8.1 Properties of Gases

8.1 Properties of Gases

• The atmosphere is a sea of gases.

• The behavior of gases is different than that of liquids.
• A gas has no shape or volume and will fill any container.

• The gas fills the entire volume of the container when it moves in random directions.

• The small forces between the particles of a gas are attractive.
• There are particles that are far apart and can fill a container of any size and shape.

• The volume of the gas is the same as the volume of the container.
• Gases can be easily compressed because most of the volume is empty.

• Gas particles are moving quickly.
• When gas particles collide, they travel in new directions.

• The gas completely walls of the container exert pressure.
• An increase in the number of col fills a container of any size and lisions against the walls of the container causes an increase in the pressure of the gas.

• As the temperature increases, gas particles move faster.
• Gas particles hit the walls of the container more often at higher temperatures.

• Some of the characteristics of gases are explained by the kinetic molecular theory.
• You can smell perfume when a bottle is opened on the other side of a room because its particles move rapidly in all directions.
• The molecules in the air are moving at 1000 mph at room temperature.
• They move more slowly at lower temperatures.
• When temperatures are high, tires and containers can explode.
• When gas particles are heated, they move faster, hit the walls of a container with more force, and cause a build-up of pressure inside a container.

• Pressure, volume, temperature, and the amount of gas are the four properties of a gas.

• They hit the walls of the container.

• Why does heating the container cause it to smash into the walls of the container more often and with increased force.

• Each of us is under pressure from a column of air that extends from the atmosphere to the surface of Earth.

• You can hear or see the atmospheric pressure in countries other than the United States on a TV weather report.
• The unit torr or pounds per square inch can be used in a hospital.

• The volume of gas is the same as the size of the container.
• Adding more gas particles is what happens when you inflate a tire.
• The volume increases when the number of particles hitting the walls of the tire or basketball increases.
• A tire can look flat on a cold morning.
• The volume of the tire has decreased because of a lower temperature, which reduces the speed of the molecule, which in turn reduces the force of their impacts on the walls of the tire.
• L and mL are the most common units for volume measurement.

• The temperature of a gas is related to its particles.
• The gas particles will have more energy than they did at 200 K if we heat it to 400 K.

• All comparisons of gas behavior and all calculations related to temperature must be done using the kelvin temperature scale.

• Scientists predict that the particles will have zero pressure and zero energy at absolute zero, even though no one has created the conditions for it.

• When you add air to a bicycle tire, it increases the amount of gas in the tire.
• In grams, we measure the amount of gas.
• The grams of gas need to be changed to moles.

• The properties of a gas are given in a summary.

• The number of grams of helium increases when it is added to a balloon.

• The amount of gas is given by the mass in grams.

• A tube of mercury called a manometer is used to check your blood pressure.
• A physical examination is done after the cuff is wrapped.
• There are two separate measurements.

• The normal slowly released from the range is 100 to 200mmHg.
• Reducing the pres is 60 to 80mmHg.
• The two measures are usually expressed as a sure sign of the arteries.
• Older people have higher values.

• There is a higher risk of stroke, heart attack, or kidney damage when the blood pressure is 140/90 or higher.
• The brain can hear low blood pressure, which can cause dizziness and fainting.

• A stethoscope and inflatable cuff are used to measure blood pressure during a physical exam.

• Sound is heard in the arteries of people using digital blood pressure monitors.
• A second pressure reading is taken.
• They have not been tested for use in all situations and moment of silence, and the pressure when can give inaccurate readings.

• Billions and billions of gas particles hit against the walls of a container, and they exert pressure, which is a force acting on a certain area.

• The pressure unit is named after Evangelista Torricelli, the inventor of the barometer.
• The units of Torr and MMHg are the same.
• It is equivalent to 29.9 in.

• The downward pressure of a mercury column in a closed glass tube is equal to the pressure in the exact atmosphere.
• The mercury column height is called atmospheric pressure.

• Pressures are reported in kilopascals because a pascal is a very small unit.

• The US equivalent of 1 atm is 14.7 lbs/in.2.
• It is possible to check the air pressure in the tires of a car with a pressure gauge.
• The pressure on the outside of the tire is influenced by the atmosphere.

• The measurement of pressure is done using 1 atm and 1 arious units.

• The mercury column rises on a sunny day.
• The mercury column falls on a rainy day because the atmosphere exerts less pressure.

• The level of the atmospheric pressure decreases.

• Divers need to be aware of the pressures on their ears and lungs when they dive into the ocean.
• As the diver descends, the pressure on the diver increases rapidly.
• At a depth of 33 feet below the ocean's surface, the water exerts 1 atm of pressure on the diver, which results in a total pressure of 2 atm.
• There is a total pressure of 4 atm on a diver at 100 ft.
• The pressure of the breathing mixture is adjusted continuously by the diver's regulator.

• The hospital respiratory unit has a tank of oxygen that has a pressure of 888-492-0 888-492-0.

• The pressure of the oxygen gas can be calculated.

• A patient with severe COPD gets oxygen from an oxygen tank.

• A tank of nitrous oxide is used as an anesthesia.

• A container of cooking spray explodes.

• The hot-air balloon's air is heated to make it rise.

• You can smell the smell of onions cooking.

• Gases move at higher temperatures.

• Gases can be compressed more quickly than liquids.

• Gases have low densities.

• Oxygen is in a tank at a pressure of 2.20 atm.

• When the temperature and amount of gas don't change, use the pressure-volume relationship to calculate the unknown pressure.

• Imagine if you could see the air particles hitting the walls.

• The pressure within the container increases as the air particles are crowded together.

