1. A 50.0-L reaction vessel contains 1.00 mol N2, 3.00 mol H₂, and 0.500 mol NH₃. Will more ammonia, NH₃, be formed or will it dissociate when the mixture goes to equilibrium at 400⁰C? The equation is   N₂(g) + 3H2(g)  ↔ 2NH₃(g).  Kc is 0.500 at 400⁰C.

2. The equilibrium constant Kc for the reaction  2NO(g) + O2(g)  ↔2NO2(g)  equals 4.0 x10¹³ at 25⁰C. Does the equilibrium mixture contain predominantly reactants or products?   If[NO] = [o₂ = 2.0 x 10^-6M]  at equilibrium, what is the equilibrium concentration of NO₂?

3. Carbon monoxide and hydrogen react in the presence of a catalyst to form methanol, CH3OH:                    

CO(g) + 2H2(g) ↔CH3OH(g)

An equilibrium mixture of these three substances is suddenly compressed so that the concentrations of all substances initially double. In what direction does the reaction go as a new equilibrium is attained?

4.  The reaction  CO(g) + H2O(g) ↔CO2(g) + H2(g)   is used to increase the ratio of hydrogen in synthesis gas (mixtures of CO and H2). Suppose you start with 1.00 mol each of carbon monoxide and water in a 50.0-L vessel. How many moles of each substance are in the equilibrium mixture at 1000⁰C? The equilibrium constant Kc at this temperature is 0.58.

5.   Do any of the following stable octahedral complexes have geometric isomers? If so, draw them.

a. [Co(NH3)5Cl]2^_                                        b. [Co(NH3)4(H2O)2]3^_

6.(a)   Explain the bonding in Cr(NH3)6]³⁺  complex in terms of VBT.

(b)      Using Crystal Field Theory explain which one of the following is a low-spin complex and the other one is high-spin complex.

            [Co(H₂O)6]Cl2    and    K₄[Co(CN)6]  .