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# Gas Laws (Lab Report Sample)

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the task was to write a lab report on gas laws. the sample provided presents a lab report on the topic and calculations based on the data obtained from the lab

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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
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
TrialT, Kelvin (K)P,mmHgV,ml1Initial (hot)371.0741.932561Final (cool)294.6724.432112Initial (hot)371.5741.68261.92Final (cool)295.3722.98227.4
Table 2: Measurements for Mass of Condensed vapor
Trial 1Trial 2Trial 3Mass of flask and cap, empty (g)91.29g89.52g91.53gMass of flask and cap, w/condensed vapor (g)91.63g89.77g91.74gMass (m) of Condensed vapor (g)0.34g0.25g0.21gTemperature (T) of boiling water bath (°C)98.3°C99°C96.7°CTemperature (T) of boiling water bath (K)371.3K372K365.7KPressure (P) inside the lab (mmHg)29.2129.2129.21Pressure (P) inside the lab (mmHg)0.97620.97620.9762Volume (V) of flask (ml)161ml166ml157.5mlVolume (V) of flask (L)0.161L0.166L0.1576LMolar Mass of the Unknown Liquid (g/mol)66g/ml47g/mlAverage 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). ...
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