• When a change in one property causes another to change, the properties are related.

• The pressure and volume are related.

• Whitney had an asthma attack and was given oxygen through a face mask.

• The given and needed quantities should be stated.

• The pressure decreases from 3800 to 570.
• We predict that the volume will increase because of the oxygen available.

• The gas law equation can be used to solve a mystery.

• The ratio of pressures is greater than 1, which increases the volume as predicted.

• 2 is equal to 12 L.

• There is a bubble of methane gas in an underground gas reserve.

• When you consider the mechanics of breathing, the importance of Boyle's law becomes apparent.

• The rib cage elastic, balloon-like structures contained within an air expands as it contracts.
• The flexible floor of the cavity is formed by the rib muscles.

• The process of taking a breath of air begins when the lungs contract and the rib cage expands.
• The lung's elasticity allows it to expand.

• When the volume of the lungs increases, the pressure in the lungs falls below the pressure of the atmosphere.

• The lungs squeeze between the lungs and the environment because their volume decreases.
• The volume and pressure of the lungs have changed.

• A closed container holds a gas at a pressure of 2.0 atm.

• The pressure goes up to 6.0 atm.

• The pressure is still at 2.0 atm.

• The pressure goes down to 0.40 atm.

• If there is a pressure of 650mmHg and a volume of 220 mL of hydrogen gas, the air in the cylinder has a pressure of 220mmHg.

• The air pressure in the tank is 1.20 atm.

• A sample of oxygen has a pressure of 760 and a volume of 30.0 L.

• There is a balloon.

• A sample of Ar gas has a volume of 5.40 L. When the pressure is 3.62 atm, there is no change in temperature or amount of gas.

• A sample of Ne gas has a pressure that is unknown.

• The atmospheric pressure doesn't change even though the balloon is inside the house.

• C3H6 is a general anesthetic.

• The balloon is placed in a chamber that has a pressure of five atm.
• What is the final volume in liters?

• A closed container holds a gas with a volume of 4.0 L. A patient's oxygen tank holds 20.0 L of oxygen at a pres pressure when the volume changes at a certain time.

• The volume is small.

• The volume increases to 12 L.

• The volume was compressed to 0.40 L.

• The diaphragm moves up into the lung.

• The lungs have higher pressure than the atmosphere.

• When the pressure and amount of gas don't change, use the temperature-volume relationship to calculate the unknown temperature.

• You are going to take a ride in a hot-air balloon.
• The captain uses a propane burner to heat the air inside the balloon.
• When the air is heated, it expands and becomes less dense than the air outside, which causes the balloon and its passengers to lift off.
• Jacques Charles proposed in 1787 that the volume of a gas is related to the temperature.

• Charles's law is that hot-air balloon gas expands when it is heated.

• The amount of gas and pressure are not changed when the temperature is changed.
• When the amount of gas does not change, the volume of the container must also decrease.

• Laparoscopic surgery uses helium gas to inflate the abdomen.
• A sample of gas has a volume of 5.40 L and a temperature of 15 degrees.

• The given and needed quantities should be stated.

• The temperature goes from 15 to 42 degrees.
• The volume will increase if the temperature of the gas is Charles's law.

• The gas law equation can be used to solve a mystery.
• The temperature increases.

• The table shows that the temperature has gone up.
• The volume must increase because the temperature is related to it.
• The ratio of the temperatures is greater than 1, which increases the volume as predicted.

• The temperature of the air that a mountain climber inhales is -8 degC.

• A volume of air is breathed into the lungs on a cold day, where the body temperature is 37 degrees.

• The hot-air balloon's heater is turned off.

• The amount of gas in a car on a hot day is the same as in a balloon filled with helium at the amusement park.

• A sample of argon has a volume of 3.80 L.

• A gas has a volume of 4.00 L.

• Neon gas is contained in a balloon at 45 degrees.

• The temperature went from 100 K to 300 K.

• There is a balloon in the freezer.

• An air bubble has a volume of 0.500 L. There is no change in the pressure or amount of gas.

• A gas sample has a volume of 0.256 L with no change in the pressure or amount of ture.
• The temperature gas has a volume of 0.198 L.

• When the volume and amount of gas don't change, use theGay-Lussac's law to calculate the unknown temperature or pressure.

• If we could observe the molecule of a gas as the temperature rises, we would notice that they move faster and hit the sides of the container more often.
• The pressure would increase if volume and amount of gas did not change.

• Oxygen tanks can explode if they are heated.

• An oxygen tank has a pressure of 120 atm at a room temperature.

• If the pressure inside exceeds 180 atm, the decreases will be greater.

• The given and needed quantities should be stated.
• We can see that the temperature increases.
• We use Gay-Lussac's law to predict the pressure.

• The gas law equation can be used to solve a mystery.

• The pressure is increased when the temperature factor is greater than 1.

• We would expect the oxygen tank to break because the calculated pressure of 270 atm exceeds the limit of 180 atm.

• In a storage area of a hospital where the temperature is 55 degrees, the pressure of oxygen gas in a steel cylinder is 965 Torr.
• When the volume and a hospital storage room are involved, the oxygen gas has to be cooled down to 850 Torr.

• The volume and amount of gas in the sample do not change.

• The perature of a gas with an initial pressure of 1500 Torr is 22 degrees.
• The final temperature was cooled to 20 degrees.

• The temperature is heated to 28 degrees.

• There is a pressure of 520.

• There is steam at 1.00 atm and 100 degC.

When the temperature of -12 degC is heated to give a pressure of 1650 Torr, what is the pressure?