Ideal Gas Law Practice
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- Camilla Gibbs
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1 Ideal Gas Law Practice Directions: Show all of your work for each problem below and put a BOX around your final answer for each problem. Obey all significant figure rules during this assignment. You must complete at least 15 of the problems below. Any additional problems that you choose to complete will be counted for extra credit. Remember to make a list of all of your variables before trying to do any math. You will need a calculator, pink reference sheet, yellow equation sheet, and periodic table to complete the problems. You may also find your Ideal Gas Notes from yesterday to be helpful. Reminders: Temperature must ALWAYS be in Kelvin (K) Volume must ALWAYS be in Liters (L) Pressure may have any units, but the units for R must have matching pressure units When using the Combined Gas Law equation, you may eliminate any variable that does not change 1) A student collects 425 ml of oxygen at a temperature of 24 o C and a pressure of atm. How many moles of oxygen did she collect? 2) What is the volume of 1.5 moles of an ideal gas at 25 o C and a pressure of kpa? 3) If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 201 K, and then I raise the pressure to 14 atm and increase the temperature to 301 K, what is the new volume of the gas?
2 4) What pressure, in atm, will 1,360 g of N2O gas exert on its container with a volume of 25.0 L if stored in a shed whose temperature reaches 59 o C in the summer? 5) A tank with a volume of 658 ml contains 1.50 g of Ne gas at a pressure of 450 kpa. What is the temperature of the gas in o C? 6) Container A (with volume 1.23 L) contains a gas under 3.24 atm of pressure. Container B (with volume 0.93 L) contains a gas under 2.82 atm of pressure. Container C (with volume 1.42 L) contains a gas under 1.21 atm of pressure. If all of these gases are put into Container D (with volume 1.51 L), what is the total pressure in Container D? Hint: Use the combined gas law first to determine the partial pressure of each gas in Container D (change in volume). 7) A gas takes up a volume of 17 liters, has a pressure of 2.3 atm, and a temperature of 299 K. If I raise the temperature to 351 K and lower the pressure to 1.5 atm, what is the new volume of the gas?
3 8) I have an unknown volume of gas held at a temperature of 115 K in a container with a pressure of 60.0 atm. If increasing the temperature to 225 K and decreasing the pressure to 30.0 atm causes the volume of the gas to be 29 liters, how many liters of gas did I start with? 9) A tank contains 115 moles of neon gas. It has a pressure of 57 atm at a temperature of 45 o C. Calculate the volume of the tank. 10) A scuba tank has a pressure of 195 atm at a temperature of 10 o C. The volume of the tank is 350 L. How many moles of air are in the tank? 11) A gas that has a volume of 28 liters, a temperature of 45 o C, and an unknown pressure has its volume increased to 34 liters and its temperature decreased to 35 o C. If I measure the pressure after the change to be 2.0 atm, what was the original pressure of the gas? 12) A helium-filled balloon has a volume of 208 L and it contains 9.95 moles of gas. If the pressure of the balloon is 1.26 atm, determine the temperature in Celcius degrees.
4 13) A tank of oxygen has a volume of 1650 L. The temperature of the gas inside is 35 o C. If there are 9,750 moles of oxygen in the tank, what is the pressure in atm? 14) Container A (with volume 1.56 L) contains a gas under kpa of pressure. Container B has 1/3 the volume of Container A, but its gas is under twice the pressure as that of Container A. If the gases from A and B are combined into Container C (with volume 0.95 L), what is the pressure in Container C? Hint: Use the combined gas law first to determine the partial pressure of each gas in Container C (change in volume). 15) A gas has a temperature of 14 o C and a volume of 4.5 liters. If the temperature is raised to 29 o C and the pressure is not changed, what is the new volume of the gas? 16) A canister of acetylene has a volume of 42 L. The temperature of the acetylene is 305 K and the pressure is 780 torr. Determine the amount (moles) of gas in the canister.
5 17) If I have 2.9 L of gas at a pressure of 5.0 atm and a temperature of 50 o C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4 L and decrease the pressure to 3.0 atm? 18) Calculate the volume of a CO2 cartridge that has a pressure of 57 atm at a temperature of 21 o C. The cartridge contains mol of CO2. 19) Container A (with volume 150 ml) contains a gas under an unknown pressure. Container B (with volume 250 ml) contains a gas under 628 mm Hg of pressure. Container C (with volume 350 ml) contains a gas under 437 mm Hg of pressure. If all of these gases are put into container D (with volume 300 ml), giving it 1439 mm Hg of pressure, find the original pressure of the gas in Container A. Hint: Use the combined gas law first to determine the partial pressure of each gas in Container D (change in volume).
6 20) A tank contains 2,500 L of argon gas. The pressure is 13,790 kpa and the temperature is 25 o C. How many moles of argon are in the tank? 21) If I have 17 liters of gas at a temperature of 67 o C and a pressure of atm, what will be the pressure of the gas if I raise the temperature to 94 o C and decrease the volume to 12 liters? 22) If I have 21 liters of gas held at a pressure of 78 atm and a temperature of 901 K, what will be the volume of the gas if I decrease the pressure to 45 atm and decrease the temperature to 750 K? 23) I have an unknown volume of gas at a pressure of 0.50 atm and a temperature of 325 K. If I raise the pressure to 1.2 atm, decrease the temperature to 320 K, and measure the final volume to be 48 liters, what was the initial volume of the gas?
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