?

1 Answer
Dec 9, 2015

Answer:

The equilibrium will shift to the right.

Explanation:

The equilibrium in question is the following:

#I_2+Cl_2rightleftharpoons2ICl" " " "K_P=81.9#

The expression of #K_P# is: #K_P=(P_(ICl)^2)/(P_(I_2)*P_(Cl_2)#

Since we have the initial pressures, we will determine the direction of the equilibrium from the reaction quotient #Q_P#.

The expression of #Q_P# is: #Q_P=((P_0)_(ICl)^2)/((P_0)_(I_2)*(P_0)_(Cl_2))#

#=>Q_P=(0.1)^2/((0.1)xx(0.1))=1 < K_P#

Since #Q_P < K_P# then the equilibrium will shift to the right to increase the pressure of the product (numerator) and decrease the pressure of reactants (denominator).