Question

Could you please find my mistake in this problem? I'm not getting the right answer. :[

Use the reactions below to predict the equilibrium constant for the reaction 2A(g)<->3D(g)

A(s)<->1/2B(g)+C(g) k1=0.0334

3D(g)<->B(g)+2C(g) k2=2.35

I know that you have to make modifications according to the stoichiometric coeffecients. So do I divide k1 by 2 and the multiply that by the inverse of 2.35 (which = 1/2.35 because the equation is reversed)?

I got this answer
0.0034/2=0.0167*(1/2.35)
=0.0071

Answer 1

See my response to the original post.