Gas Homework - 14 SB

Name: Gas Homework Objective 15.1 Complete Chemistry End of Chapter Exercises 1,2,3 and 6 in Chapter 8.5 The Kinetic Molecular Theory Each Gas Law has a few problems to practice. For “completion” of this homework do ½ of each type of problem Objective 15.2 Boyles Law Problems: 1. A gas OF 2 occupies a volume of 458 mL at a pressure of 1.01 kPa and temperature of 295 K. When the pressure is changed, the volume becomes 477 mL. If there has been no change in temperature, what is the new pressure? 2. Dinitrogen monoxide gas occupies a volume of 2.45 L at a pressure of 1.03 atm and a temperature of 293 K. What volume will the gas occupy if the pressure changes to 0.980 atm and the temperature remains unchanged? 3. The cylinder of a car’s engine has a volume of 0.6250 L when the piston is at the bottom of the cylinder. When the piston is at the top of the cylinder the volume is 0.0600 L. If the cylinder is filled with air at an atmospheric pressure of 765.1 mmHg when the piston is at the bottom, what is the pressure when the piston is at the top of the cylinder? 4. A discarded spray paint can contains only a small volume of the propellant gas dinitrogen tetroxide at a pressure of 34,470 Pa. The volume of the can is 473.18 mL. If the can is run over by the garbage truck and flattened to a volume of 13.16 mL, what is the pressure in Pa assuming the can doesn’t leak. 5. A sample of 10.0 L of argon gas is stored in a cylinder at a room temperature of 23.8°C and a pressure of 78.6 lb/in 2 . The sample is transferred completely to another 2.8 L cylinder. Several hours after the transfer, the second cylinder has also attained room temperature. What is the pressure in the second cylinder. Charles Law Problems: 1. A tank of compressed CO 2 has a temperature of 23.6°C and a volume of 31.4 L. The CO 2 is completely transferred into a smaller tank that has a volume of 25.0L. Assuming none of the CO 2 escapes during the transfer, what is the temperature of the CO 2 in the smaller tank if the temperature is lowered to achieve the same pressure as in the larger tank? 2. A mercury barometer at a room temperature of 22.4°C has a volume of 10.6 mL between the sealed end of the tube and the mercury. The sun rises and shines through a window on the barometer and warms it to 27.8 °C. If the atmospheric pressure remains constant, what is the new volume between the sealed end of the tube and the mercury? 1 0114914,58mL 0.9701hPa 1.8 730.052 765.187 9 162501 7968.75 mmHg 341470 pax 473.18 mL 13 16 123 855Pa 78.6 6.8951hPa 10L 2 8 LX Pz 19.35 5251hPa hx 8.314 23.6 C 10.624,139ft 10.18mL

Name: 3. What will be the volume of a C 2 O gas sample at 309 K if its volume at 215 K is 3.42 L? Assume that the pressure is constant. 4. A gas chlorine trifluoride sample at 83°C occupies a volume of 1400 m 3 . At what temperature will it occupy 1200 m 3 . 5. At 75°C, a NF 3 gas has a volume of 3.22 dm 3 . What volume will it occupy at 75K? Amonton’s Law Problems 1. A sample of hydrogen at 47°C exerts a pressure of 0.329 atm. The gas is heated to 77°C at constant volume. What will its new pressure be? 2. To what temperature must a sample of nitrogen at 27°C and 0.625 atm be taken so that its pressure becomes 1.125 atm at constant volume? 3. The pressure on a P 4 S 3 gas which is 340 mmHg at -73°C is doubled, but its volume is held constant. What will the final temperature be in degrees Celsius? 4. At 84°C, a dinitrogen pentoxide gas in a container exerts a pressure of 0.503 atm. Assuming the size of the container has not changed, at what Celsius temperature would the pressure be 1.20 atm Combined Gas Law Problems: 1. If I initially have a NO gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200K, and then I raise the pressure to 14 atm and increase the temperature to 300K, what is the new volume of the gas? 2. Dichlorine monoxide gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299K. If the temperature rises to 350 K and the pressure lowers to 1.5 atm, what is the new volume of the gas? 3. IF 5 gas that has a volume of 28 liters, a temperature of 45°C, and an unknown pressure has its volume increased to 34 liters and its temperature decreased to 35°C. If I measure the pressure after the change to be 2.0 atm, what was the original pressure of the gas? 4. Dichlorine heptoxide gas has a temperature of 14°C , and a volume of 4.5 liters giving a pressure of 690 mmHg. If the pressure is adjusted to normal pressure and the volume raised to 10. 3L what is the new temperature of the gas? V2 3.422 30914 2151h 4.91L Claim 1400m 6.0821 atm.ms mol.in 356.154 46.74 0.0821 71 5 273.15 1.65 C V1 Ff 0.694dm 0.329 350.15 320.15 0.359 atm 1 125am300 1519 0.625atm 54019 680 mmHg 1340 mmHg x 73 223.151 546.319 273.15 273.15 C 1.20 0503 357.1514 857.7114 584.71 C 143 1 4 99 49.29 liters 14,8214 35015 25.62 2.0 34 318.15 28 308.15 3.08 atm 1 23m01 6.082057C atm molla 287 15141 696 mmHg 10.34 293.1519

