Gases assignment and quiz

The table describes a gas stored in four different containers. Properties of Stored Gas Container Properties 1 · Low number of collisions with container walls · Medium average kinetic energy · Large number of particles 2 · Large number of collisions with container walls · Medium average kinetic energy · Small number of particles with little spaces between them 3 · Large number of collisions with container walls · High average kinetic energy · Large number of particles with large spaces between them 4 · Few collisions with container walls · Low average kinetic energy · Small number of particles Which container has gas stored at the highest temperature? 1 2 3 4

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Which statement best describes the collisions of gas particles according to the kinetic-molecular theory? When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with no gain or loss of energy. As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with no gain or loss of energy. When particles pass close enough to one another, their attractions pull them together, and then they bounce apart with a loss of energy. As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with a loss of energy.

As particles travel in straight lines, their paths sometimes meet, and then they bounce apart with no gain or loss of energy.

Which observation indicates that the kinetic-molecular theory has limited use for describing a certain gas? Gas particles are acting like tiny, solid spheres. Gas particles are obeying Newton's laws of motion. Increasing pressure is reducing the volume of the gas. Increasing collisions of gas molecules will increase energy between them.

Increasing collisions of gas molecules will increase energy between them.

Which statement best describes the compressibility of a gas? Increasing the temperature of a gas decreases the pressure. Increasing the temperature of a gas increases the pressure. Increasing the pressure on a gas decreases the volume. Increasing the pressure on a gas increases the volume.

Increasing the pressure on a gas decreases the volume.

A substance is made up of slow-moving particles that have very little space between them. Based on this information, what can most likely be concluded about this substance? It is not a gas because its particles do not move continuously. It is a gas because its particles move continuously in a straight line. It is not a gas because its particles do not have large spaces between them. It is a gas because its particles move in many different directions.

It is not a gas because its particles do not have large spaces between them.

Consider the graph. mc007-1.jpg Based on the information in the graph, which statement best applies to a gas? Its particles have the highest average kinetic energy. Its particles have the smallest volume of all three states of matter. Its particles are slowing down because of a temperature increase. Its particles are moving apart due to repulsion between them.

Its particles have the highest average kinetic energy.

Which is an example of the kinetic-molecular theory not holding true for a gas? The average kinetic energy of particles depends only on the temperature. The particles in a gas travel in straight lines in a continuous, random motion. The attraction between particles causes a gas to condense at low temperatures. The particles in a gas make up a small portion of the total volume of the gas.

The attraction between particles causes a gas to condense at low temperatures.

Which statement about gases is true? They are made up of particles that always move very slowly. They are made up of particles that travel in a curved path when in motion. They are made up of hard spheres that vibrate quickly in stationary positions. They are made up of hard spheres that are in random motion.

They are made up of hard spheres that are in random motion.

Imagine the movement of a single gas molecule inside a container. Explain the particle's motions in terms of kinetic-molecular theory.

Which of the following did you include in your response? Gas particles act like tiny, solid spheres. Gas particles are in constant, random motion. Gas particles obey Newton's laws of motion. Faster particles collide more often and with more force. Collisions are elastic, there is no energy lost as the particle hits the sides.

A student checks the air in her bicycle tires early in the morning when it is cool outside. If she measures it again later in the day when it is hotter outside, what will she most likely observe? Explain your answer in terms of kinetic-molecular theory.

Which of the following did you include in your response? The tire pressure will be higher when the temperature is higher. Pressure is the result of collisions of gas molecules with the walls of the tire. Temperature is a measure of the average kinetic energy of the gas molecules. As temperature increases, gas molecules move more quickly and they collide with the tire walls more frequently and with more force. Pressure and temperature are directly proportional.

A chemist is studying the properties of a gas under various conditions. He observes that when the gas is at room temperature and low pressure, it behaves as an ideal gas. When the gas is cooled to 10 kelvin and is placed under high pressure, however, it deviates significantly from an ideal gas. Explain these observations.

Which of these did you include in your answer? The ideal gas model assumes that gas particles experience no intermolecular attractions. At low temperature, gas particles move slowly. At high pressures, gas particles are very close together. The closeness of the gas particles and their low speed allow intermolecular forces to become important at high pressure and low temperature. The intermolecular forces cause the gas to deviate from ideal behavior.

Both hydrogen sulfide (H2S) and ammonia (NH3) have strong, unpleasant odors. Which gas has the higher effusion rate? If you opened a container of each gas in a corner of a large room, which odor would you detect first on the other side of the room? Assume the temperature is constant. Explain your answer.

Which of these did you include in your answer? The molar mass of H2S is greater than the molar mass of NH3, making the velocity and effusion rate of NH3 particles faster. Effusion rate is inversely proportional to molar mass. NH3 will have a higher average molecule velocity, so it will diffuse faster and will reach the other side of the room more quickly.

Which step will decrease the pressure of a gas inside a closed cubical container? increasing the number of moles of gas decreasing the volume of the container increasing the speed of the gas particles decreasing the temperature inside the container

decreasing the temperature inside the container

If gas particles start colliding with the walls of their metallic container with increased force, what is their direct effect? lower gas pressure higher gas pressure lower volume of gas higher volume of gas

higher gas pressure

According to the kinetic-molecular theory, the collision between two ideal gas particles is a result of... neither attraction nor repulsion. repulsion from the wall of the container. repulsion from other gas particles. attraction between the two particles.

neither attraction nor repulsion.

A graph of gas pressure versus the number of particles in a container is a straight line. Which other relationship will have a similar graph? volume versus pressure, because they are also directly proportional volume versus temperature, because they are also directly proportional volume versus pressure, because they are also inversely proportional volume versus temperature, because they are also inversely proportional

volume versus temperature, because they are also directly proportional