Practise MYP Chemistry questions on 5.20 Reversible Reactions and review the explanations to check your understanding.
Use these questions for topic practice and to find ideas you want to revisit in your notes or lessons.
According to the "arrow and rate" dynamic model, if the arrow representing the forward reaction is significantly longer than the arrow for the reverse reaction, what can be concluded about the state of the system?
Which of the following gas-phase equilibrium systems will experience NO change in the position of equilibrium when the total pressure of the system is increased?
How does the rate of the reverse reaction change during the initial stages of a reversible reaction when only reactants are present?
In a reversible reaction starting with only reactants, as the system approaches equilibrium, the rate of the forward reaction __________ while the rate of the reverse reaction increases.
The Haber process uses a 'compromise' temperature. If the forward reaction is exothermic, according to Le Chatelier's Principle, using a __________ temperature would actually result in a higher percentage yield of ammonia, even though it would be too slow for industrial use.
The system has reached dynamic equilibrium
The system has reached completion and all reactants are gone
The system is currently producing more product than it is consuming
The reverse reaction has completely stopped
It increases from zero as products are formed
It decreases as reactants are used up
It is initially higher than the forward rate
It remains constant until equilibrium is reached
