Proteins are broken down in the body during digestion.
What type of substance acts as a catalyst in this process?
In industry, ammonia is produced by reacting nitrogen with hydrogen.
The equation for the reaction is:
N2(g)+3H2(g)⇌2NH3(g) \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) N2(g)+3H2(g)⇌2NH3(g)How many moles of nitrogen react completely with 9.0×1049.0 \times 10^49.0×104 moles of hydrogen?
The reaction is carried out at a temperature of 450 ∘C450\ ^\circ\text{C}450 ∘C and a pressure of 200200200 atmospheres.
The forward reaction is exothermic.
Explain what happens to the yield of ammonia if a temperature higher than 450 ∘C450\ ^\circ\text{C}450 ∘C is used.
A pressure of 200200200 atmospheres is used instead of atmospheric pressure.
The higher pressure gives a greater yield of ammonia and an increased rate of reaction.
Explain why.
An iron catalyst is used in the reaction to produce ammonia from nitrogen and hydrogen.
Explain how a catalyst increases the rate of a reaction.
Suggest why a catalyst is used in this industrial process.
Do not give answers in terms of increasing the rate of reaction.
Suggest the effect of using the catalyst on the equilibrium yield of ammonia.
21 exam-style questions on AQA GCSE Chemistry 6.2 Reversible reactions and dynamic equilibrium, covering 6.2.1 Reversible reactions, 6.2.2 Energy changes and reversible reactions, 6.2.3 Equilibrium, 6.2.4 The effect of changing conditions on equilibrium (HT only), 6.2.5 The effect of changing concentration (HT only), 6.2.6 The effect of temperature changes on equilibrium (HT only), and 6.2.7 The effect of pressure changes on equilibrium (HT only). Each one has a worked solution and a mark scheme showing where the marks go.