At 500K, NOCl is 90% decomposed for the reaction 2NOCl<->2NO+Cl2. If we assume that 1.00mol of NOCl in 1.00L before dissociation, what is the value of Kc for equilibrium at 500K?

1 Answer
Dec 11, 2017

Kc36....

Explanation:

For 2NOCl(g)2NO(g)+Cl2(g)

We write Kc=[NO]2[Cl2][NOCl(g)]2

Now initially there were 1.00molL1 with respect to NOCl; at equilibrium [NOCl]=0.10molL1, [NO]=0.90molL1, and [Cl2]=0.45molL1...

And so we fill in the numbers....

Kc=(0.90molL1)2×0.45molL1(0.10)2=36.5