Ice Table Chemistry

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$^{-5}$

0.800 moles of N$_2$ (g) are placed in a 7.00 L flask with 3.00 moles of H$_2$ and allowed to react for some time. After several hours the concentrations of H$_2$ (g) is measured at 0.278 M. What is the equilibrium constant for the reaction at this temperature?

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

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