Equilibrium In 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$^{-5}$

A 2.16 L reaction vessel contains 0.186 mol HCONH$_2$, and 0 mol of NH$_3$ and CO. How many moles of each substance are in the equilibrium mixture at 400 K? What is the pressure in the vessel?

HCONH$_2$ $\leftrightharpoons$ NH$_3$ + CO , K$_C$ = 4.84

At 1000 K, 0.250 mol SO$_2$ and 0.200 mol O$_2$ react in a 10.0 L reaction vessel to form 0.162 mol of SO$_3$ at equilibrium. What is K$_{eq}$ at 1000 K for the reaction?

2 SO$_2$ (g) + O$_2$ (g) $\leftrightharpoons$ 2 SO$_3$ (g)