charles' law lab report essay

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IB Chemistry - Charles' Law Lab Report

Gas laws experiment

Relationship between Volume and Temperature and find Absolute Zero

Aim : to measure accurately the volume of a fixed mass of gas at different temperatures and use these data to determine the relationship between the variable and to determine absolute zero, the temperature at which the volume would theoretically drop to zero.

• The volume of water in 250ml beaker = 150ml

Data Processing

• % of uncertainty on temperature  = 0.5/temperature*100 = 0.5/24*100 = 2.08 = ±2%
• Absolute uncertainty on temperature =   temperature*% of uncertainty on temperature = 24*2% = ±0.48
• Kelvin = ℃+273  = 24+273 = 297
• Height  = End of capillary – Bottom of bubble = 6.0 – 2.2 = 3.8cm
• % of uncertainty on height  = % of uncertainty on the end of capillary + % of uncertainty on the bottom of bubble = (0.05/6.0*100) + (0.05/height*100) = 0.83+ (0.05/3.8*100) = 0.83 + 1.32 = 2.15= ±2%
• Absolute uncertainty on height =   Height*% of uncertainty on height = 3.8*2% = ±0.076
• H(V)/T = k(constant)  = 3.8/279 = 0.014 (Temperature should be replaced into Kelvin)
• % of uncertainty on constant =   % of uncertainty on temperature + % of uncertainty on height = 2 + 2 = 4%
• Absolute uncertainty on constant = constant*% of uncertainty on constant

= 0.014*4% = 5.6*10∧-4

• Form the graph that has been made by the result of the experiment, the relationship between temperature and height (which is same as height in this experiment) was directly proportional.

This is a preview of the whole essay

• The Charles’ law defined that the relationship between temperature and the volume for a gas at constant pressure is linear or V=k (constant)T. Every gas we use gives the same value of temperature for this intercept, -273℃ and the behaviour of gases tells us that the temperature has an absolute zero. So if I want to double the volume at constant pressure of a gas initially at 10℃, I heat it to 293℃ not 20℃.
• A) Effect of changing the pressure at constant temperature : From the Kinetic Molecular Theory, temperature (heat) is the kinetic energy in an atom. Therefore the more kinetic energy molecules have, the higher temperature is. If the kinetic energy is constant which mean the temperature is at constant, only volume can decrease or increase the level of pressure. If I want to increase the pressure which means I want molecules hit each other more frequently, then volume will decrease so that the space that atoms have will be less so molecules will hit each other more frequently. On the other hand, if the pressure decreases, volume will increase according to the Boyles’ law that volume and pressure are inversely proportional.
• B) Effect of changing the temperature at constant pressure : At constant pressure, the temperature will either increase or decrease. So, volume will change depends on how the temperature will change. This phenomenon was proved by Charles who said the temperature and the volume are directly related. For example, if the temperature increases, the volume will increase. If temperature decreases, the volume will decrease and vice versa. This could happen due to the speed of molecules. If temperature is high, kinetic energy will increase then the seed of molecules will increase too which means the space (volume) will be bigger due to molecules’ collision. On contrast, if temperature is low, kinetic energy will decrease then the speed of molecules will decrease too which means their power of collision will slow down so volume will decrease. This is shown prominently for gas because molecules in gas are more freely moveable.  

From the experiment, I was able to find out the relationship between the temperature and the height (I used height instead of using volume because these are same) that the temperature and the height were directly related. To find the height, I had to subtract the scale of the end of capillary from the scale of the bottom of bubble. And, for the temperature, all I had to do was just read the scale of thermometer per 10℃. And then I need to change the Celsius into the Kelvin temperature because, the Lord Kelvin said that a reasonable temperature scale should start at a true zero value. Therefore, according to the results, when the temperature increased, the height (volume) increased too. However, the constancy keeps increasing in the results which must be similar to each other’s. . According to the Charles’ law, the temperature and the volume (height) are directly proportional. Therefore, the height (volume)*inversed temperature showed constancy. Moreover, there was not vast difference between temperatures. It was because of the substance of molecules that we used liquid. The characteristics of liquid are definite volume, take the shape its container and incompressible. Moreover, the motion of molecules in liquid is less random than that of gas. Therefore, there was not significant reduction.

