If at equilibrium [H2] = 0.100 mol/L , [HI] = 0.120 mol/L and [I2] = 0.210 mol/L at 250oC, calculate the equilibrium constant at that temperature (don’t forget the units).
2HI (g) ⇄ H2 (g) + I2 (g)

At equilibrium at 100oC, a 2.0-L flask contains:
0.750 mol of PCl5 0.500 mol of H2O 0.075 mol 0f HCl 0.050 mol of POCl3
Calculate the Keq for the reaction (don’t forget the units):

Consider the following equation 2SO3(g) ⇄ 2SO2(g) + O2(g)
At equilibrium [SO3] = 0.600 mol/L [SO2] = 0.540 mol/L & [O2] = 0.270 mol/L
Calculate the value of the equilibrium constant, Kc (don’t forget the units).

Consider the following equilibrium: N2O4(g) ⇄ 2 NO2(g)
1.00 moles of NO2 and 3.20 moles of N2O4 are present in a 4.00 L flask at equilibrium at 20oC.
Calculate the Keq at 20oC (don’t forget the units).

0.800 moles CO, 0.800 moles H2O, 4.00 moles CO2, & 6.50 moles H2 are found in a 2.00L container . at 690oC at equilibrium. Calculate the value of the equilibrium constant (don’t forget the units).
CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g)

2NO2 (g) ⇄ 2NO(g) + O2 (g)
At equilibrium there are 4.50 mol of NO2 , 3.00 mol of NO and 2.00 mol of O2 in the 1.00 L container.
Calculate the value of the equilibrium constant (don’t forget the units).

Kc= 0.798 mol. L-1 at 25oC for the reaction: 2SO3 (g) ⇄ 2SO2 (g) + O2 (g)
In a mixture at equilibrium, [SO2] = 4.20 mol/L and [SO3] = 11.0 mol/L. Calculate the equilibrium [O2] in this mixture at 25oC (don’t forget the units).

Consider the following equilibrium: 2SO3 (g) ⇄ 2SO2 (g) + O2 (g)
0.500 moles of SO2 and 0.500 moles of SO3 are present in a 1.00 L flask at equilibrium at 100oC. If the Keq = 0.680 mol. L-1, calculate the O2 concentration at 100oC (don’t forget the units).
2HCl (g) + POCl3 (g) ⇄ PCl5 (g) + H2O (g)