Gas Laws Test Gas Pressure Gas Pressure Kinetic Molecular Theory of Ideal Gases Kinetic Molecular Theory of Ideal Gases Boyle’s Law (Problems & KMT) Boyle’s Law (Problems & KMT) Charles’ Law (Problems & KMT) Charles’ Law (Problems & KMT) Gay-Lussac’s Law (Problems & KMT) Gay-Lussac’s Law (Problems & KMT) Combined Gas Law (Problems) Combined Gas Law (Problems) Avogadro’s Law Avogadro’s Law Dalton’s Law of Partial Pressures (Problems) Dalton’s Law of Partial Pressures (Problems) Diffusion/Effusion (Definitions, Light Vs. Heavy) Diffusion/Effusion (Definitions, Light Vs. Heavy) Real Vs. Ideal Gases (Differences, Conditions) Real Vs. Ideal Gases (Differences, Conditions)

Gases can be compressed because A.) gas molecules are in constant motion B.) gas molecules move in straight lines between collisions with the walls of the container C.) the size of a gas molecule is very small compared to the space between molecules D.) there are no forces of attraction between gas molecules E.) gas molecules slow down when they become cooler

According to the kinetic theory of gases, which assumption is correct? A.) Gas particles strongly attract each other B.) Gas particles travel in curved paths C.) The volume of gas particles prevents random motion D.) Energy may be transferred between colliding particles

The kinetic molecular theory assumes that the particles of an ideal gas A.) are in random, constant, straight-line motion B.) are arranged in a regular geometric pattern C.) have strong attractive forces between them D.) have collisions that result in the system losing energy

In a gaseous system at equilibrium with its surroundings, as molecules of A(g) collide with molecules of B(g) without reacting, the total energy of the gaseous system A.) decreases B.) increases C.) remains the same

If the pressure on a given mass of gas in a closed system is increased and the temperature remains constant, the volume of the gas will A.) decrease B.) increase C.) remain the same

As the pressure of a gas at 760 torr is changed to 380 torr at constant temperature, the volume of the gas A.) decrease B.) increase C.) remain the same Decrease Pressure, Increase Volume

A gas sample has a volume of 25.0 millilters at a pressure of 1.00 atmosphere. If the volume increases to 50.0 milliliters and the temperature remains constant, the new pressure will be A.) 1.00 atm B.) 2.00 atm C.) atm D.) atm PV = PV (1.00atm)(25.0mL) = P(50.0mL)

A cylinder with a tightly fitted piston is shown in the diagram below. A.) decreases B.) increases C.) remains the same

A sample of gas is held at constant pressure. Increasing the kelvin temperature of this gas sample causes the average kinetic energy of its molecules to A.) decrease and the volume of the gas sample to decrease B.) decrease and the volume of the gas sample to increase C.) increase and the volume of the gas sample to decrease D.) increase and the volume of the gas sample to increase

A quantity of gas has a volume of 254 mL at 27ºC. When the temperature becomes 17ºC at constant pressure the gas has a volume of A.) 263 mL B.) 246 mL C.) 299 mL D.) 160 mL V = V T 254mL = V 300K 290K

If the temperature on a given mass of gas in a closed system is increased and the volume remains constant, the pressure of the gas will A.) decrease B.) increase C.) remain the same

A fixed volume of gas exerts a pressure of 1.00 atm at a temperature of 25ºC. What is the pressure of the gas when it is heated to 100ºC? A.) atm B.) 1.25 atm C.) 2.50 atm D.) 4.00 atm P = P T 1atm = P 298K 373K

Which will always decrease the volume of a sample of methane gas which occupies a volume of 2.4 L at 25 °C? A.) An increase in pressure and an increase in temperature B.) A decrease in pressure and a decrease in temperature C.) An increase in pressure and a decrease in temperature D.) A decrease in pressure and an increase in temperature

A gas occupies a volume of 444 mL at 273 K and 79.0 kPa. What is the final kelvin temperature when the volume of the gas is changed to 1880 mL and the pressure is changed to 38.7 kPa? A.) 31.5 K B.) 292 K C.) 566 K D.) 2360 K (79.0kPa)(444mL) = (38.7kPa)(1880mL) 273K T