Absolute zero is the coldest temperature that the atoms can be which is -273℃. When the atoms are all stopped the gas is absolutely as cold as can be so we call this phenomenon as absolute zero. When the temperature is -273℃, the volume will be 0. However, gases do not really reach a 0 volume but the spaces between molecules approach 0. We use the unit called Kelvin (K) because absolute zero means the temperature never goes down more than -273℃ so we make the temperature as positive value to calculate easier.

There were few limitations in my experiment. The height difference between at 82℃ (right after boiling the water) and at 24℃ (room temperature) was quite strange. According to the theory, at 82℃, the height (volume) must be the greatest but in the experiment, the height showed the lowest scale. Moreover, it does not show a graphically straight line which means there was something wrong with the temperature. I think that was because of the room temperature or the problem in cooling process. When we cool the water, we used ice for saving time otherwise it will take hours till the room temperature. Besides, we are not sure that the temperature will be constant in the room. Then the speed of cooling time will be different and there might be error in calculating the volume which is height in this experiment. There were huge uncertainties which were affected by the ruler I think. The ruler did not have more detailed scale like electronic rulers. Though we can see the gap between the smallest unit but we can write it down because we do not know exactly what it is.

Improvement

To improve the experiment, we may do more trials to make the experiment more accurate. Also, make it sure that our experiment will be done under the exactly same circumstance. So that there will not be any mistake in temperature and proportion with volume. Sometimes, we missed to measure the height at proper temperature so we assumed the approximate height. For the next time, make it sure that we must be always ready for taking the scale of height at right temperature. At some temperature, the bubble thingy did not move at all. For example, at 72℃ and 62℃, there was not any difference in height. That might be because of inappropriate working problem. We have to make it sure that the equipment works properly. Besides, preparing more accurate ruler may help to reduce uncertainties.

Document Details

• Word Count 1514
• Page Count 6
• Level International Baccalaureate
• Subject Chemistry

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Charles Law Lab Report Essay Example

• Pages: 4 (852 words)
• Published: April 28, 2017
• Type: Laboratory Work

The volume of the air sample at the high temperature, (Vn),decreases when the sample is cooled to the low temperature and becomesV1. All of these measurements are made directly. The experimental data is then used to verify Charles'law by two methods: 1. The experimental volume (V""o) measured at the low temperature is compared to the V1 predicted by Charles' law where Yy(t oretic (vH,[ he at)= + ) 165 2. The V/T ratios for the air sample measured at both the high and the low temperatures are compared. Charles'law predicts that these ratios will be equal. V"_V" TH TL

Pressure Considerations

The relationship between temperature and volume defined by Charles' law is valid only if the pressure is the same when the volume is measured at each temperature. That is not the case in this experiment.

• The volume, Vs, of air at the higher temperature, Ts, is measured at atmospheric pressure' P"t* in a dry Erlenmeyer flask. The air is assumed to be dry and the pres. nr" is obtained from a barometer.
• The experimental air volume, (V"*p) at the lower temperature, Tp, is measured. over water. This volume is saturated with water vapor that contributes to the total pressure in the flask.

Therefore, the experimental volume must be corrected to the volume of dry anrat atmospheric pressure. This is done using Boyle's law as follows: a. The partial pressure of the dry air, Poo, is calculated by subtracting the vapor pressure of water from atmospheric pressure: P. r--PffrO=POA b. The volume that this dry air would occupy at Pur,''is then calculated using the Boyle's law equation: = (%,. oXp*) (voo)(%,_) (%,. oXp*). =Sff

(voo) PROCEDURE Wear protective glasses. NOTE: It is essential that the Erlenmeyer flask and rubber stopper assemblvbe as drv as possiblein order to obtain reproducibleresults.

Dry a L25 mL Erlenmeyer flask by gently heating the entire outer surface with a burner flame. Care must be used in heating to avoid breaking the flask. If the flask is wet, first wipe the inner and outer surfaces with a towel to remove nearly all the water. Then, holding the flask with a test tube holder, gently heat the entire flask. Avoid placing the flask directly in the flame. Allow to cool. While the flask is cooling select a l-hole rubber stopper to fit the flask and insert a b cm piece of glass tubing into the stopper so that the end of the tubing is flush with the bottom of 66 the stopper. Attach a 3 cm piece of rubbertubingto the glass tubing (see Figure 19. 1-). Insert (wax pencil) the distance that it is inserted. Clamp the the stopper into the flask and mark flask so that it is submerged as far as possible in water contained in a 400 mL beaker (without the flask touching the bottom of the beaker) (see Figure I9. 2). Heat the water to boiling. Keep the flask in the gently boiling water for at least 8 minutes to allow the air in the flask to attain the temperature of the boiling water. Add water as needed to maintain the water level in the beaker.

