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When an inflated balloon is placed in a temperature above room temperature, the gas molecules will gain more energy an increase the circumference of the balloon, in a cold temperature, the balloons gas molecules will loose this energy and movement causing the balloons circumference to decrease in size.

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3+ latex balloons

1 freezer thermometer

1 candy thermometer
Large pot

Flexible measuring tape

One room temperature area

One above room temperature area

One cool area, far below room temp

Clock-timer

Place for note taking

Graph creator

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Step 1: Blow up the first balloon, until it is quite full. *Keep in mind my measurement of the freezer, where the balloon will go. Measure the circumference of the balloon by measuring the balloon at the widest part. Mark this balloon with the number 1. Use the circumference data table shown in Balloon Morphing: How Gases Contract and Expand | Science Project under balloon number one.  Inflate another balloon, without ting the balloon, get someone else to help measure the balloon in its widest part, and stop inflating once the measurement is within .5 cm of the first measurement. Mark this measurement under balloon under 2 in the circumference data table. Repeat this step with the third balloon.

Step 2: Measure the temperature of my room temperature room, with my thermostat. Write this temperature in the first box under temperature. Leave the balloons at least 2 feet above the ground at room temperature. Measure the balloon's circumference at the widest part, not so tight that the balloon is being squeezed. Write down measurements under each balloon in the table.

Step 3: Clear out a space large enough for a balloon to sit for one hour. Place one balloon in the freezer as well as the thermometer for one hour. Immediately remove the balloon and measure the circumference right away. Do this step for all other balloons. After all balloons have been in the freezer for one hour each, immediately measure the last circumference. Write down the temperature as shown on the thermometer.

Step 4: Allow the last balloon to come to room temperature for 20 minutes. Over medium- low heat, place the balloon within a pot. Leave for about 5-10 minutes or until I see changes. Immediately remove balloons from the hot temperature, and record circumference in the table. Measure temperature according to the candy-thermometer.

Step 5: Find the average of the data. First, add up all of the circumferences for each temperature, then divide by 3 and this will be the average. Cube the average for each temperature, by multiplying each average by itself 3 times.

Step 6: Then, to create the graph, plot each temperature in celcius on the x axis on some graph paper. Then plot each average circumference cubed on the y axis. Then, draw a line by hand. ?

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-Balloon #1 after one hour in the freezer

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Balloon #2 after one hour in the freezer

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Balloon #3 after 1 hour in the freezer

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The Freezer Thermometer reading about -10 degrees F

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Balloon #1 over medium heat in water.

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Balloon #2 over medium heat in water.

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Balloon #3 over medium heat in water.

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Candy/food thermometer reads about 140 degrees F.

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Is there a linear relationship between the circumference of my balloon cubed and the changes in temperature?

There is not a linear relationship between the circumference and the changes in temperature. Because the number of degrees isn't constant as the environment changes, and the circumference increases and decreases at different rates, the relationship isn't linear.

What was the change when going from room temperature to hot temperature, and what was the change when going from room temperature to cool temperature?

When going from room temperature to hot temperature, I took down about a 3 cm change on average in circumference. I noticed that as the balloon was in the pot of hot water, it would rotate, and as soon as I took it out, the balloon was warm and misty on the outside. And then, when going from room temperature to my cool temperature, I noticed that the circumference changed by about 1.5 cm on average. I noticed that the balloon was less firm than at room temperature when it was immediately taken out of the freezer.

How do I think the gas molecules inside of the balloon act as the temperature increases?

When the temperature outside of a balloon increases, according to Amontons law, when the temperature outside increases, gas molecules will increase in speed and energy, and as the balloon holds the molecules in its walls, the pressure increases due to the more forceful collisions from the energized molecules. A balloon is able to change in size and shape depending on how the gas molecules inside of it react, so according to Charles Law, the pressure a gas gains from the temperature outside, the pressure inside can only be maintained if the space increases in size. I think that the gas molecules increase in pressure by creating more forceful collisions that make the balloon expand in space.

What happens to the space between the gas molecules as the temperature decreases?

As the temperature decreases on the outside of the balloon, the gas molecules will have less energy, and less space between them. The motion of the gas molecules is what keeps the balloon inflated, if these molecules have less space between them, because they are cooled and not heated, they give the opposite effect of heating when the molecules will have more space between them, the balloon will shrink in size. The pressure outside of the balloon is equal to the pressure inside, and this means when cooled, the pressure decreases.

