The reaction H,0(0) + CO,(aq) H,CO,(aq) is at equilibrium. What does this mean?.

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9b. Explain equilibrium based on collision theory

 

9. The reaction H,O(1) + CO,(aq) = H,CO,(aq) is at equilibrium. What does this mean?
Transcribed Image Text:9. The reaction H,O(1) + CO,(aq) = H,CO,(aq) is at equilibrium. What does this mean?
The Ins and Outs
of Équilibrium
If you leave a closed, partly filled bottle of water in the sunlight, before
long you will observe water droplets near the top of the bottle and in the
neck. How did they get there? As the sun shines on the bottle, the water
begins to evaporate. As the number of vapor molecules increases, so does
the chance that they will interact with each other and recondense to form
water. This is how the water droplets get to the top of the bottle.
Changing phase is a reversible process. In a closed container, as the
amount of vapor increases and the amount of liquid decreases, the rate of
condensation increases and the rate of vaporization decreases. Eventually
the two rates become equal. When the rate of vaporization is equal to the
rate of condensation, the amount of vapor and the amount of liquid stops
changing. This is called equilibrium. Just because the rate of vaporization
and condensation is equal at equilibrium, it doesn't mean that the amount
of vapor and the amount of liquid is equal. For example, the amount of gas
at equilibrium will be greater at a high temperature than at a low
We're
back!
I'm sure
glad they
Jevaporated!
Then l'm
getting out
of here!
The social dynamics of phase equilibrium
temperature.
There are other kinds of equilibrium besides phase equilibrium. Some chemical reactions are reversible and reach
equilibrium too. When undissolved solid sits at the bottom of a saturated solution, there is solution equilibrium. It may look
like the same undissolved solid at the bottom of the container the entire time, but dissolved material comes out of solution and
new material dissolves continuously. Only the amount ofundissolved material remains the same. This is often called dynamic
equilibrium because there is constant activity although there is no real change.
Transcribed Image Text:The Ins and Outs of Équilibrium If you leave a closed, partly filled bottle of water in the sunlight, before long you will observe water droplets near the top of the bottle and in the neck. How did they get there? As the sun shines on the bottle, the water begins to evaporate. As the number of vapor molecules increases, so does the chance that they will interact with each other and recondense to form water. This is how the water droplets get to the top of the bottle. Changing phase is a reversible process. In a closed container, as the amount of vapor increases and the amount of liquid decreases, the rate of condensation increases and the rate of vaporization decreases. Eventually the two rates become equal. When the rate of vaporization is equal to the rate of condensation, the amount of vapor and the amount of liquid stops changing. This is called equilibrium. Just because the rate of vaporization and condensation is equal at equilibrium, it doesn't mean that the amount of vapor and the amount of liquid is equal. For example, the amount of gas at equilibrium will be greater at a high temperature than at a low We're back! I'm sure glad they Jevaporated! Then l'm getting out of here! The social dynamics of phase equilibrium temperature. There are other kinds of equilibrium besides phase equilibrium. Some chemical reactions are reversible and reach equilibrium too. When undissolved solid sits at the bottom of a saturated solution, there is solution equilibrium. It may look like the same undissolved solid at the bottom of the container the entire time, but dissolved material comes out of solution and new material dissolves continuously. Only the amount ofundissolved material remains the same. This is often called dynamic equilibrium because there is constant activity although there is no real change.
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