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# Charles Law Lab Report Essay

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I9 EXPERIMENT Charles’Law MATERIALS AND EQUIPMENT 125 mL Erlenmeyer flask, one-hole rubber stopper, glass and rubber tubing, pneumatic trough, thermometer, screw clamp. DISCUSSION The quantitative relationship between the volume and the absolute temperature of a gas is summartzed in Charles’law. This law states: at constant pressure, the volume of a particular sample of gas is directly proportional to the absolute temperature. Charles’ law may be expressed mathematically: V “. T (constant pressure) V = kT o, : T = k (constant pressure) (1) (2) here V is volume, T is Kelvin temperature, and k is a proportionality constant. dependent on the number of moles and the pressure of the gas. If the volume of the same sample of gas is measured at two temperatures, V1/T1 = k and V2/T2- k, and we may say that V, V, or V” = (V,f[]) z T1 T2 “[Tr/ {. o. rrt. nt pressure) (3) where V1 and T, represent one set of conditions and V2 and T2 a different set of conditions, with pressure the same at both conditions. Experimental Verification of Charles’ Law This experiment measures the volume of an air sample at two temperatures, a high temperature, Ts, and a low temperature, T1.

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. 1. 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. 2. 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*) . =Sffi (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.

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. 168 NAME SECTION DATE REPORT FOREXPERIMENT 19 Charles’Law INSTRUCTOR Data Table Tlial 1 Temperature of boiling water, Ts Temperature of cold water, Tp Volume of water collected in flask (decreasein volume due to cooling) -oC, OC. K -OC, -OC, T? ial 2 -K -K -K Volume of air at higher temperature, Vs (volume of flask measured onlv after Trial 2) Volume of wet air at lower temperature (volume of flask less volume of water collected),V””p Atmosphere pressure, P”t(barometer reading)

Vapor pressure of water at lower temperature, Puoo (seeAppendix 6) 169 REPORT FOR EXPERIMENT 19 (continued) NAME CALCULATIONS: In the spaces below, show calculation setups for T? ial 1 only. Show answers for both trials in the boxes Tbial 1 1. Corrected experimental volume of dry air at the lower temperature calculated from data obtained at the lower temperature. (a) Pressure of dry air (Ppa) POL=PAr–Pg”O T)ial2 (b) Corrected experimental volume of dry air (lower temperature). = vnr=(%*’)|. +tl Po,”[ J 2 . Predicted volume of dry air at lower temperature

Vs calculated by Charles’ law from volume at higher temperature (VH). vL=(v”)+l . . (r) rTHJ 3. Percentage error in verification of Charles’law. Voo – Vt vo etror = x loo VL 4. Comparison experimentalV/T ratios. (Use dry of volumesand absolutetemperatures. ) (a) vH = TH (b) vna = TL 170 REPORT FOIt. u,lxp. t)RIMENT 19 (continued) NALE 5 . On the graph paper provided, plot the volume- temperature values used in Calculation 4. Temperature data must be in oC. Draw a straight line between the two plotted points and extrapolate (extend) the line so that it crosses the temperature axis.

Is 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 heated? 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? oc (b) At what temperature does Charles’law predict that the extrapolated line should intersect the r-axis? oc t72 REPORT FOR EXPERIMENT 19 (continued) NAME J E o E = 173

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