• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Butane Molar Mass Lab

Extracts from this document...

Introduction

Lab Partners Name Date November 8, 2009 Course Chemistry AP/IB Period 2 Butane's Molar Mass ABSTRACT Butane is a colorless gas with the molecular formula of C6H10 and is considered to be an Alkane. An Alkane is when the compound is formed by single bonds connecting the carbons and hydrogens. Butane was discovered by Dr. Walter Snellings in Pittsburg and he gas is used for cigarette lighters, heaters, stove fuels, and other heating appliances. The accepted value for the molar mass of butane is 58.124 g/mol. We tested the accepted value by calculating the molar mass of butane in a butane cigarette lighter. We took a beaker, and submerged it into water. Then we measured the mass of the cigarette lighter, and then slowly released butane gas bubbles into the beaker so that the bubbles collected at the top, where there was no air. We recorded the initial volume of water, then equalized the pressure inside and outside the beaker until the water levels inside and outside the beaker were the same. ...read more.

Middle

n = (0.976 atm)(0.0143 L) / (0.08206 Latm/molK)(295.65) n = 5.75e-4 n= PV/RT (Trial 3) n = (0.976 atm)(0.0158 L) / (0.08206 Latm/molK)(295.65) n = 6.356e-4 n= PV/RT (using averages) n = (0.976 atm)(0.0145 L) / (0.08206 Latm/molK)(295.65) n= 5.833e-4 Percent Error: The accepted value of the molar mass of butane is 58.124 g/mol. To calculate percent error: Trial 1: Difference between Calculated and Accepted values = 58.124 g/mol - 55.65 g/mol = 2.474 g/mol Trial 2: Difference between Calculated and Accepted values =58.124 g/mol - 69.53 g/mol = -11.406 g/mol Trial 3: Difference between Calculated and Accepted values = 58.124 g/mol - 47.20 g/mol = 10.924 g/mol Average: Difference between Calculated and Accepted values = 58.124g/mol - 56.57g/mol = 1.554g/mol CONCLUSION AND EVALUATIONS (CE) CONCLUDING - Determining the molar mass of butane through experimentation is possible with multiple trials. The more trials completed, the closer the average molar mass of butane is to the accepted value of the molar mass of butane. To determine the molar mass, take the mass of butane in the beaker and divide that by the number of moles of butane. ...read more.

Conclusion

Another systematic error that could have occurred is that the ambient room pressure was taken from a website dictating the pressure in the area, rather than directly in our room. The measurements in the lab are reliable taking into consideration the equipment windows of error and there are few to no flaws and weaknesses in the procedure itself. IMPROVING THE INVESTIGATION - The experiment could have been improved by measure the atmospheric pressure directly in the room, obtaining a more accurate room pressure to ensure that the pressure of butane was calculated correctly. Other improvements may include more accurate equipment such as a balance, beaker, and thermometer. Also, the butane used in the experiment could have been certified as pure butane, rather than butane from a common lighter. APPENDICES - "Cornellbiochem - Butane." Cornellbiochem - home. Web. 08 Nov. 2009. Brown, Theodore L., H. Eugene LeMay Jr., Bruce E. Bursten, and Catherine J. Murphy. Chemistry The Central Science; AP Edition. 10th ed. Upper Saddle River: Prentice Hall College Div, 2005. Print. ?? ?? ?? ?? 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related International Baccalaureate Chemistry essays

1. ## Molar Heat combustion chemistry - investigate the effect of molar mass on the molar ...

Error propagation accounts for all of these errors. Limitations and Improvements: Limitations The Effects on the experiment Improvements The distance between the flame and the aluminium can If the distance between the flame and aluminium can is further than usual, less energy will be transferred to the water and more will be lost the atmosphere and surroundings, and vice versa.

2. ## IB chemistry revision notes

Low Acid S Simple Covalent 8-atoms in a ring Insulator Low Acid Cl Simple Covalent Cl=Cl Insulator Low Acid Ar Mono-Atomic Mono-Atomic Insulator Lowest - BONDING Ionic Bonding * When are two elements likely to combine to form a Binary Compound which is ionic in nature?

1. ## Change of Potential Difference in Voltaic Cells Lab Report

Observe and record any change in colors of the solution or electrodes. 7. Detach the voltmeter and rinse the electrodes using distilled water. 8. Repeat these steps two more times to get more accurate results ** Repeat these steps using different concentrations of copper sulfate each time (0.4, 0.6,

2. ## Determining the Molar Mass of Volatile Liquid

89.9 x 100= 0.1 % Total uncertainty: 0.30% + 0.10% +0.1% = 0.50% Amount of volatile liquid = 1.14 x 10-2 � 0.50 % moles Calculation of the mass of the condensed gas: Mass of condensed gas= mass of flask with condensed vapor- mass of empty flask Mass of condensed

1. ## Experiment: Analysing molar mass of Aspirin

However, there are difference between the experimental molar mass of aspirin when using phenolphthalein and bromothymol blue as indicator. The obtained molar mass of aspirin when using phenolphthalein indicator is smaller than using bromothymol blue as indicator. The difference with the theoretical value is also less.

2. ## Chemistry thermo lab, Hess's Law.

Finally, the change in enthalpy: 1. 2. 3. Reaction 2: First, we have to calculate the ?T by subtracting the final temperature by initial temperature: 1. 2. Now we calculate the mass of the solution, assuming it has the density as water: 1.

1. ## Organic lab. Comparison of alkanes and alkenes

Part III ? Alcohols and Carboxylic acids 1. Oxidation of ethanol Substance Ethanol + potassium dichromate + dilute sulfuric acid Observations When first placed in the water bath the solution turns from orange-yellow to first a light green. The smell is quite alcoholic and strong, pungent.

2. ## The chemistry of atmospheric and water pollution.

Example of a CFC include: CCl3F (trichlorofluromethane). CFCs are synthetic in that they are produced from human activity. CFCs were developed to replace ammonia as a refrigerant in the 1930s. At the time, their properties were found to be ?safer? than the ammonia because they were much more stable. • Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to 