Name: Gas Stoichiometry (if conditions are not mentioned – assume STP) 1. Find the mass of benzene required to produce 2.66L of carbon dioxide gas at STP from the reaction described by the following equation: 2C 6 H 6 + 15 O 2 → 6H 2 O + 12 CO 2 2. What volume of SO 3 is produced from the reaction of 12.4L of SO 2 and 3.45 L of O 2 from the following equation: 2SO 2 + O 2 → 2SO 3 3. Determine the percent yield for the reaction between 15.8g of NH 3 and excess oxygen to produce 18.1L of NO gas from the following reaction: 4NH 3 + 5O 2 → 4NO + 6H 2 O 4. If 4.1 g of Cr is heated with 9.3L of Cl 2 gas, what mass of CrCl 3 will be produced from the following equation: 2Cr + 3Cl 2 → 2CrCl 3 (name CrCl 3 ) 5. Find the mass of sodium required to produce 5.68L of hydrogen gas at STP from the reaction described by the following equation: 2Na + 2H 2 O → 2NaOH + H 2 6. Determine the percent yield for the reaction between 46.5g of ZnS and 13.3g of oxygen if 5.4L of sulfur dioxide is recovered. 2ZnS + 3O 2 → 2 ZnO + 2SO 2 7. What mass of NaCl will be produced by the reaction of 188.7g of NaI with 29.4L of Cl 2 gas: 2NaI + Cl 2 → 2NaCl + I 2 if the temperature of the reaction is at 25.0°C and a pressure of 0.992 atm 8. How many liters of oxygen are necessary from the combustion of 134g of magnesium: 2Mg + O 2 → 2MgO if the temperature of the reaction is at 100°C and a pressure of 820 mmHg 9. Determine the percent yield for the reaction between 28.1g of Sb 4 O 6 and excess C if 3.56L of CO are recovered: Sb 4 O 6 + 6C → 4Sb + 6 CO if the temperature of the reaction is at 72°C and a pressure of 690 mmHg Objective 15.4 Dalton’s Law Problems 1. Three of the primary components of air are carbon dioxide, nitrogen, and oxygen. In a sample containing a mixture of only these three gasses at exactly one atmosphere pressure, the partial pressures of carbon dioxide and nitrogen are given as P CO2 = 0.285 mmHg, P N2 = 593.525 mmHg. What is the partial pressure of oxygen? 0.019792 78.11g mol 1.547g 2 22.42 44.82 2 3.45 6.90L 18.12 20.77 100 87 51.996 35.453 3 158.33 0.079 12.529 1 0.2536 0.1268 22.99 2.91g 5 42 199g L 10.746g 10.746g 17.94g 100 59.9 22.99 gimo Na 35.45 91m01 8.44g mol x 1.23 moles 71.89g 31.998 moles 0 08206 L atm moic 100 C 26.19L 760 10.285 569 523 190.2 mmHg

Name: 2. Determine the partial pressure of oxygen collected by water displacement if the water temperature is 20.0°C and the total pressure of the gases in the collection bottle is 730.0 mmHg. (to find water vapor pressure use book table on pg 199 or internet ( http://antoine.frostburg.edu/chem/senese/101/toolbox.shtml ) use water properties calculator 3. A sample of gas of dinitrogen monoxide is collected over water at a temperature of 35.0°C when the barometric pressure reading is 742.0 mmHg. a. What is the partial pressure of the dry gas? b. Write the chemical formula 4. A mixture of three gases, A, B, and C, is at a total pressure of 6.11 atm. The partial pressure of gas A is 1.69 atm; that of gas B is 3.89 atm. What is the partial pressure of gas C? Objective 15.5 Complete Chemistry End of Chapter Exercises 2 and 5 in Chapter 8.4 Effusion and Diffusion of gases 1. A sample of N 2 diffuses 20.8 cm in 5.0 minutes. Would a sample of Kr(g) diffuse more or less in the same amount of time under the same conditions? Explain 2. A sample of helium gas diffuses 15.0 cm in 3.0 minutes. Would it take a sample of Cl 2 gas to diffuse the same distances the same amount of time? Explain 3. A 3.2x10 -3 mole sample of oxygen gas effuses from a container in 10.0 minutes. Would the same amount of CH 4 gas effuse in that time under the same conditions? Explain 1018.07131 13.426 17.54 730.0 712.46 mmHg I 5422 mmHg 699.8 mmHg NO T1 bill 6.11 atm 1.69atm 3.89 at m A 1.69 0.53 atm 13 3.89 1. Di ff usion of N2 vs Kr(g) To determine whether a sample of Kr(g) would di ff use more or less than N2 in the same amount of time under the same conditions, we can compare their molar masses. The rate of di ff usion is inversely proportional to the square root of the molar mass of the gas. Since Kr has a higher molar mass than N2, it would di ff use less in the same amount of time under the same conditions. 2. Di ff usion of He vs Cl2 Helium gas di ff uses 15.0 cm in 3.0 minutes. To determine if it would take a sample of Cl2 gas to di ff use the same distance in the same amount of time, we compare their molar masses. The rate of di ff usion is inversely proportional to the square root of the molar mass of the gas. Since Cl2 has a higher molar mass than He, it would di ff use less in the same amount of time under the same conditions. 3. E ff usion of O2 vs CH4 A 3.2x10-3 mole sample of oxygen gas e ff uses from a container in 10.0 minutes. To determine if the same amount of CH4 gas would e ff use in that time under the same conditions, we compare their molar masses. The rate of e ff usion is inversely proportional to the square root of the molar mass of the gas. Since CH4 has a higher molar mass than O2, it would e ff use less in the same amount of time under the same conditions.

Name: desired volume of the balloon is 1.250L, what must the temperature be in °C?