Read and record the temperature of the boiling water. While the flask is still in the boiling water, seal it by clamping the rubber tubing tightly

with a screw clamp. Remove the flask from the hot water and submerge it in a pan of cold water, keeping the top down at all times to avoid losing air. Remove the screw clamp, letting the cold water flow into the flask. Keep the flask totally submerged for about 6 minutes to allow the flask and contents to attain the temperature of the water. Read and record the temperature of the water in the pan. Figure 19. Rubber stopper assembly Figure 19. 2 Heating the flask (and air) in boiling water t67 In order to equalize the pressure inside the flask with that of the atmosphere, bring the water level in the flask to the same level as the water in the pan by raising or lowering the flask (see Figure 19. 3). With the water levels equal, pinch the rubber tubing to close the flask. Remove the flask from the water and set it down on the laboratory bench. Using a graduated cylinder carefully measure and record the volume of liquid in the flask. Repeat the entire experiment.

Use the same flask and flame dry again; make sure that the rubber stopper assembly is thoroughly dried inside and outside. After the second trial fill the flask to the brim with water and insert the stopper assembly to the mark, letting the glass and rubber frll to the top and overflow. Measure the volume of water in the flask. Since this volume is the total volume of the flask, record it as the volume of air at the higher temperature. Because the same flask is used in both trials. it is necessarv to make

this measurement onlv once. Figure 19. 3 Equalizing the pressure in the flask.

The water level inside the flask is adjusted to the level of the water in the pan by raising or lowering the flask.

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Charles Law Lab Report

This sample paper on Charles Law Lab Report offers a framework of relevant facts based on recent research in the field. Read the introductory part, body, and conclusion of the paper below.

The volume of the air sample at the high temperature, when the sample is cooled to the low enrapture and becomes. All of these measurements are made directly. The experimental data is then used to verify Charleston by two methods: 1. The experimental volume (V””o) measured at the low temperature is compared to the VI predicted by Charles’ law where Y(t erotic at)- ) 2.

The WET ratios for the air sample measured at both the high and the low temperatures are compared, Charleston predicts that these ratios will be equal.

Pressure Considerations The relationship between temperature and volume defined by Charles’ law is valid Only if the pressure is the same When the volume s measured at each temperature. That is not the case in this experiment. 1. The volume, Vs…… Of air at the higher temperature, TTS is measured at atmospheric pressure’ in a dry Erlenmeyer flask.

The air is assumed to be dry and the pres. NRC” is obtained from a barometer. 2. The experimental air volume, at the lower temperature, Tip, is measured. Over water.

This volume is saturated with water vapor that contributes to the total pressure in the flask. Therefore, the experimental volume must be corrected to the volume of dry Ankara atmospheric pressure. This is done using Bole’s law as follows: a. The partial pressure of the dry air, Poor is calculated by subtracting the vapor pressure of water from atmospheric pressure: P.

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R–From-POP b. The volume that this dry air would occupy at Purr,’IIS then calculated using the Bole’s law equation: = =Sift (vivo) PROCEDURE Wear protective glasses.

Why Can The Erlenmeyer Flask Be Wet

NOTE: It is essential that the Erlenmeyer flask and rubber stopper assembled as dry as possible order to obtain reproducibility’s_ Dry a 125 ml Erlenmeyer flask by gently heating the entire outer surface with a burner flame. Care must be used in heating to avoid breaking the flask. Fifth flask is wet, first Wipe the inner and outer surfaces with a towel to remove nearly all the water. Then, holding the flask With a test tube holder, gently heat the entire flask. Avoid placing the flask directly in the flame. Allow to cool.

While the flask is cooling select a I-hole rubber stopper to fit the flask and insert a b CM piece Of glass tubing into the stopper so that the end of the tubing is flush with the bottom of the stopwatches a 3 CM piece of reprobating the glass tubing (see Figure 19. 1-). Insert (wax pencil) the distance that it is inserted. Clamp the the stopper onto the flask and mark flask so that it is submerged as far as possible in water contained in a 400 ml beaker (without the flask touching the bottom of the beaker) (see Figure 19. 2). Heat the water to boiling.

