Questions:

1) Write the equilibrium expression for the following reactions:

a) 2HI_(g) ⇌ H_2(g) + I_2(g)

b) H₂O_(g) + C_(s) ⇌ H_2(g) + CO_(g)

2) Nitrosyl Chloride decomposes according to the following equation:

2NOCl_(g) ⇌ 2NO_(g) + Cl_2(g)

At equilibrium the concentrations of these three gases were: [NOCl] = 0.00043, [NO] = 0.0072, [Cl₂] = 0.0016. Calculate K_eq for this equilibrium system:

3) 0.050 moles of SO_2(g) was reacted with 0.040 moles of oxygen to produce SO_3(g) in a 1L container. At equilibrium there was 0.024 moles of SO_2(g) remaining. Use an ICE table to calculate K_eq for this system:

4) Under certain conditions the equilibrium constant for the decomposition of dinitrogen tetraoxide to form nitrogen dioxide is 12.2. In a closed vessel, the concentration of N₂O_4(g) was 0.04M and the concentration of NO_2(g) was 0.03M. Determine if this system is at equilibrium and if not, which way the system will shift to reach equilibrium: