Name: Gas Laws Worksheet #1 - Boyle's, Charles’, Gay-Lussac's, and Combined Gas Law Solve all problems – you must show your work (including units). The correct answer is given in parentheses at the end of the problem. Boyle's Law 1. A gas sample contained in a cylinder equipped with a moveable piston occupied 300.0 mL. at a pressure of 2.00 atm. What would be the final pressure if the volume were increased to 500.0 mL at constant temperature? (1.20atm)

2. Pressure Conversions    a. Convert 0.650 atm to mm Hg.    b. Convert 710.0 torr to atm.3. Temperature Conversions    a. Convert 30.0 Celsius to Kelvin    b. Convert 25 Celsius to Kelvin4. Name 4 factors that affect the properties of gasesSolve the following using the gas equations. Temperature must always be converted to kelvin before using in any equation. In addition to Kelvin for the Ideal Gas Law, pressure must be in atmospheres, volume in Liters, and n in moles. The gas constant with units is R=0.08206 (L atm)/(n K).  Notice that the units of R dictate which units must be used for each parameter.  Mind the significant figures in your calculations.5. Boyle’s Law  -  Temperature constant   a. A sample of gas has a volume of 400.0 mL when measured at 25oC and 760.0 torr.       What volume will it occupy at 25oC and 195.0 torr?     b.  What final pressure must be applied to a sample of gas having a volume of         200.0 mL at 20.0 oC and 750.0 torr pressure to permit the…

7. The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two gases. a. What is the mole fraction of each gas in the mixture? b. If the mixture occupies a volume of 10.5 L at 65°C, calculate the total number of moles of gas in the mixture. C. Calculate the total mass of the mixture (hint, find the mass of each gas in the mixture). с. d. Calculate the relative rates of effusion for molecules of CH4 to that of a molecules of O2.

1. At 27°C and 720 Torr, a certain gas sample has a volume of 765 mL. a. What would be its new volume if the temperature and pressure were changed to 57°C and 792 Torr? Hint: Use Combined Gas Law. b. How many moles are present in that gas sample? Hint: Use Universal Gas Law.

A sample of hydrogen gas that occupies a volume of 31.9 L at a temperature of 0 °C and a pressure of 1 atm contains ___ moles of gas.

Which of the following should be done to reduce the pressure of 1 mole of an ideal gas in a 22.4 L container to zero torr? O Double the temperature of the gas. O Cool the gas to absolute zero. Halve the volume of the container. O Cool the gas to zero Celsius. Double the amount of gas.

A sample containing 4.70 gg of O2O2 gas has an initial volume of 11.0 LL . What is the final volume, in liters, when each of the following changes occurs in the quantity of the gas at constant pressure and temperature? A. A sample of 0.650 mole of O2O2 is added to the 4.70 gg of O2O2 in the container. B. A sample of 1.65 gg of O2O2 is removed from the 4.70 gg of O2O2 in the container. C.A sample of 4.80 gg of O2O2 is added to the 4.70 gg of O2O2 gas in the container.

13.  A barometer is used to measure the total pressure of a mixture of gases A, B, and C. The total pressure is measured to be 750 torr. Assume the partial pressure of gas A is 203 torr and the partial pressure of gas B is 167 torr. What is the pressure of gas C? Do not include units with your answer.

A sample of nitrogen gas that occupies a volume of 45.5 L at a temperature of 0 °C and a pressure of 1 atm contains ________ moles of gas.

Doubling the initial pressure, from 1.0 atm to 2.0 atm, while keeping the temperature constant causes the volume of a gas to go from 1000 mL to a final volume of