Molar Mass Of Butane Lab

Lab Written report on the Molar Mass of Butane

✅ Paper Type: Free Essay	✅ Bailiwick: Chemistry
✅ Wordcount: 1481 words	✅ Published: tertiary Nov 2020

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Introduction

As the world of chemistry constantly evolves, certain elements, compounds, and fifty-fifty substances are always undergoing substance identification. Moreover, at that place are many methods to identify a substance. As noted by Austin Peay State University's department of chemistry, the identification of a substance can be adamant by making simple observations such as odor, temperature, and well-nigh importantly, color. However, some gas substances cannot exist hands observed for their color. In such cases, determining the tooth mass of the substance can show to be helpful in substance identification.

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According to Purdue University's section of chemistry, for many chemists, it is impractical to collect and measure gas because gases have small densities. However, considering butane is non soluble in water, information technology allows for water to be displaced from a container. In doing and so, it facilitates the drove of gas. In Dalton's Constabulary of partial of pressures, the full pressure in a container is equal to the sum of the gas nerveless and water vapor.

In 1834, physicist Emil Clapeyron wrote an equation that assisted many chemists in agreement the behavior of everyday gases. Clapeyron equation is recognized equally the ideal gas constabulary and is written as PV=nRT. It states that the product of a gas'southward volume (L) and force per unit area (atm) is proportional to the product of the gas constant, moles (mol), temperature (Grand). The gas constant, "R" has an verbal value of 0.0821 L*atm/mol*k. This equation is of import because the number of moles, "northward", can exist used to determine the tooth mass of butane by rearranging the equation to north=PV/RT. In this experiment, the moles and mass volition exist required to determine the molar mass of butane in a butane lighter.

Experimental

To begin the experiment, the mass of a butane lighter was measured before using the butane gas to deplete the water to the 80mL marking on a graduated cylinder. Secondly, the temperature of the of the water was measured afterwards waiting v minutes for the temperature to remain constant. Afterwards, the mass of the butane lighter was measured a 2nd time to decide the displacement.

In calculating the molar mass, the platonic gas law was used to offset decide the number of moles. Finally, the mass of the butane displaced was divided past the moles to eventually produce the molar mass of the butane. The experiment was repeated for four trials.

Results

Table 1: Data of tooth mass experiment

	Units	Trial 1	Trial 2	Trial three	Trial iv
Initial Mass of Lighter	g	14.053	fourteen.827	16.234	13.903
Terminal Mass of Lighter	g	14.273	xv.060	sixteen.346	14.071
Mass of Butane	g	0.220	0.233	0.112	0.168
Volume of Gas collected	50	0.101	0.084	0.094	0.082
Air temperature	Thousand	293.000	293.000	293.000	293.000
Water temperature	Yard	293.000	293.000	293.000	293.000
Vapor pressure of H₂O	atm	0.023	0.023	0.023	0.023
Barometric Pressure	atm	0.988	0.988	0.988	0.988
Accustomed Tooth Mass of Butane	58.12g/mol

Certain data included in the table were given as a standard. That standard was used to compare the experimental result to. The accepted molar mass of butane, vapor pressure level of H₂O and barometric force per unit area was given as a standard.

Table 2: Number of moles by the equation n=PV/RT for trials 1-4

Trial 1 Data	northward=PV/RT (mol)	Trial 2 Information	n=PV/RT (mol)
P= 0.9649	0.004	P= 0.9649	0.003
V= 0.101		Five= 0.084
R= 293		R= 293
T= 0.0821		T= 0.0821

Trial 3 Data	north=PV/RT (mol)	Trial 4 Data	n=PV/RT (mol)
P= 0.9649	0.004	P= 0.9649	0.003
V= 0.094		Five= 0.082
R= 293		R= 293
T= 0.0821		T= 0.0821

The number of moles was calculated past multiplying the pressure and volume and dividing that product by the abiding gas and temperature. The pressure level was determined past subtracting the pressure level of H₂O from the total pressure.

Table iii: Tooth mass of butane calculations

The tooth mass was calculated by dividing the mass of butane by the experimental number of moles. The boilerplate of all four trials resulted in a molar mass of 54.17g/mol.

Discussion

The experiment was designed to be able to facilitate substance identification by determining the molar mass of butane. The tooth mass of butane was found by first computing the number of moles using the ideal gas law, northward=PV/RT. Next, the mass of the butane displaced was divided by the moles to finally give the molar mass of the butane. The boilerplate experimental molar mass resulted in 54.17g/mol while the accepted value was 58.12g/mol. This is a percent mistake of 6.779%. In the futurity, this experiment tin can exist improved upon past not letting the butane gas escape the graduated cylinder. In doing then, it will allow for more accurate results when calculating.

Bibliography

"Identification of a Pure Substance." Austin Peay Land Academy Section of Chemistry, Chem 1111 Lab Handouts. Revision S18.
Finding the Tooth Mass of Butane. University of Illinois Urbana-Champaign, www.chem.uiuc.edu/chem103/molar_mass/introduction.htm.
Collection of Gas Over Water. Purdue University, chemed.chem.purdue.edu/genchem/lab/techniques/gascollect.html.

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