Reversible Reactions and Equilibrium

State that some chemical reactions are reversible as shown by the symbol ⇌
Describe how changing the conditions can change the direction of a reversible reaction for:
(a) the effect of heat on hydrated compounds
(b) the addition of water to anhydrous compounds
limited to copper(II) sulfate and cobalt(II) chloride
State that a reversible reaction in a closed system is at equilibrium when:
(a) the rate of the forward reaction is equal to the rate of the reverse reaction
(b) the concentrations of reactants and products are no longer changing
Predict and explain, for a reversible reaction, how the position of equilibrium is affected by:
(a) changing temperature
(b) changing pressure
(c) changing concentration
(d) using a catalyst
State the symbol equation for the production of ammonia in the Haber process,
N2(g) + 3H2(g) ⇌ 2NH3(g)
State the sources of the hydrogen (methane) and nitrogen (air) in the Haber process
State the typical conditions in the Haber process as 450 °C, 20,000 kPa / 200 atm and an iron catalyst
State the symbol equation for the conversion of sulfur dioxide to sulfur trioxide in the Contact process,
2SO2(g) + O2(g) ⇌ 2SO3(g)
State the sources of the sulfur dioxide (burning sulfur or roasting sulfide ores) and oxygen (air) in the Contact process
State the typical conditions for the conversion of sulfur dioxide to sulfur trioxide in the Contact process as 450 °C, 200 kPa / 2 atm and a vanadium(V) oxide catalyst
Explain, in terms of rate of reaction and position of equilibrium, why the typical conditions stated are used in the Haber process and in the Contact process, including safety considerations and economics