IGCSE Chemistry Revision Notes
Topic:Chemical reactions
Sub Topic: 6.3 Reversible reactions and equilibrium
Syllabus Objectives:
CORE:
- 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
EXTENDED:
- 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 using information provided
- 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, 20000kPa /200atm 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, 200kPa /2atm 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
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