# See table 1 attached p water mm hg note the gas

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(see Table 1 attached) P water mm Hg Note: The gas collected in the cylinder is a mixture of C 4 H 10 (g) and H 2 O (g) . Use Dalton’s Law of Partial Pressure to calculate the pressure of butane in the mixture. P total = P butane + P water vapor 10. Pressure of dry butane P butane mm Hg 11. Convert P butane from mm Hg into kPa using the unit factor method. SHOW your conversion below. = P butane kPa

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M o l e s 1. Calculate the number of moles of butane collected using R = 8.31 kPa · L / mol · K P= V= n = __________ R= Τ = PV = nRT n = 2. Calculate the experimental molar mass of butane by dividing the mass, M (line 3), by n, the number of moles. MM experimental = 3. Calculate the accepted value for the molar mass of butane using a periodic table. Butane C 4 H 10 MM accepted = 4. Calculate the ERROR (the difference between the accepted value and your experimental value). 5. Calculate the percentage error in your result. This is: x 100 % error Bonus QUESTIONS: 1. How many grams of butane did you collect in this experiment? 2. What volume would the same number of grams of ethane (C 2 H 6 ) have occupied at the same conditions of temperature and pressure?
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