Introduction - the volume of any gas is directly proportional to the temperature of that gas when pressure and moles are held constant. This is know as Charles' Law.In this experiment you will attempt to prove this law.
Procedure-
1. Obtain a balloon and blow it up. Do not tie the balloon. Knead the balloon (you "knead" a balloon for this experiment) to reduce the elasticity. Deflate the balloon. Blow up the balloon to a size which will fit easily into a 600 or 1000 ml beaker. Allow plenty of extra room. Tie the end of the balloon.
2. Fill the beaker about half full of water. Place the balloon in the water and subtract the volume of the water from the volume of the water plys ballon when the balloon is immersed in the water. Record the volume of the balloon and the temperature of the water.
3. Heat the water an balloon to about 80 degress C. Repeat step two.
4. Pur out the hot water and add ice plus water. Cool the balloon to 0-10 degrees C and repeat step two.
5. Clean up your mess.
Data Table-
Temperature (degrees C) Volume of gas in balloon
Questions:
1. Make a graph of volume versus temperature. Let the x-axis be temperature and the y-axis be volume. Scale the graph so as much of it is used as possible.
2. What type of curve did you obtain? (parabola, straight line, hyperbola, ellipse, circle,etc)
3. What does this tell you about the relationship between volume and temperature for a gas?
4. What is the significance of the temperature at which the balloon would occupy no volume?
Label your Graph completely!!