Two More Laws Worksheet - Max Study



The gas from an erupting volcano had the following composition: 65.0 % CO2 ( 494 mm Hg), 25.0 % H2 (190 mm Hg) 5.4 % HCl (41.0 mm Hg) 2.8 % HF (21.3 mm Hg), 1.7 % SO2 ( 12.9 mm Hg), and 0.1 % H2S (0.760 mm Hg). What are the partial pressures of each gas if the total pressure is 760.0 mm of Hg?

1. A container of gases consists of the following mixture of gases: 2.0 moles of helium (60. mm Hg), 6.0 moles of carbon dioxide (180 mm Hg), 10.0 moles of neon (300. mm Hg), and 12.0 moles of xenon (360 mm Hg). If the total pressure is 900.0 mm of Hg, determine the partial pressure of each gas.

2. A sealed tank contains the following mixture of gases: 2.0 grams of helium (50. kPa), 48.0 grams of oxygen (150 kPa), 14.0 grams of nitrogen (50. kPa), 64.0 grams of sulfur (IV) oxide (100. kPa), and 9.0 grams of hydrogen gas (450 kPa). If the total pressure is 800.0 kPa, then find the partial pressure of each gas.

3. Nitrogen is collected over water at 21.5(C. What is the partial pressure of nitrogen if the atmospheric pressure is 99.4 kPa? (96.8 kPa)

4. Argon is collected over water at 30(C. Find the pressure of the dry gas if the barometric pressure is 0.975 atm. (0.933 atm)

6. 223 mL of H2 was collected over water on a day when the atmospheric pressure was 762 mm Hg. The temperature of the water was 19oC. How many molecules of hydrogen were collected? (5.49 x 1021 molecules)

7. Xenon Hexafluoride decomposes into its elements. All of the substances in the reaction are gases.

o Write a balanced equation for this reaction. XeF6 (g) ( Xe(g) + 3F2(g)

o 252.1 ml of the products are collected over water at 18oC and 2.045 atm. Find the partial pressure of each dry gas. PXe = 0.506 atm PF2 = 1.518 atm

8. Each of the four tires of Mr. B's “ride” is filled with a different gas, to a tire gauge of 2.0 atm at 25 C. The mass of the gas for each of the tires is as follows: Tire 1: Air (80.0 % N2 and 20.0 % O2), = 116.0 grams; Tire 2: Neon = 80.7 grams; Tire 2: Helium = 16.0 grams; and Tire 4: an unknown gas = 160.0 grams. The barometric pressure is 1.0 atm.

a) Which tire contains the largest number of molecules/atoms?

ALL THE SAME NUMBER OF PARTICLES (ATOMS OR MOLECULES)

b) What is the molar mass of the unknown gas? 40 g/mol

c) What is the name of the unknown gas? argon

d) The neon and helium filled tires are punctured with equal size pinholes. If the helium-filled tire goes flat in 4.0 hours, how long would it take for the neon-filled tire to go flat?

9.12 hours

e) What is the partial pressure of N2 in the air filled tire? (1.6 atm)

f) Which tire contains molecules/atoms having the greatest kinetic energy?

All the same KE (same T)

g) In each tire, should the pressure be increased or decreased to make the gas behave more ideally at the same temperature?

Decrease pressure to idealize behavior.

h) What is the volume of each of the tires under the given conditions? (48.9 L)

i) Which tire's contents would most closely approximate the behavior of an ideal gas? Why?

He least IMF and smallest size, therefore occupying least volume.

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download