Gas Law Worksheet



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Gas Law Worksheet
Name: ________KEY_________


  1. In general, as temperature increases, volume will _____INCREASE_____.




  • This is _____CHARLES’_____ Law. It has a _____DIRECT_____ relationship.



  1. In general, as pressure increases, temperature will _____INCREASE_____.




  • This is _____GAY – LUSSACS_____ Law. It has a _____DIRECT_____ relationship.



  1. In general, as pressure increases, volume will _____DECREASE_____.




  • This is _____BOYLE’S_____ Law. It has a _____INDIRECT_____ relationship.



  1. True or False—The pressure in my car tires is greater at noon than at midnight.

THE TEMPERATURE IS HIGHER AT NOON CAUSING THE PARTICLES TO MOVE FASTER AND COLLIDE MORE OFTEN


  1. True or False—Gas molecules have no volume or mass.

IDEAL GASES DO NOT HAVE VOLUME OR MASS, BUT REAL GASES DO. (EX: DEFLATED BALL < INFLATED BALL)


  1. You got balloons for your birthday and don’t want them to lose their helium. You decide to put them in the freezer for safekeeping. What will they look like the next morning when you take them out? Why?

WHEN THE TEMPERATURE DROPS, THE PARTICLES WILL NOT MOVE AS FAST. THIS WILL CAUSE THE VOLUME

TO DECREASE AND THE BALLOONS WILL SHRINK.



  1. Say you have an accident on the way home and let go of your balloons. Will they float up forever into space, will they eventually pop, or deflate? Why?


AS THE BALLOON RISES, THERE WILL BE LESS PRESSURE BECAUSE THERE ARE FEWER PARTICLES AT HIGHER

ELEVATIONS. SINCE THE PARTICLES WILL NOT BE PRESSING AGAINST THE SIDE AS MUCH, THE BALLOON WOULD

EVENTUALLY POP.


  1. Why do they have to pressurize the cabin in airplanes?


THE HIGHER UP YOU GO, THE LOWER THE AIR PRESSURE. THERE ARE FEWER MOLECULES OF AIR WHICH MAKES THE AIR PRESSURE LOW AND VERY LITTLE OXYGEN TO BREATH. IF YOU WERE TO GO HIGH ENOUGH, YOU

WOULD DIE FROM LACK OF OXYGEN. THIS WOULD OCCUR BEFORE YOUR LUNGS WOULD EXPLOAD AS THEIR



VOLUME INCREASES AS THE PRESSURE DECREASED.


  1. A bubble forms at the bottom of a lake. As it rises to the surface (but before it gets there), will it grow, shrink, or pop? Why?

AS THE BUBBLE HEADS TO THE SURFACE THE PRESSURE AROUND IT WOULD DECREASE. SINCE THERE WOULD BE

LESS COLLISIONS ON THE EXTERIOR OF THE BUBBLE, ITS VOLUME WOULD EXPAND. DEPENDING HOW FAR

DOWN IT WAS AND IF IT MAKES CONTACT, THE BUBBLE MAY EVENTUALLY POP.

Math Calculations – from the 3 Gas Laws


  1. A gas thermometer measures temperature by measuring the pressure of a gas inside the fixed volume container. A thermometer reads a pressure of 2.45 atm at 0 ˚C  (273 K). What is the temperature when the thermometer reads a pressure of 3.41 atm?


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  1. Calcium carbonate decomposes at 1200° C to form carbon dioxide and calcium oxide. If 25 liters of carbon dioxide are collected at 1200° C  (1473 K), what will the volume of this gas be after it cools to 25° C  (298 K)?

___________________________





  1. I have added 15 L of air to a balloon at sea level (1.0 atm). If I take the balloon with me to Denver, where the air pressure is 0.85 atm, what will the new volume of the balloon be?

___________________________




  1. If I have 45 liters of helium in a balloon at 25° C  (298 K) and increase the temperature of the balloon to 55° C  (328 K), what will the new volume of the balloon be?

___________________________




  1. If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?

___________________________




  1. The temperature of a sample of gas in a steel tank at .29 atm is increased from -100.0˚C  (173 K) to 25.0 ˚C  (298 K). What is the final pressure inside the tank?


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Combined Gas Law Calculations


  1. A gas occupied .355 L at a pressure of 1.98 atm and a temperature of 22 oC  (295 K). The pressure increases to 2.95 atm and the temperature drops to 15 oC  (288 K). What is the new volume?

___________________________




  1. A sample of nitrogen gas occupies a volume of 2.00 L at .99 atm and 0.00° C  (273 K). The volume increases to 4.00 L and the temperature decreases to -136 oC  (137 K). What is the final pressure exerted on the gas?






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