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AP Chemistry – Chapter 5 – Test. Mr. Richardson Sept 17, 2003 1. What is the cause of gas pressure? (1pt) 2. On the Kelvin scale, a temperature of 22 degrees Celsius has a value of what? (1pt) Name:_________________ Section #:_________ 7. In a closed container at 1.0 atmosphere, the temperature of a sample of gas is raised from 300 K to 400 K. What will be the final pressure of the gas? (3 pts) 3. Convert 120 K to ºC (1pt) 4. Define diffusion (1pt): 8. A sealed, inflexible container of oxygen gas has a volume of 2 liters. When the temperature of the gas is 300 K, the pressure in the container is 110 kPa. At what temperature will the pressure be cut in half? (3 pts) 5. Define Effusion (1pt): 6. At standard pressure, a sample of nitrogen occupies 500 mL. What volume does the gas occupy when the pressure doubles? (3 pts) 7. At a pressure of 5.0 atmospheres, a sample of gas occupies 40. liters. What volume will the same sample occupy at 1.0 atmosphere? (3 pts) 9. Organize the following gasses in order of their rates of diffusion, from slowest to fastest. (1 pt) Oxygen, O2 Ammonia, NH3 Hydrogen, H2 Carbon Dioxide, CO2 10. Which of the following gases would have the fastest rate of diffusion, assuming all of the gases are at the same temperature? (1 pt) Ne Ar Kr He N2 CO2 1 15. When ammonium nitrite undergoes decomposition, only gases are produced according to the equation: NH4NO2(s) N2(g) + 2H2O(g) 11. Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest? (3 pts) What is the total volume of gases produced at 819K and 1.00 atm pressure when 128 g of ammonium nitrite undergoes the above decomposition reaction? (3 pts) 12. A sealed flask contains 1 molecule of hydrogen for every 3 molecules of helium at 20 °C. If the total pressure is 400 kPa, what is the partial pressure of the hydrogen? (3 pts) 16. What is the pressure exerted by some nitrogen gas collected in a tube filled with water on a day when the room temperature is 18.0 °C and the room pressure is 750.0 mmHg? [The partial pressure of water at 18 °C is 15.5 mmHg.] (3 pts) 13. A mixture of gases, nitrogen, oxygen, and carbon dioxide at 27 C and 0.50 atmospheres pressure occupied a volume of 492 mL. How many moles of gas are there in this sample? (3 pts) 14. A mixture of gases at 810 kPa pressure contains: 3.0 moles of oxygen gas, 2.0 moles of helium gas, and 4.0 moles of carbon dioxide gas. 17. What is the partial pressure (in mm Hg) of neon in a 4.00 L vessel that contains 0.838 mol of methane, 0.184 mol of ethane, and 0.755 mol of neon at a total pressure of 928 mmHg? (3 pts) 18. What is the rms speed of methane molecules at 45.0 °C? (1 pt) What is the partial pressure of helium gas, PHe.? (3 pts) 2 19. A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 629 torr. Calculate the volume (L) the gas will occupy when the temperature is increased to 125.0 °C, while maintaining the pressure at 629 torr. (3pts) Bonus 1. A gas at 20 atm pressure with a volume of 2.0 Liters expands against a 5 atm pressure to a volume of 8.0 Liters. How much work is done by the gas 20. Calcium hydride (CaH2) reacts with water to form hydrogen gas: Bonus #2: In the presence of excess oxygen, methane gas burns in a constantpressure system to yield carbon dioxide and water: CaH2 (s) + 2H2O (l) → Ca(OH)2 (aq) + 2H2 (g) How many grams of are needed to generate 48.0 L of gas at a pressure of 0.888 atm and a temperature of 32 °C? (3pts) CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O(l) △H = -890 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure. 3