11A: Gas Laws and the Molar Mass of Butane Data Sheet for Boyle's Law Name: Input your Volumes (mL) and Pressures (psi). Then complete the rest of the table, and make the graphs. a. Graph 1: V in mL (y-axis) vs. P in atm (x-axis) (You may use a French curve.) b. Graph 2: V in mL (y-axis) vs. 1/P in atm' (x-axis) (Use a ruler to draw the line of best fit.) V (ml) P (psi) P (atm) 1/P (1/atm or atm-¹) 65ml 60me 55 ml 50ml 45 m 40 me 35 mi 30 ml 25 mc 20 me 14.q 15.9 17.0 18.8 20.7 23.2 26.5 30.8 36.7 46.6 1.01 1.08 1.16 1.28 1.41 1.58 1.80 2.09 2.30 3.17 0.990 0.926 0.862 0.709 0.635 0.585 0.478 0.400 0.315 1. Convert each pressure in psi to a pressure in atm, round it to the correct number of digits, and record it in the data table. Note that 14.70 psi equals exactly 1 atm. Then take each pressure in atm and calculate 1 divided by that pressure. (Show one of each sample calculation here. Do the rest in your calculator only.) 2. What is the slope, m, of Graph 2? Show your calculations here, and include the correct units. What is the y-intercept, b, of Graph 2? Show your calculations here, and include the correct units.

7,8,9,10

m

Use the standard molar volume of a gas at STP (1mol/22.4L) to find how many moles of methane (CH4) are in a 3.55 X 105 L storage tank. How many grams of methane is this?

In Dalton's Law of Partial Pressures: Ptrapped gas = Pdry gas + Pwater vapor  Why must the pressure of water vapor be included in this calculation? a. The pressure exerted by the evolved H2(g) is reduced because of the co-presence of water vapor, thus Pwater vapor has to be added to Pdry gas. b. Some of the liquid water evaporates into the gas, and increases the total pressure generated by the trapped gas. c. As the H2(g) is bubbled up the reaction solution, some of the H2(g) molecules are solubilized by water in the aqueous solution, effectively decreasing the measured pressure above. d. The pressure contributed by the H2(g) is greater than the measured total pressure because of the contribution of partial pressure of water vapor.

If 0.211 g of gas occupies 204.5 mL at STP, what is the molecular weight of this gas? R = 0.08206 atm L / mole K

At 570 mm Hg and 25.0 celcius a gas sample has a volume of 2270 ML. What is the final pressure  (in mm Hg) at a volume of 1250 and a temp of 280 celsius?

A.) a mixture of argon and neon gases, in a 8.32 L flask at 21 degrees Celsius, contains 15.3 grams of argon and 2.24 grams of neon. The partial pressure of neon in the flask is ____atm and the total pressure in the flask is ____atm. B.) a mixture of helium and xenon gases is maintained in a 9.17 L flask at a pressure of 1.28 atm and a temperature of 84 degrees Celsius. If the gas mixture contains 0.637 grams of helium, the number of grams of xenon in the mixture is ____grams.

P2=_____atm

At 571  mm Hg and 323 K, a gas sample has a volume of 2.45 mL. What is the final pressure (in mm Hg) at a volume of 1.53 mL and temperature of 463 K?  (Report your answer to the nearest 1 mm Hg)