Keep the flask in the gently boiling water tort at least 8 minutes to allow the air in the atlas to attain the temperature of the boiling water. Add water as needed to maintain the water level in the beaker. Read and record the temperature of the boiling water. While the flask is still in the boiling water, seal it by clamping the rubber tubing tightly with a screw clamp. Remove the flask from the hot water and submerge it in a an of cold water, keeping the top down at all times to avoid losing aim Remove the screw clamp, letting the cold water flow into the flask.

Keep the flask totally submerged for about 6 minutes to allow the flask and contents to attain the temperature of the water. Read and record the temperature of the water in the pan. Figure 19. I Rubber stopper assembly Figure 192 Heating the flask (and air) in boiling water In order to equalize the pressure inside the flask with that of the atmosphere, bring the water level in the flask to the same level as the water in the pan by raising or lowering the flask (see Figure 19. ). With the water levels equal, pinch the rubber tubing to close the flask.

Remove the flask from the water and set it down on the laboratory bench. Using a graduated cylinder carefully measure and record the volume of liquid in the flask, Repeat the entire experiment, use the same flask and flame dry again; make sure that the rubber stopper assembly is thoroughly dried inside and outside, After the second trial fill the flask to the brim with water and insert the stopper assembly to the mark, letting the glass and rubber furl to the top and overflows Measure the volume of water in the flask.

Since this volume is the total volume of the flask, record it as the volume of air at the higher temperature. Because the same flask is used in both trials. It is necessary to make this measurement only once. Figure 19. 3 Equalizing the pressure in the flask. The water level inside the flask is adjusted to the level Of the water in the pan by raising or lowering the flask. NAME SECTION DATE REPORT PRESENTIMENT 19 Charleston INSTRUCTOR Data Table Tail 1 Temperature of boiling water, TTS Temperature of cold water, Tip Volume of water collected in flask (decrease volume due to cooling) -co CO.

K – co, -co, T? Ill 2 Volume of air at higher temperature, Vs….. (volume of flask measured only after Trial 2) Volume of wet air at lower temperature (volume of flask less volume of water Atmosphere pressure, reading) Vapor pressure of water at lower temperature, Poop (expanding 6) REPORT FOR EXPERIMENT 19 (continued) NAME CALCULATIONS: In the spaces below, show calculation setups for T? Ill 1 only.

Show answers for both trials in the boxes T bill I I, Corrected experimental volume of dry air at the lower temperature calculated from data obtained at the lower temperature. A) Pressure of dry air (App) T)IA (b) Corrected experimental volume Of dry air (lower temperature). 2 . Predicted volume of dry air at lower temperature Vs….. Calculated by Charles’ law from volume at higher temperature (VHF). Roth 3. Percentage error in verification of Charleston. Vivo – Vt vow terror = x lo FL 4. Comparison experimental/T ratios. Use dry of volumes obstreperousness’s. ) (b) ;nun = REPORT MEET 1 g (continued) ANAL 5 . On the graph paper provided, plot the volume- temperature values used in Calculation 4. Temperature data must be in co. Draw a straight line be,even he two plotted points and extrapolate (extend) the line so that it crosses the temperature axis. QUEUE ACTIONS ADD PROBLEMS 1 . (a) In the experiment, why are the water levels inside and outside the flask equalized before removing the flask from the cold water? B) When the water level is higher inside than outside the flask. Is the gas pressure in the flask higher than, lower than, or the same as, the atmospheric pressure? (specify which) 2. A L AS ml sample of dry air at 230″C is cooled to OIC”C at constant pressure, What volume will the dry air occupy at 100″C? 3. A 250 ml container of a gas is at CO’S_ At what temperature will the gas occupy a volume of 125 ml, the pressure remaining constant? 4 . (a) An open flask of air is cooled.

Answer the following: 1. Under which conditions, before or after cooling, does the flask contain more gas molecules? 2. Is the pressure in the flask at the lower temperature the same as, greater than, or less than the pressure in the flask before it was cooled? (b) An open flask of air is heated, stopper in the heated condition, and then allowed to cool back to mom temperature. Answer the following: 1. Does the flask notation the same, more, or fewer gas molecules now compared to before it was heated? 2. 5 the volume occupied by the gas in the flask approximately the same, greater, or less than before it was heated? 3. Is the pressure in the flask the same, greater, or less than before the flask was 4. DO any Of the above conditions explain Why water rushed into the flask at the lower temperature in the experiment? Amplify your answer. 5. On the graph you plotted, (a) At what temperature does the extrapolated line intersect the r. Axis? Co (b) At what temperature does Charleston predict that the extrapolated line should intersect the r-axis?

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