Question

Chemistry Lab Determination of the Universal Gas Constant (R)

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Given:

Initial mass of butane lighter: 54.24g

Final Mass of Butane Lighter: 54.01g

Temperature of water: 23.0°C

Volume of gas collected: 100.0mL

FIND:
Barometric pressure of room: 766.86 mmHg CONVERTED TO atm

Vapor pressure of water at room temperature(PH2O) (IN atm)

FIND:

Mass difference if butane lighter in grams

Moles of Butane gas collected in moles of C4H10

Partial pressure if butane gas in atm

Converted temperature of water in Kelvin

Converted volume of gas collected in Liters

Experimental value of R in Latm/molk

Accepted value of R in Latm/molk

Percent error in experimental value of R in %

CONCLUSION QUESTIONS:

1. List at least 3 factors that either did it could contribute to the percent error

2. Should the value of R go up or down if the gas had not been corrected for the partial pressure of water. Why?

3. How could this experiment be repeated to increase the accuracy, or in other words, decrease the percent error?


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Answer 1

To solve this problem, I'll need some additional information related to the molar mass of butane (C4H10). Please provide the molar mass of butane so that I can proceed with the calculations.