The temperature of a 2.0-liter sample of helium gas at STP is increased to 27ºC and the pressure is decreased to 80. kPa. What is the new volume of the helium sample? A.) 1.4 L B.) 2.0 L C.) 2.8 L D.) 4.0 L (101.3kPa)(2.0L) = (80kPa)V 273K 300K

At the same temperature and pressure, 1.0 liter of CO(g) and 1.0 liter of CO 2 (g) have A.) equal masses and the same number of molecules B.) different masses and a different number of molecules C.) equal volumes and the same number of molecules D.) different volumes and a different number of molecules

The atmosphere contains a mixture of gases with a total pressure of 760 Torr. The partial pressure of Oxygen is Torr, Argon is 7.10 Torr, and Carbon dioxide is 0.27 Torr. What is the partial pressure of Nitrogen? A.) 594 Torr B.) 926 Torr C.) Neither is correct 760Torr = Torr Torr Torr + P N

Which of the gases below will diffuse the fastest? A.) NH 3 B.) N 2 C.) CO 2 D.) Ar 17g/mol 28g/mol 44g/mol 40g/mol Lighter is faster

If you were to blow up a balloon inside and then take it outside into the blistering cold, the balloon would: A.) shrink B.) expand C.) stay the same size D.) not enough information is given Decrease Temperature, Decrease Volume

The pressure inside a container of gas can be increased in each of the following ways, except: A.) Increasing the amount of gas in the container B.) Increasing the temperature of the gas C.) Increasing the volume of the container D.) Increasing the size of the gas molecules More particles, more collisions Faster moving, more collisions More room to move, less collisions Larger particles mean less volume to move. More collisions

If a set amount of gas occupies a container and the volume of the container decreases, what happens to the pressure inside the container? A.) the pressure decreases B.) the pressure increases C.) the pressure remains the same D.) the volume cannot decrease because the gas has filled the container Decrease Volume, Increase Pressure The space between particles allows the volume to be compressed

The evening before a birthday party, several balloons are filled with helium gas. The birthday party occurs on a hot summer day. The next day some of the balloons have burst! They burst because A.) The helium particles got bigger B.) The space between the helium particles increased C.) A and B are the correct reasons Increasing temperature increases volume (the distance between the particles, causing them to occupy more space). Temperature does not effect the attraction between the nucleus and the electron cloud (no change in particle size)

The evening before a birthday party, several balloons are filled with helium gas. The birthday party occurs on a hot summer day. The next day the balloons made of latex became smaller. This is because A.) Some of the helium particles escaped through pores in the latex B.) The helium particles became smaller C.) The helium particles compressed each other as they moved D.) None of the above explains it Diffusion

The evening before a birthday party, several balloons are filled with helium gas. The birthday party occurs on a hot summer day. A guest at the party dives in the swimming pool holding an inflated balloon! When she gets to the bottom of the pool, the balloon A.) becomes smaller B.) becomes bigger C.) does not change in size D.) does not submerge with the diver Increase Pressure, Decrease Volume

If there is a fire, you are told to get low to the ground because hot air rises. Hot air rises because A.) Heat always flows upward B.) Diffusion causes heat to rise C.) The lower air pressure at the ceiling attracts the hot air D.) Heat causes gases to expand, making them less dense and allowing them to rise High Temp to Low Temp

A real gas differs from an ideal gas because the molecules of real gas have A.) some volume and no attraction for each other B.) some volume and some attraction for each other C.) no volume and no attraction for each other D.) no volume and some attraction for each other

Helium is most likely to behave as an ideal gas when it is under A.) high pressure and high temperature B.) high pressure and low temperature C.) low pressure and high temperature D.) low pressure and low temperature

A real gas behaves more like an ideal gas when the gas molecules are A.) close and have strong attractive forces between them B.) close and have weak attractive forces between them C.) far apart and have strong attractive forces between them D.) far apart and have weak attractive forces between them

Under which conditions of temperature and pressure would helium behave most like an ideal gas? A.) 50 K and 20 kPa B.) 50 K and 600 kPa C.) 750 K and 20 kPa D.) 750 K and 600 kPa High temperature, low pressure