University:
High School
Course:
High School Chemistry
Academic year:

2022
Views:

416

Pages:

2
Author:

Amel S.

Name:_______________________ Per:___ Ideal Gas Law Problems I. Ideal Gas Law Concepts 1. a. Under what conditions of pressure and temperature do “ideal” gases behave like “real” gases? Why? b. Which type of gas (ideal or real) is most commonly observed in nature & why? 2. Compare the behavior of ideal gases to real gases in the following table: Ideal Gases (Kinetic Molecular Theory)  Molecules are far apart. Real Gases     Collisions between molecules are elastic.   Molecules move continuously in rapid, random motion.  Molecules are attracted to each other (strong intermolecular attraction). 3. Determine the # of molecules, volume, & mass of each of the following samples of gas at STP? Description # of Molecules Mass Volume a. 2 mole of O2 gas @ STP 4. b. 2 moles of CO2 gas @ STP c. 1 mole of O2 gas @ STP d. 1 moles of CO2 gas @ STP e. 0.5 mole of O2 gas @ STP f. 0.5 mole of CO2 gas @ STP Based on your calculations above, does the size (mass) of the molecule affect its volume? Explain! 5. What size (volume) container would be 3.01 x 1023 molecules of N2 gas occupy at STP? II. Use the Ideal Gas Law (PV = nRT) to solve these problems. Show: a) the value of each variable b) the re-arranged formula and c) work to solve for the unknown. 1. How many moles are contained in 5.60L Cl 2 at STP? (Ans: .250 mol) P= V= n= R= T= 2. Find the volume, in Liters, of 1.25 moles of CO at STP. (Ans: 28.0L) P= V= n= R= T= 3. Determine the number of moles of a gas contained in 1.25L at 250K and 1.06atm. (Ans: .0646 mol) P= V= n= R= T= 4. Calculate the volume, in Liters, occupied by 4.00 g of O2 at 57°C and .888 atm.(Ans: 3.81L) P= V= n= R= T= 5. What pressure will be exerted by 25.1 g of CO2 at a temperature of 25 °C and a volume of 0.5L? P= V= n= R= T= 6. For an unknown quantity of gas at a pressure of 1.2 atm, a volume of 31 liters, and a temperature of 87°C, how many molecules of gas are in the container? P= V= n= R= T= 7. Using the equation PV=nRT, calculate the value of “R” for 1 mole of N2 gas at STP & volume. III. Use the Ideal Gas Law OR Combined Gas Law to solve these problems. Show: Formula & work 1. What would the volume in mL be of an ideal gas, if a 0.85 mole sample had temperature of 21.49K at a pressure of 1.26atm ? 2. At standard temperature, a gas has a volume of 275mL in a flexible container. When the absolute temperature (in Kelvin) is doubled, what is the new volume if the pressure is held constant? 3. If a gas has an initial pressure of .75 atm is allowed to expand to 435mL at .48atm, what was the initial volume? 4. How many grams of oxygen (O2 ) will occupy a volume of 2.5 liters at 1.2 atm and 25 °C? 5. My car has an internal volume of 2600 liters. If the sun heats my car from a temperature of 200 C to a temperature of 550 C. Assume volume in the car stays constant. a. What will the pressure inside my car be? Assume the pressure was initially 760 mm Hg. b. How many molecules of gas are in the car after it’s been heated?