Equilibrium Ice Tables

Find the equilibirium concentrations when starting with 0.50 M H$_2$ and 0.50 M Br$_2$

H$_2$ + Br$_2$ $\leftrightharpoons$ 2 HBr , K$_C$ = 143

0.20 M I$_2$ is placed in a reaction vessel. Find the concentrations of I$_2$ and I at equilibrium.

I$_2$ (g) $\leftrightharpoons$ 2 I (g) , K$_C$ = 3.8 x 10$^{-5}$

Predict the effect an increase in H$_2$ would have on the following reaction. What if we increase the temperature? If we remove H$_2$O?

CO (g) + H$_2$O (g) $\leftrightharpoons$ CO$_2$ (g) + H$_2$ (g) + heat, K$_C$ = 5.10

3 A(s) + 5 B(g) $\leftrightharpoons$ 5 C(g) + 6 D(s) $\triangle$H = 0 kJ

A. Predict the change in A when D is added

B. Predict the direction of reaction when the pressure is increased

C. Predict the direction of reaction when the heat is increased