Chemical equiilibrium questions | form six Chemistry

(a) (i) Define the term dynamic equilibrium
(ii) State the equilibrium law
(b) given the following system at equilibrium:
2SO₂(g) + O₂(g) 2SO₃(g) ΔH = -188.0kJmol^-1
Predict the change of the concentration of SO₃ if
(i) the pressure of the system is increased
(ii) a noble gas is added such that the pressure of the system increases but no volume changes occur
(iii) more SO₃ is added to the system
(iv) the temperature of the system is increased
(c) Consider the decomposition of phosphorous pentachloride: PCl₅(g) PCl₃(g) + Cl₂(g)
Derive an expression which relates K_c and K_p for the above equilibrium where K_c and K_p are the equilibrium constants in terms of concentration and pressure respectively.
(d) At 500^oC, the reaction between nitrogen and hydrogen to form ammonia has K_c = 8.0x10^-2 Calculate its K_p value.

Briefly explain the following phrases , giving one example for each

1. Reversible reaction
2. Heterogeneous equilibrium

1. State the equilibrium law and provide the corresponding expression.
2. List four characteristics of chemical equilibrium.
3. Write the expression for the equilibrium constant. , for the equation 

(i) Briefly explain the effect of change of pressure to a system at equilibrium.
(ii) Why does a Coca cola soda fizz out when its bottle is opened? Give a reason.

Consider the following equilibrium:
2CrO​ ₄​ ^2- ​ (aq) + 2H​ +​ (aq) ⇌ Cr​ _2​ O​ ₇​ ^2-​ (aq) + H​ _2​ O (l)
                        Yellow                                 Orange
What would be observed when:
(i) dilute NaOH is added to the equilibrium mixture?
(ii) dilute HCl is added to the equilibrium mixture?

The following equilibrium was established during the preparation of phosphorus(V)
pentachloride:
(i) Calculate the equilibrium constant for this reaction at 127^oC if the equilibrium
concentrations observed at this temperature were 0.034 mol/L for ammonia, 0.85 mol/L
for nitrogen and 0.031 mol/L for hydrogen.
(ii) Using the same equilibrium concentrations in (i), calculate the equilibrium constant at 127^oC for the equilibrium:
2NH​_3​ (g) ⇌ N​₂​ (g) + 3H​₂​ (g)

Briefly explain the following phrases , giving one example for each;

1. Reversible reaction
2. Heterogeneous equilibrium

1. State the equilibrium law and provide the corresponding expression.
2. List four characteristics of chemical equilibrium
3. Write the expression for the  equilibrium constant   for the equation .

The equilibrium equation for the oxidation of hydrogen chloride to chlorine is . In a certain experiment 0.80 moles of hydrogen chloride was mixed with 0.20 moles of oxygen in a closed vessel of capacity 10.00 dm³. At equilibrium , it was found that the mixture contained 0.20 moles of hydrogen chloride . Calculate the equilibrium constant for the reaction.Show your work clearly including manipulations of units.

1. State the law of mass action.
2. State the Le Chatelier`s principle.
3. Define dynamic equilibrium.
4. State three factors that change the position of the chemical equilibrium.