Lab Exercise 9-CEM131 Determining the Molar Mass of Butane Name Melissa Wagner Data Table Mass of butane lighter before

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Lab Exercise 9-CEM131 Determining the Molar Mass of Butane Name Melissa Wagner Data Table Mass of butane lighter before release of gas (a) Mass of dried butane lighter after release of (al Volume of Gas (m) Water Temperature (°C) Barometric Pressure (mm) 2 Vapor Pressure of water (mit almopher MG2 Trial 1 21.47 21.54 Calculate the molar mass of butane Convert the water temperature from Celsius to Kin Using Daton's Law of Partial Pressures and the fact that the butane gas was cer partial pressure of butane gas in the cylinder 7 molar mass given please prit Score Calculate the average molar mass of butane Trial 2 0.20 29°C 762 30.0mming 28.4mmit 26.4 By using the ideal Gas Law, calculate the moles of butane in t ander Calculate the percent error between your experimentally-d 21.57 21.35 0.22 28% 21.35 21.12 B Your percent error is likely pretty high, why do you think that is? Whered experiment? How could you improve your data? 0.23 a4°℃ late the eference
Data Table Mass of butane lighter before release of gas (g) Mass of dried butane lighter after release of gas (g) Volume of Gas (ml) Water Temperature (°C) Barometric Pressure (mmHg) Vapor Pressure of water (mmHg) atmospheric 462 mmHg Pressure Vapor Pressure of Water Temperature (°C) Vapor Pressure (mmHg) 17.5 18.7 19.8 21.1 22.4 23.8 25.2 20 21 22 23 24 25 26 27 28 29 30 31 100 Calculations 26.7. 28.4- 30.0* 31.5 33.7 760 Trial 1 21.47 21.54 0.20 29°C 762 Trial 2 21.57 21.35 0.22 28°C Trial 3 21.35 21.12 0.23 24°C 762 767 30.0mmHg 28.4 mmHg 26.4 Show all calculations for one set. Include all units. Round all calculated values to the allowed significant figures. Box numerical answers. Show all three trials, until question 6. Calculate the mass of hutane gas used.
2 5. Using Dalton's Law of Partial Pressures and the fact that the butane gas was collected over water, calculate the partial pressure of butane gas in the cylinder Convert the water temperature from Celsusto evi By using the Ideal Gas Law, calculate the moles & Calculate the molar mass of butane Calculate the average molar mass of butane cylinder 7. Calculate the percent error between your experimentally-determined average molar mass and the referer molar mass given. Your percent emor is likely pretty high, why do you think that is? Where do you think the error enterst experiment? How could you improve your data?
Mass of butane lighter before release of gas (g) Mass of dried butane lighter after release of gas (g) Volume of Gas (ml) Water Temperature (°C) Barometric Pressure (mmHg) Vapor Pressure of water (mmHg) atmospheric 462 mmitg Pressure Vapor Pressure of Water Temperature (°C) Vapor Pressure (mmHg) 17.5 18.7 19.8 21.1 22.4 23.8 25.2 26.7. 28.4- 30.0* 31.5 33.7 760 20 21 22 23 24 25 26 27 28 29 30 31 100 Calculations Trial 1 21.47 21.54 29°C 462 Trial 2 21.57 21.35 28°C 462 30.0mmHg 28.4 mmHg Trial 3 21.35 21.12 24°C 767 26:4 how all calculations for one set. Include all units. Round all calculated values to the allowed significant figures. B umerical answers. Show all three trials, until question 6.
S N 2₁ montre Using Dalton's Law of Partial Pressures and the fact that the butane gas was collected ove partial pressure of butane gas in the cylinder.