part a. For an exothermic reaction (one that gives off heat, H is negative), what effect will increasing the temperature of the reaction have on the

part a.

For an exothermic reaction (one that gives off heat, ΔH is negative), what effect will increasing the temperature of the reaction have on the equilibrium? What effect will decreasing the temperature have on the reaction?

a. Increasing the temperature will shift towards products, Decreasing the temperatue will shift towards the reactants

b. Increasing the temperature will shift towards the products, Decreasing temperature will also shift towards products

c. Increasing the temperature will shift towards reactants, Decreasing the temperatue will shift towards the products

d. Increasing or decreasing the temperature will not affect the reaction

part b.

The reaction COCl2(g) ⇌ CO(g) + Cl2(g) has an equilibrium constant, Kc = 2.19 x 10-10 at 100. ºC. Is the following mixture at equilibrium and if not, in which direction must it shift to reach equilibrium?

[COCl2] = 1.25 x 10-3 M, [CO] = 2.6 x 10-8 M, [Cl2] = 2.35 x 10-9 M

a. Must shift towards products.

b. Must shift towards reactants.

c. Not at equilibrium, direction of shift cannot be determined.

d. At equilibrium.

part c.

What is the pH of a 0.18 M solution of HC2H3O2? (Ka = 1.74 x 10-5)

a. 2.75

b. 7.45

c. 5.50

d. 1.76

part d.

What is the pH of a 0.025 M solution of KOH?

a. 15.60

b. 1.60

c. -1.60

d. 12.40

part e.

The reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g) has an equilibrium constant, Kp = 0.345 at 900 K. In an equilibrium mixture the pSO2 = 0.35 atm and pO2 = 0.55, what is the partial pressure of SO3 in the mixture? 

a. 0.195 atm

b. 0.646 atm

c. 0.00232 atm

d. 0.803 atm

part f.

What is the pH of a solution prepared from 1.33 M HC2H3O2 and 0.53 M KC2H3O2? Ka(HC2H3O2) = 1.8 x 10-5

a. 4.35

b. 4.74

c. 5.14

d. 9.65

part g.

For AgCl,