2.5 mol NOCl(g) was placed in a 2.50 L reaction vessel at 400 degrees C. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation:
2NOCl(g)<-->2NO(g)+Cl2(g)
Calculate the equilibrium constant, Kc, for the reaction.
2NOCl(g)<-->2NO(g)+Cl2(g)
Kc=[(NO)^2(Cl2)]/(NOCl)^2
Starting with 2.5 mol NOCl, if 28% is dissociated, then (Cl2) must be 2.5 mol x 0.28. (NO) must be twice that, and (NOCl) must be 2.5 mol - (Cl). Plug and chug. Check my thinking.
Bob, the choices are:
a. 0.021
b. 0.039
c. 0.169
d. 26
e. 47
I keep getting 0.169
Help me with my thinking. Once I plug and chug, I should be dividing each by 2.50 L's and squaring the results of NO and NOCl before completing it, right?
1 answer
Yes, that is correct. The equation for Kc is Kc=[(NO)^2(Cl2)]/(NOCl)^2. So, you need to divide each of the concentrations by 2.50 L and then square the concentrations of NO and NOCl before completing the equation.
0 answers