Gas Laws (Lab Report Sample)

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Gas Laws: Lab Report
Introduction
An ideal gas is regarded as one in which all the collitions found between molecules or atoms are perfectly elastic. Additionally, ideal gases are assumed to lack the intermolecular forces of attraction. The goal of this experiment was to apply the ideal gas laws to calculate the volume of a gas and compare it with a measured volume in a lab experiment. Given that the ideal gas law can be rearranged mathematically to allow for the computation of the condensed vapor (H20g) of a volatile liquid, the objectives of the experiment included the application of the Condensed Gas Law and the calculation of the Molar Mass of a condensed vapor. The general objective was to learn about the Gas Laws.
Procedure
Combined Gas Law
A trough having regular tap water was prepared and 3 inches of temperature probe allowed to extend into the water trough for thermal equilibration. A single hole rubber stopper was then inserted in the neck of a dry, clean 250ml Erlenmeyer flask with a tapered glass tube stuck through the hole. A large beaker of water was then placed on a hot plate; the earlier prepared flask placed inside it (without turning it on); the bottom of the flask lowered into the water bath allowing the water level to rise up to the neck of the flask. The position of the flask was secured by clamping and a few boiling stones added to the water bath for regulating the boiling. The water bath was then heated by heating the hot plate until constant boiling was achieved and the water temperature measured using a thermometer. Keeping the water at the measured temperature ensured that the air in an Erlenmeyer flask and the boiling water were similar. Pressure (Pi) of air within the lab was then obtained by reading the barometer in the lab. Pressing the rubber stopper over the hot air flask tip, the flask was brought over the trough with no air escaping and holding the flask upside down, the neck of the flask was stuck under water. Water and not air was allowed to draw into the flask. Holding the flask under the water for ten minutes allowed the air temperature inside the flask to get to equilibrium with the water outside. The water volume drawn into the flask was then measured holding the flask up and down to match the level of water in the trough. The water volume enough to fill the buret tip and flask was also measured. The measurements for Vi, Vf, and Pi earlier taken were then recorded.
Molar mass of a condensed vapor
Aluminium foil was placed over 125ml Erlenmeyer flask and a pinhole made in the foil cap to allow for vapor escaping. The flask and the cap were then weighed and recorded. An unknown liquid was subjected to heat while inside a flask in the fume hood to determine the water bath temperature. The flask was then cooled at room temperature and the reappearance of condensed vapor noted. The cold flask, condensed vapor inside it, and the cap were weighed and recorded. This part was repeated to eliminate or reduce the error margins. The barometer was read to record the pressure (P) and the volume of flask determined by filling it with water and using a graduated cylinder to take the measurement.
Raw Data
Table 1: Gas Law Measurements
TrialT, Kelvin (K)P,mmHgV,ml1Initial (hot)371.0741.932561Final (cool)294.6724.432112Initial (hot)371.5741.68261.92Final (cool)295.3722.98227.4
Table 2: Measurements for Mass of Condensed vapor
Trial 1Trial 2Trial 3Mass of flask and cap, empty (g)91.29g89.52g91.53gMass of flask and cap, w/condensed vapor (g)91.63g89.77g91.74gMass (m) of Condensed vapor (g)0.34g0.25g0.21gTemperature (T) of boiling water bath (°C)98.3°C99°C96.7°CTemperature (T) of boiling water bath (K)371.3K372K365.7KPressure (P) inside the lab (mmHg)29.2129.2129.21Pressure (P) inside the lab (mmHg)0.97620.97620.9762Volume (V) of flask (ml)161ml166ml157.5mlVolume (V) of flask (L)0.161L0.166L0.1576LMolar Mass of the Unknown Liquid (g/mol)66g/ml47g/mlAverage Molar Mass (g/mol)Actual Molar Mass(g/mol)32.0416
Calculations
Vf (direct measured)= (Vi minus the volume of water drawn into the flask)
= 261.9- 44.5= 217.4ml
Vf (ml)= Vi (Pi/PfTf/Ti)
Pi = 741.68
Vi = 261.9
Ti = 371.5
Tf= 295.3
Pf= Pi- WVP at Tf= 741.68 - 18.7= 722.98
Vf (ml)= Vi (Pi/PfTf/Ti)
= 261.9× (741.68/722.98 × 295.3/371.5
Vf (experimental)= 261.9 (0.81865)
=213.57ml
Percentage difference = calculated v.s direct measurement *100
The difference = 3.83/ 217.4*100
= 1.76%
Molar Mass of a Condense Vapor
MM=mRT/PV
T= 365.7K
P= 29.21
Density= m/V= 0.34/0.1576= 2.1574
R= 0.082056
MM= 32.26
Results
Vf (direct measured) = 217.4ml
Vf (experimental)= 213.57ml
Percentage differenced= 1.76%
MM= 32.26
Discussion
The ideal gas law implies the law of the equation of state. The law applies to the ideal gases and describes the association between the partles number or amount n temperature T in Kelvin, pressure P in atmospheres (atm) and volume V measured in liters (L). the ideal gas law is abbreviated as PV=nRT (R= 0.082056 L-atm/mol-K- universal gas constant). ...