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When an inflated balloon is placed in a temperature above room temperature, the gas molecules will gain more energy and increase the circumference of the balloon, in a cold temperature, the balloon's gas molecules will lose this energy and movement causing the balloon's circumference to decrease in size.

My experiment aims to observe the ways that gas molecules will behave and change their environment when contained inside of a balloon, at different temperatures for equal amounts of time. My experiment showed me that the gas molecules affect the circumference of the balloon as the molecules loose, and gain energy in their different environments. A balloon was what makes sense for this experiment, as it is a place to contain the molecules which can change as the pressure builds and decreases. Now looking at my circumference data table, my evidence supports my hypothesis. At room temperature, the circumference of the balloon remains as a starting point. But as each balloon was placed in the freezer, they all had at the highest a 1 inch decrease in size. This supports my idea that the gas molecules will decrease in pressure as they are placed in a below room temp. area, because the pressure outside of a balloon is equivalent to the pressure that the molecules create inside of the balloon. (13.2: Gas Pressure) When the balloon was placed in room temperature again, the increase in temperature allowed the balloons to come back to a larger circumference. When the balloon is placed in a heated area, the circumference increases. The heat from the water, and the steam rising around the balloon allows the molecules to gain more energy, space between them, all increasing how much room the gas molecules need to take up. When I took the balloon out of the heat, I saw that the circumference increased at the most by about 1 inch. This overall supports the claim that a balloon's environment and its temperature will make it increase or decrease in size.
The reason that balloons will decrease in size when placed in a cool temperature, or increase in size when placed in a hot environment is according to the laws of Kinetic Molecular Theory. This theory claims that gas molecules are able to be compressed, because of the room between them. In comparison to solid, or liquid molecules, which are tightly packed and not able to be compressed, gas molecules have a space 10x the size of one molecule between two of them. Under a hot temperature, this space can increase, and decrease in a cool environment or when contained. (Compressibility | CK-12 Foundation) The reason that gas molecules are able to make the balloon increase, is defined according to Amontons law, which says if the temperature increases, gas molecules will increase in speed. The Kinetic-Molecular Theory | Chemistry. Gas molecules are always in motion, and moving in an orderly straight line. When contained inside of a balloon, the molecules will hit the balloon's walls, and when they collide they don't lose energy but create them. According to Charles law: the pressure a gas gains from the temperature it is surrounded by, the pressure will only be maintained if the space increases, as the room between molecules will grow. The Kinetic-Molecular Theory | Chemistry.  This is why we see a change in circumference when a balloon is heated, but not when it is cooled. When a balloon is cooled, the molecules have less space between them, and become more compressed.
With my understanding of the Kinetic Molecular Theory, my conclusions that the balloon increases and decreases in size, shows that the gas molecules are behaving according to the KMT laws, so my conclusion fits in with my understanding of the concepts of compressibility, KMT, and how pressure within a contained surface works. My experiment however, could have some errors that could lead to my conclusions being incorrect. Firstly, with a home conducted experiment, there are more factors I did not consider, such as the effects of an unsanitized surface on the balloons and how that will make them behave. With any science experiment, there are also possibilities that the technology I am using to tell time, the temperature, or record data is faulty and gives me an incorrect reading of my constants. Another human error would be removing the balloons from their environments, and then not measuring the circumference quickly enough. Another would be, incorrectly placing the measuring tape on the balloon, and getting the wrong measurement that is too big or too small. Outside of human error though, my experiment is limited mostly because of the lack of technology accessible to see what gas molecules actually behave like on the microscopic level. Because of this, I cannot 100% assure that the molecules are behaving according to the KMT laws I describe. My experiment is also limiting because using the example of a balloon is not inclusive of the ways that gas molecules behave in other environments, or how it might be different if I were to have used a hot air balloon or water balloon. My experiment also limits how the molecules might behave in all extremes of temperatures. Because I cannot test every 1 degree difference, I will not see all of the ways that gas molecules behave at different levels. Overall, science experiments like this have many limits, if you do them outside of a lab. My hypothesis could have been reached because I used sources that only support my idea, and none that counter the KMT theory. My incorrect measurements, or conversions of units could have led to my hypothesis.