# PLEASE ANSWER ABY OF THESE YOU KNOW. Thank you!!! 1. Explain why increasing the volume of a container decreases the pressure of the gas in the container, assuming the temperature remains fixed. 2.Container A and container B have the same volume. Container A holds twice as many moles of gas as container B. In which container is the pressure probably highest? Explain your answer. 3.Explain why gases can be compressed but solids and liquids cannot. 4.Given that PV=k, if k=2.0 L⋅atm for a 4.0 L container of gas, what is the pressure of the gas? 5.A 3.0 L container holds a sample of oxygen gas at 1.5 atm pressure. If the pressure increases to 2.0 atm and the temperature remains constant, what is the new volume of the container? 6.Use the kinetic theory of gases to explain Boyle’s law. Your answer 7.The pressure inside a typical 11.0 L scuba tank is about 204 atm at room temperature. How many 2.0 L soda bottles would be required to hold all the air in a scuba tank if you filled each bottle to 1.0 atm pressure at the same temperature? 8.A sample of a gas has a volume of 1.5 L at 150 K. If the gas is heated to 235 K at constant pressure, what will its final volume be? 9.The temperature of a gas rose from 250 K to 350 K. At 350 K, the volume of the gas was 3.0 L. If the pressure did not change, what was the initial volume of the gas? 10.The temperature of a gas is decreased by a factor of two at constant pressure. Does the gas expand or shrink? Answer without doing any calculations. Explain your answer. Your answer 11.A sample of a gas takes up 2.35 L of space at room temperature ( 20.0°C). What volume will the gas occupy at −5.00°C? (Hint: Don’t forget to convert the temperatures to kelvins.) 12.The gas inside a rigid container has a pressure of 0.50 atm at 273 K. The pressure of the gas increases to 1.0 atm. What is the final temperature of the gas? 13.Gay-Lussac’s law can be expressed by the equation P=kT. If a gas has a temperature of 273 K at 1.0 atm, what are the value and units of the constant k in this equation? 14.Use the kinetic theory of gases to explain Gay-Lussac’s law. 15.The pressure of a gas enclosed in a rigid container quadruples. By what factor does its temperature change? Explain your answer. Your answer 16.At 273 K, 1.5 mol N2 gas fills a 2.5 L container to a pressure of 13.4 atm. What will the pressure inside the container be if the temperature increases to 355 K and the container shrinks to a volume of 2.3 L? 17.A bacterial culture isolated from sewage produces 0.376 L of methane ( CH4) at 304 K and 1.5 atm. What would the volume of the methane be at STP? 18.The maximum safe pressure that a 4.00 L vessel can hold is 3.50 atm. If the vessel contains 0.410 mol of helium, what is the maximum temperature to which the vessel can be subjected? 19.A 34.5 L container holds 25.6 mol O2 gas at 321 K. By how much would the pressure change if the temperature decreased to 285 K and 4.5 mol O2 were added to the container? (Hint: Calculate the initial pressure inside the container first.)

1. Pressure decreases with increasing volume as the increased volume increases space for molecules to move around, thus decreasing the collisions and decreasing pressure. 2. A has a higher pressure given that the higher the n value, or moles present, the higher the pressure will be if everything else is held constant. 3. Gases have weaker intermolecular forces than liquids and solids. 4. Pressure must be 1/2, or 0.5 as PV=k, (P)(4)=(2), (P)=(2/4) 5. 2.25 L 6. Increasing space will decrease collisions and vice versa 7. 1122 2L bottles 8. 2.35 L 9. 2.1428 L 10. It would expand as they are directly proportional 11. 2.14959 L 12. 546K 13. .003663 atm`K 14. If pressure and temperature are directly proportional, then they increase or decrease at a constant rate 15. quadruples as they are directly proportional 16. 18.9963587 atm Sorry hun, I gotta go. Good luck!