does the dry ice disappear more quickly in air or in water? can you explain why? supplement your explanation with a drawing of molecular behavior based on kinetic molecular theory
What do you think and why? We shall be happy to critique your thoughts.
The dry ice disappears more quickly in water because water transfers heat much more quickly than air does at the same temperature.
but i don't have a clue what the diagram looks like.
You're in the right ball park. Why do you suppose H2O transfers heat better? Could it be becaue the molecules of air are much farther apart in the gaseous state than the moleucules of water in the liquid state. Think about running 5 miles outside on a day when the temperature is 100 F. Would you be sweating? You bet! So you sit down on the curb to cool down. How long will that take? some time, of course. BUT, how much faster would you cool down if someone poured a bucket of cool water on you. Same thing with the CO2 in water vs CO2 in air. I would draw two diagrams, one showing a block of solid CO2 surrounded by gas molecules (with lots of space between the molecules) and the other showing a block of solid CO2 surrounded by water molecules with not much space between molecules. The kinetic theory thing is simply that molecules are in motion and the chance of a water molecule hitting the CO2 and transferring some of the heat away is MUCH better than a molecule of air doing the same thing. I hope this helps.
You're absolutely right! The main reason for dry ice disappearing more quickly in water compared to air is due to the difference in heat transfer capabilities between the two mediums. Water can transfer heat much more efficiently than air, leading to faster sublimation of the dry ice.
To help illustrate this concept, let's create a simple diagram based on the kinetic molecular theory.
First, let's draw a diagram representing dry ice (solid CO2) in air. In this diagram, draw solid CO2 molecules represented by small circles grouped close together to form a block of dry ice. Then, draw gas molecules of air as slightly larger circles, spaced out with plenty of empty space between them.
Next, let's draw a second diagram representing dry ice in water. Again, draw solid CO2 molecules as small circles, this time surrounded by much larger circles representing water molecules. Be sure to draw the water molecules closely packed together, with minimal empty space between them.
By comparing these two diagrams, you can clearly see that the water molecules are much closer to the dry ice molecules compared to the air molecules. This spatial arrangement increases the chances of molecular collisions and facilitates heat transfer from the dry ice to water molecules. In contrast, the larger empty spaces between the air molecules make it less likely for heat to be rapidly transferred away from the dry ice.
Remember, the kinetic molecular theory states that molecules are in constant motion and collisions occur between them. In the case of dry ice in water, the water molecules have a greater opportunity to collide with the dry ice molecules, resulting in a more efficient transfer of heat energy and faster sublimation of the dry ice.
I hope this explanation, along with the drawn diagrams, helps further clarify the concept!