Iits number 2 on the sheet! Thank you! Length of Air Column (thermometer units)50Lab 14Charles' LawIntroduction:The volume an amount of trapped gas occupies depends on the temperature and pressureof the gas. If we increase the temperature of the gas while keeping the pressure of the gasconstant what happens to the volume of the gas? As the temperature of the gas increasesthe average kinetic energy of the gas particles increases. This means that the particles aremoving on average faster and with collide with the walls of the container more often andwith greater force. This would result in an increase in the pressure of the gas. The onlyway we can keep the pressure constant is to increase the volume of the gas. This allowsthe greater force to be distributed over a greater area, thus keeping the pressure constant.Similarly, if you decrease the temperature of the gas the volume decreases. Scientistswondered if there was a temperature so low that the volume of the gas would drop tozero. This would be the lowest temperature possible and could serve as the zero point inan absolute temperature scale. Since there is a linear relationship between temperatureand volume it is possible to measure the volume at different temperatures, plot the valueson a graph and extrapolate the line to the temperature where the volume would be zero.Charles' Law Graph09302010-250ode-Temperature (C)In this experiment you will be working with a sample of gas (air) trapped in a narrowglass capillary tube. The bottom of the tube is sealed and the gas is held in the tube by asmall plug of oil near the open end of the tube. This oil plug acts as a frictionless pistonthat allows the volume of the gas to expand as the temperature increases. This keeps thepressure inside the tube equal to the constant pressure of the atmosphere.Since the gas is in a cylindrical container the volume of the container can be calculated:V = Tr" 1, where r= gas.inner radius of the capillary and 1 = length of the column ofSince r and rt are constant, you can simply plot the length in place of the volume in yourgraph. You can measure the length of this column using the markings on your%3D%3Dhermometer. Lab 14Charles' LawReport SheetName Alexandra TLab DayScale reading of bottom of capillary tube I2810.2Scale readingScale reading of top of capillary tubeTemp °C25.23655.1283031.933.985.23739-0: - 143.125TLEて2Calculated temperature at which length would = 0 : ~Questions:1. Will the volume of the air in the tube actually fall to zero if you lowered thetemperature of the gas to -273°C? Why or why not. The two main components of air arethe real gases N2 and O2. Look up the melting and boiling points of these two gases.These numbers may help you answer this question.%3D2. We assumed that during the course of the experiment the atmospheric pressure in theroom was constant, however this may not be so. Explain the following: If the pressure inthe room decreased while you were heating the gas, the volume of the gas would stillincrease. But if the pressure in the room increased while you were heating the thevolume of the gas may increase, decrease or even remain the same during the course ofthe experiment.gas,3. Use the best fit equation that was calculated by excel for your data to calculate thetemperature to which the gas would need to be increased so that it would occupy theentire capillary tube. You will need to calculate the length of the capillary tube inthermometer units to answer this question.9.

Question

Iits number 2 on the sheet! Thank you! Length of Air Column (thermometer units)50Lab 14Charles' LawIntroduction:The volume an amount of trapped gas occupies depends on the temperature and pressureof the gas. If we increase the temperature of the gas while keeping the pressure of the gasconstant what happens to the volume of the gas? As the temperature of the gas increasesthe average kinetic energy of the gas particles increases. This means that the particles aremoving on average faster and with collide with the walls of the container more often andwith greater force. This would result in an increase in the pressure of the gas. The onlyway we can keep the pressure constant is to increase the volume of the gas. This allowsthe greater force to be distributed over a greater area, thus keeping the pressure constant.Similarly, if you decrease the temperature of the gas the volume decreases. Scientistswondered if there was a temperature so low that the volume of the gas would drop tozero. This would be the lowest temperature possible and could serve as the zero point inan absolute temperature scale. Since there is a linear relationship between temperatureand volume it is possible to measure the volume at different temperatures, plot the valueson a graph and extrapolate the line to the temperature where the volume would be zero.Charles' Law Graph09302010-250ode-Temperature (C)In this experiment you will be working with a sample of gas (air) trapped in a narrowglass capillary tube. The bottom of the tube is sealed and the gas is held in the tube by asmall plug of oil near the open end of the tube. This oil plug acts as a frictionless pistonthat allows the volume of the gas to expand as the temperature increases. This keeps thepressure inside the tube equal to the constant pressure of the atmosphere.Since the gas is in a cylindrical container the volume of the container can be calculated:V = Tr&#34; 1, where r= gas.inner radius of the capillary and 1 = length of the column ofSince r and rt are constant, you can simply plot the length in place of the volume in yourgraph. You can measure the length of this column using the markings on your%3D%3Dhermometer. Lab 14Charles' LawReport SheetName Alexandra TLab DayScale reading of bottom of capillary tube I2810.2Scale readingScale reading of top of capillary tubeTemp °C25.23655.1283031.933.985.23739-0: - 143.125TLEて2Calculated temperature at which length would = 0 : ~Questions:1. Will the volume of the air in the tube actually fall to zero if you lowered thetemperature of the gas to -273°C? Why or why not. The two main components of air arethe real gases N2 and O2. Look up the melting and boiling points of these two gases.These numbers may help you answer this question.%3D2. We assumed that during the course of the experiment the atmospheric pressure in theroom was constant, however this may not be so. Explain the following: If the pressure inthe room decreased while you were heating the gas, the volume of the gas would stillincrease. But if the pressure in the room increased while you were heating the thevolume of the gas may increase, decrease or even remain the same during the course ofthe experiment.gas,3. Use the best fit equation that was calculated by excel for your data to calculate thetemperature to which the gas would need to be increased so that it would occupy theentire capillary tube. You will need to calculate the length of the capillary tube inthermometer units to answer this question.9.

Accepted Answer

As per the phenomenon of the expansion of gas in a piston, it is known that if external pressure is…