General Chemistry 2: Chemical Equilibrium

A 1.9 L vessel contains a gaseous mixture with 0.455 mol SO$_2$, 0.183 mol O$_2$, and 0.568 mol SO$_3$. Is the reaction at equilibrium? If not, what is the direction of the reaction?

2 SO$_2$ + O$_2$ $\leftrightharpoons$ 2 SO$_3$, K$_C$ = 280

A 1 L reaction vessel contains 2.5 mol A, 3 mol B, and initially 0 C. Find the concentrations of all species at equilibrium.

A + 2B $\leftrightharpoons$ 3 C , K$_C$ = 0.25

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$^{-5}$

Starting with 0.50 M N$_2$O$_4$, calculate the equilbrium concentrations of all species involved in the reaction below.

N$_2$O$_4$ $\leftrightharpoons$ 2 NO$_2$ K$_C$ = 1.2

A 2.5 L reaction vessel contains 0.55 mol PCl$_5$, 0.55 mol PCl$_3$, and 0 mol Cl$_2$. Find the molarity of Cl$_2$ at equilibrium.

PCl$_5$ $\leftrightharpoons$ PCl$_3$ + Cl$_2$ , K$_C$ = 3.8 x 10$^{-2}$

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