Lab 3 Ideal Gas laws ->Rapidly Imploding Can, The Manometer Setup, Ideal Gas Law verification(LoggerPro), Balloon and marshmallow demonstration(imperfect)<-

Rapidly Imploding Can
Boiling water in can and dunking it in cold reservoir water

Imploding Can Setup and demo.

Prediction:The can will fast implode because of PV=nrT

In demo, we heated the water inside a soda can and then turned it upside down into a container filled with cold water. We observed the affects the temperature change would have on the can. It was discovered that as the temperature decreases (ice bath) the volume decreases as well (imploding of can). Thus, according to demo, the steam inside the can immediately condenses and act as if a vacuum condensing the can very fast. 

We were asked to find the relationship between force and momentum.

The Manometer Setup

Pressure=F over area
Manometer formulaic explanation.

   Pressure is found by first finding the height difference from the equilibrium point. Then, the point after blowing into the straw is found later. Based on the calculations in the picture,  the pressure is dependent on the height of the water. The density and the value of gravity remains the same and so using Pressure=Force/Area, the formula can be rearranged to find the weight of the column of water. Manometer used most widely in thermometers and various thermo measuring devices. 

Ideal Gas Law verification(loggerPro)

Prediction

For this part of Lab, we predicted syringe as it will have linear relationship from 20 mL of air to 5 mL of air against the pressure as the result. But result surprises us because the non-linear nature of pressure and volume shown in Logger Pro graph.

However, realistically, the result came as a inverse relationship.

We tried to fit it using linear line Pressure=MV+b which surprisingly have a high correlation but doesn't really explain the graph visually. But by convention, we use a inversely proportion comparison between pressure and volume

 

   Overall, we determined the relationship between pressure and temperature would be linear and proportional. After the experiment, putting a 125 mL flask into boiling water, the prediction was proven correct. Although showing some error, the LoggerPro graph is roughly linear. When giving the physical meaning to the best fit line, it looks similar to P=P₀+ρgh equation.

   After studying the relationship between temperature and volume, a 25 mL flask was put in a beaker of cold water, room temperature water, and hot water and the pressures were recorded for each beaker of water. By using LoggerPro from its trendline equation, we have supported a linear relationship between the two.

   Furthermore, the pressure is constant, the volume is able to change because the temperature is changing as well. Thus, volume and temperature are proportional and that when one increases, other increases also from the assumption that the pressure is kept constant.

Concluding Boyles and Charles Law below

   From knowledge gained from previous experiments, the relationship between volume, temperature and pressure were combined to make an equation. However, because temperature is constant, we can replace that with c₃ and make the equation of Pressure=constant/Volume. And this supports the previous prediction of pressure and volume being inversely proportional according to Boyles law.

Prediction of Balloon 1 to .1 to 1.1 atm

Balloon and marshmallow demonstration(imperfect) demonstration

Marsh-mellow shrinking
experiment,
due to imperfections, the
marshmallow
 will be blown up due to air
cavities.

Observation of the balloon expanding

Balloon expanding in a pressure meter.

Video of 1 atm to .1 atm.

Video of .1 atm to normal 1 atm.

   Analysis: In expanding balloon experiment, prediction of the balloon will increase in size when the pressure decreases and when the pressure returns to its original state, as well as the balloon. It was proven that the volume increase when pressure was decreased. However, when the pressure returned to the original pressure, the balloon shrunk smaller than its original size. This is due to the loss in n, number of moles. It is highly possible that gas molecules escaped during the experiment of the pressure machine.
   For the second experiment with the marshmallows, a similar predictions were made that a increase in volume with a decrease in pressure and a smaller than its original size when pressure returned to normal because we were thinking of its imperfectsions. After performing the experiment, it was seen that the marshmallow did increase in size when pressure decreased, like the balloon, the marshmallow had a smaller size because there were microscopic holes in the balloon and marshmallow that leaked air and the both of them loses part of their structure after expansion. Once again, this could also be due to the loss in the n.