In the prior lab we went over two of the relationships of the ideal gas law and in this lab is to show the volume vs. temperature. In order to find the relationship we had a syringe connected to a flask and placing in three different temperature baths. This was done to find the change of the cc(cubic centimeter) of the syringe depending on the temperature of the water. As a result we found that both volume and temperature have a linear relationship and now having the three relationships, we were able to see how the ideal gas law's components.
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This is the set up of the experiment in order to find the relationship between volume and temperature, which turned out to be directly proportional.
The pressure stays constant in Charles Law even though the volume changes is because the pressure is sealed using the flask in which only the gas particles(water vapors) start increasing the heat causing the syringe to start moving.
Another picture of the lab set up and procedure using the equipment to find the way temperature affects the volume change in the syringe cut off with same constant pressure, Charles Law.
The uncertainty part or value of this lab was the size of the flask, which is the volume value at the beginning it was too big, 139 cm^3, giving inconsistent values causing for the use of a smaller flask with a new volume of 39.9 cm^3. Also part of the problem of the beginning of the lab was temperature of the water because when it was too hot the syringe popped out and when it was too cold, the syringe went down all the way; as a result we had to fluctuate the water temperature enough to have a value within a 10 degree change to have a consistent and appropriate amount of volume moving in the syringe.
The group's calculations and data points of the experiment in different temperature baths, also the graph showing the relationship temperature vs. volume having the units of cm^3/K. In order to find the coefficient the slope was used to find the units.
The slope of the volume vs. temperature is the constant V1/T1 = V2/T2 because in this scenario the pressure is constant.
We found the units of the coefficient to be in cm^3/K however there is constant R =8.314 atm*L/mol*K where the pressure is constant and described in the ideal gas laws. The variable n is for the moles of the material within the experiment.
The three relationships between pressure, volume, and temperature to manipulate the equations to come up with the ideal gas law. The constant rate is 8.314 Pa*cm^3/mol*K.
The lab set up with the syringe and flask to find the relationship between the volume and temperature, which resulted to be directly proportional.
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