11. Atmospheric pollution such as SO₂ is a problem that has received a lot of attention. While humans contribute significantly to this pollution through fossil fuel combustion, there are some natural sources. For example, the Kilauea volcano in Hawaii emits 200-300 tonnes of SO2 per day. If this gas is emitted at 850°C and 1.0 atm, what volume of gas is emitted? Assume the gas behaves ideally,

11. Atmospheric pollution such as SO₂ is a problem that has received a lot of attention. While humans contribute significantly to this pollution through fossil fuel combustion, there are some natural sources. For example, the Kilauea volcano in Hawaii emits 200-300 tonnes of SO2 per day. If this gas is emitted at 850°C and 1.0 atm, what volume of gas is emitted? Assume the gas behaves ideally,

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

2. Calculate the pressure of a sample of gas collected over water at 25°C if the atmospheric pressure is 0.948 atm. 1 atm = 760 mm Hg.
A sample of N2N2 gas has a volume of 19.0 L at a pressure of 1.50 atm and a temperature of 23 ∘C. What volume, in liters, will the gas occupy at 3.50 atm and 231 ∘C? Assume ideal behavior.
A medical grade diatomic gas Z (1000 grams) behaves non-ideally and must be kept at a temperature of 22 °C. Given that only 75000 cm storage tanks are available, determine the maximum pressure allowed for storage. Assuming the gas behaved ideally, how would your answer differ? van der Waals constant for Z-a: 1.25 L atm mol?; b: 0.0318 L mol Atomic mass of Z= 17 g/mol
A 4.37 gram sample of a certain diatomic gas occupies a volume of 3.00 L at 1.00 atm and a temperature of 45°C. Identify this gas.
1. Ammonia gas is produced by the reaction: N2(g) + 3H2(g) → 2NH3 (g). (a) How many liters of ammonia can be produced from 10.8 L of hydrogen? Assume that all gases were measured at a constant temperature and pressure. (b) If the reaction was made to occur at 2 atm pressure at 254 K, how many moles of ammonia were produced?
What volume in mL of O2 gas collected over water is obtained from heating 852.7 mg KClO3 (122.55) at 25°C and 1 atm. Use the gas laws .
A sample of O2 gas has a volume of 15.0 L at a pressure of 1.50 atm and a temperature of 23 ∘C. What volume, in liters, will the gas occupy at 3.50 atm and 226 ∘C? Assume ideal behavior.
29. A 2.50-L volume of hydrogen measured at –196 °C is warmed to 100 °C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.
Gaseous CO exerts pressure of 45.6 mmHg in a 56.0 L tank at 22°C was released to a room with a volume of 2.70 x 104L. The room has another two gaseous that are 5.50 g of NO2 and 8.034 x 1022 atoms of SO2 at 22°C. Calculate the partial pressure of CO in the room at 22°C. •Ans : P = 0.09458 mmHg Calculate the total pressure in the room and the molarity of CO gas in the room. •Ans: 5.14 x 10-6 M, Total pressure 2,7 x 10-4 atm Calculate the density of the mixture in the room and the mass percentage of SO2 gas in the room. 6.00027
The stopcock connecting a 1.00 L bulb containing krypton gas at a pressure of 678 mm Hg, and a 1.00 L bulb containing carbon dioxide gas at a pressure of 664 mm Hg, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, what is the final pressure in the system? mm Hg
This relationship is known as Graham’s Law of Effusion. Since both gases are at the same temperature, they must have the same average kinetic energy (½ mv2), where m is mass and v is velocity (like speed). Since both gases have the same average kinetic energy, you can state that ½ mLvL2 = ½ mHvH2. Multiplying both sides by 2 gives you mLvL2 = mHvH2. Rearranging the equation to get both masses on the same side of the equation will give you mL/mH = VH2/VL2. In 3a and 3b, you probably noticed that the heavy gas particles took twice as long to diffuse as the light gas particles. This means that the light gas particles are moving twice as fast, VH/VL = ½. Therefore, VH2/VL2 = ¼. If the light gas was Ne, what would be a reasonable identity for the heavy gas? Explain.
19. A 2.00 liter of sample of ethane, C;H6, is burned at 1.00 atm and 25.0 °C with 1.50 liters of oxygen. What is the mass of water vapor will be produced from the burning of ethane? What would be the volume of the water vapor under the same conditions? (Hint: determine the limiting reagent!) (m = 1.96 g; v = 1.29 L.