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An extremely soluble salt is added to water, and all of it dissolves. Is it at equilibrium? Explain 4b. A slightly soluble salt is added to water, and some of it dissolves. Is it at equilibrium? Explain 4c. Liquid water and water vapor reach equilibrium only in a closed container. Why?

An extremely soluble salt is added to water, and all of it dissolves. Is it at equilibrium? Explain 4b. A slightly soluble salt is added to water, and some of it dissolves. Is it at equilibrium? Explain 4c. Liquid water and water vapor reach equilibrium only in a closed container. Why?

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4a. An extremely soluble salt is added to water, and all of it dissolves. Is it at equilibrium? Explain

4b. A slightly soluble salt is added to water, and some of it dissolves. Is it at equilibrium? Explain

4c. Liquid water and water vapor reach equilibrium only in a closed container. Why?

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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