C8.8 - Dynamic equilibrium Flashcards
Closed system
A closed system is a system in which no matter:
1. Enters
Or,
2. Leaves
In a reversible reaction, what happens as the concentration of products builds up?
In a reversible reaction, as the concentration of products builds up, the rate at which they react to re-form reactants increases
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
What happens, as this starts to happen?
As this starts to happen, the rate of the forward reaction is decreasing
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, why is the rate of the forward reaction decreasing?
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value.
What eventually happens?
Eventually, both:
1. Forward
2. Reverse
reactions are happening at the same rate
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value.
Eventually, both forward and reverse reactions are happening at the same rate, but in opposite directions.
What is happening when this happens?
When this happens, the reactants are making products at the same rate as the products are making reactants
Equilibrium
Equilibrium is the point in a reversible reaction at which the:
1. Forward
2. Backward
rates of reaction are the same
At equilibrium, the rate of the forward reaction equals what?
At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction
When a reaction has reached equilibrium, what happens as the forward and reverse reactions are continuously taking place?
When a reaction has reached equilibrium, as the:
1. Forward
2. Reverse
reactions are continuously taking place, a state of ‘dynamic’ equilibrium has been reached
When a reaction has reached equilibrium, why are the forward and reverse reactions that are continuously taking place unnoticed?
When a reaction has reached equilibrium, the forward and reverse reactions that are continuously taking place are unnoticed, because they occur at the atomic level
Example of a reversible reaction
An example of a reversible reaction is the reaction between:
- Iodine monochloride, ICl
- Chlorine gas
The chemical formula of iodine monochloride
The chemical formula of iodine monochloride is ICl
Iodine monochloride in relation to chlorine
Iodine monochloride is a brown liquid, while chlorine is a yellowish green gas
Iodine monochloride is a brown liquid, while chlorine is a yellowish green gas.
These substances can be reacted together to make what?
These substances:
1. Iodine monochloride
2. Chlorine
,can be reacted together to make yellow crystals of iodine trichloride
Chemical formula of iodine trichloride
The chemical formula of iodine trichloride is ICl3
Iodine monochloride and chlorine can be reacted together to make yellow crystals of iodine trichloride.
What happens when there is plenty of chlorine gas?
When there is plenty of chlorine gas, the forward reaction makes iodine trichloride crystals
Iodine monochloride and chlorine can be reacted together to make yellow crystals of iodine trichloride.
When there is plenty of chlorine gas, the forward reaction makes iodine trichloride crystals.
However, what happens if the concentration of chlorine gas is lowered?
If the concentration of chlorine gas is lowered, the rate of the:
- Forward reaction decreases
- Reverse reaction increases
Iodine monochloride and chlorine can be reacted together to make yellow crystals of iodine trichloride.
If the concentration of chlorine gas is lowered, the rate of the forward reaction decreases and the rate of the reverse reaction increases.
What does this do?
This starts turning more iodine trichloride back to:
- Iodine monochloride
- Chlorine
How can you change the relative amounts of the reactants and products in a reacting mixture at equilibrium?
You can change the relative amounts of the:
1. Reactants
2. Products
in a reacting mixture at equilibrium by changing the conditions
You can change the relative amounts of the reactants and products in a reacting mixture at equilibrium by changing the conditions.
What is this an application of?
This is an application of Le Chatelier’s Principle
Le Chatelier’s Principle
Le Chatelier’s Principle is that when a change in conditions is introduced to a system at equilibrium, the position of equilibrium shifts, so as to cancel out the change
Henry Louis Le Chatelier
Henry Louis Le Chatelier was a French chemist who observed equilibrium mixtures
Henry Louis Le Chatelier was a French chemist who observed equilibrium mixtures.
What did he notice?
Henry Louis Le Chatelier noticed that whenever a change in conditions is introduced to a system at equilibrium, the position of equilibrium shifts, so as to cancel out the change
Henry Louis Le Chatelier noticed that whenever a change in conditions is introduced to a system at equilibrium, the position of equilibrium shifts so as to cancel out the change.
What can the change in conditions be?
The change in conditions can be changes in: 1. Concentration 2. Pressure Or, 3. Temperature
Le Chatelier’s Principle is very important in what?
Le Chatelier’s Principle is very important in the chemical industry
Why is Le Chatelier’s Principle very important in the chemical industry?
Le Chatelier’s Principle is very important in the chemical industry, because in a process with a reversible reaction, industrial chemists need to find the conditions that give as much product as possible, in as short a time as possible
Le Chatelier’s Principle is very important in the chemical industry, because in a process with a reversible reaction, industrial chemists need to find the conditions that give as much product as possible, in as short a time as possible.
However, what are there always to consider when chemists manipulate reversible reactions in industry?
There are always other:
1. Economic
2. Safety factors
to consider when chemists manipulate reversible reactions in industry
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value.
Eventually, both forward and reverse reactions are happening at the same rate, but in what?
Eventually, both:
1. Forward
2. Reverse
reactions are happening at the same rate, but in opposite directions
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value.
Eventually, both forward and reverse reactions are happening at the same rate, but in opposite directions.
When this happens, the reactants are making products at the same rate as the products are making reactants.
Overall, there is what?
Overall, there is no change in the amount of:
- Products
- Reactants
As the concentration of products builds up, the rate at which they react to re-form reactants increases.
As this starts to happen, the rate of the forward reaction is decreasing, because the concentration of reactants is decreasing from its original maximum value.
Eventually, both forward and reverse reactions are happening at the same rate, but in opposite directions.
When this happens, the reactants are making products at the same rate as the products are making reactants.
Overall, there is no change in the amount of products and reactants.
The reaction has reached what?
The reaction has reached equilibrium
Equilibrium is the point in a reversible reaction at which the forward and backward rates of reaction are the same.
Therefore, the amounts of substances present in the reacting mixture do what?
Therefore, the amounts of substances present in the reacting mixture remain constant
Iodine monochloride and chlorine can be reacted together to make yellow crystals of iodine trichloride.
If the concentration of chlorine gas is lowered, the rate of the forward reaction decreases and the rate of the reverse reaction increases.
This starts turning more iodine trichloride back to iodine monochloride and chlorine, until what?
This starts turning more iodine trichloride back to:
1. Iodine monochloride
2. Chlorine
,until equilibrium is established again
