SHOW ALL WORK

1) The air pollutant NO is produced in automobile engines fromthe high-temperature reaction, N2 (g) + O2 (g) ⇌ 2 NO (g); Kc = 1.7× 10-3 at 2300K . If the initial concentrations of N2 and O2 at2300 K are both 1.4 M, what are the concentrations of NO, N2, andO2 when the reaction mixture reaches equilibrium? Show your work(20 points).

2) For each of the following equilibria, use LeChatelier’sprinciple to predict the direction of reaction when the volume isincreased. (15 points)

(a) CO(g) + H2(g) ⇌ C(s) + H2O(g)

(b) 2H2(g) + O2 (g) ⇌ 2 H2O(g)

(c) Fe2O3(s) + 3 H2(g) ⇌ 2Fe(s) + 3 H2O(g)

3) Will the concentration of NO2 increase, decrease, or remainthe same when the equilibrium of the exothermic reaction, NOCl(g) +NO2(g) ⇌ NO2Cl (g) + NO(g) is disturbed by the following changes?(15 points)

(a) adding NOCl

(b) adding NO

(c) Removing NO

(d) Adding argon

(e) addition of a catalyst

4) Calculate [H+] of a solution prepared by dissolving 4.25grams of lithium hydroxide (24 g/mole) in water (18 g/mole) to give350.0 mL of solution. (12 points) Kw= 1.0 × 10-14

5) Lactic acid (C3H6O3), whichoccurs in sour milk and foods such as sauerkraut, is a weakmonoprotic acid. The [H+] of a 0.10 M solution of lactic acid is4.57 × 10-3. What is the value of Ka for lactic acid? (16points)

6) Write a chemical reaction foreach of the following ions reacting with water. Demonstrate withthis reaction whether they give neutral, acidic, or a basicsolution. (16 points)

(a) F-

(c) NH4+

(d) K(H2O)6+

(e) SO32-

7) Calculate the percentdissociation of 0.10 M hydrazoic acid (HN3; Ka = 1.9 ×10-5) in thepresence of 0.10 M HCl, and explain if this dissociation is more,the same, or less than if the HCl was not present. (16points)