1. For the reaction:

C(s) + CO₂ (g) = 2 CO(g) DH = +119.8 kJ

what will be the effect of each of the following on the reaction and on the value of the equilibrium constant?

Reacts to the: (right, left, no effect) The value of K: (increase, decrease, no effect)

a) add CO

b)increase temperature

c) add a catalyst

d) remove CO₂

e) add CaO(s) which reacts with CO₂

2. Write the equilibrium expression, Kc, for the following reactions:

a) PCl₅(g) = PCl₃(g) + Cl₂(g)

b) ZnSO₃(s) = ZnO(s) + SO₂(g)

c) H₂O(l) = H ⁺ (aq) + OH ^- (aq)

d) H₂(g) + FeO(s) = H₂O(g) + Fe(s)

e) 4 NH₃(g) + 3 O₂(g) = 2 N₂(g) + 6 H₂O(g)

3. A sample of chlorine gas dissociates at 1300 K by the reaction: Cl₂(g) = 2 Cl(g)When equilibrium is reached at this temperature, it is found that the partial pressure of diatomic chlorine is 0.87 atm and the partial pressure of atomic chlorine is .0000054 atm. What is the value of Kp at 1300 K?

4. A mixture of 2 mole of SO₂ and 4 mole of O₂ are placed in a 4 liter flask and kept at l000 K until equilibrium is reached. At equilibrium the vessel is found to contain 1.60 mol of SO₃. a) What is the equilibrium concentration of SO₃?b) At equilibrium, how many moles of SO₂ and O₂ are left?c)Calculate the concentration equilibrium constant for the reaction: 2SO₂(g) + O₂(g) = 2SO₃(g)

5. In the reaction:

N₂(g) + O₂(g) = 2 N0(g)

the initial concentrations were [O₂] = 0.050 M and [N₂] = 0.10 M and no N0. After the reaction had reached equilibrium the concentration of [O₂] was 0.025 M. a) What are the equilibrium concentrations of N₂, O₂, and NO? b) What is the value of Kc?

6. At some temperature the equilibrium constant, K_c, for the reaction:

Br₂(g) = 2 Br (g)

is 4.0x10^-16

When the inital [Br₂] in a flask is 4 M, what will be concentrations of Br₂ and Br at equilibrium?

(answer [Br] = 4x10^-8M explain)