How can you relate the kinetic molecular theory with the experiment?

The kinetic molecular theory can be used to explain each of the experimentally determined gas laws. The pressure of a gas results from collisions between the gas particles and the walls of the container. Each time a gas particle hits the wall, it exerts a force on the wall.

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What is kinetic molecular theory and how does it relate to phase changes?

Phase Changes

The amount of kinetic energy in a substance is related to its phase. Gases have more kinetic energy than liquids. Liquids have more kinetic energy than solids. When a substance increases in temperature, heat is being added, and its particles are gaining kinetic energy.

What does the kinetic molecular theory relate?

Kinetic Molecular Theory states that gas particles are in constant motion and exhibit perfectly elastic collisions. Kinetic Molecular Theory can be used to explain both Charles’ and Boyle’s Laws. The average kinetic energy of a collection of gas particles is directly proportional to absolute temperature only.

How do we use the kinetic molecular theory to explain the behavior of gases?

The physical behaviour of gases is explained by the kinetic molecular theory of gases. The number of collisions that gas particles make with the walls of their container and the force at which they collide determine the magnitude of the gas pressure. Temperature is proportional to average kinetic energy.

How does the kinetic molecular theory explain the properties of liquids?

The kinetic molecular theory suggests that the vapor pressure of a liquid depends on its temperature. As can be seen in the graph of kinetic energy versus number of molecules, the fraction of the molecules that have enough energy to escape from a liquid increases with the temperature of the liquid.

How can you relate the kinetic molecular theory with the experiment color drop?

Placing a drop of food coloring in water provides a visual representation of this process – the color slowly spreads out through the water. If matter were not made of particles, then we would simply see a clump of color, since there would be no smaller units that could move about and mix in with the water.

What do you understand by the kinetic energy of molecules?

Kinetic energy is a form of energy that an object or a particle has by reason of its motion. If work, which transfers energy, is done on an object by applying a net force, the object speeds up and thereby gains kinetic energy.

How do intermolecular forces relate with the assumptions of the KMT?

In particular, KMT’s assumptions that intermolecular forces are negligible, and the volume of molecules is negligible, aren’t always valid. Real gas molecules do experience intermolecular forces. As pressure on a real gas increases and forces its molecules closer together, the molecules can attract one another.

What are the main points of the kinetic theory of matter?

The kinetic theory of matter (particle theory) says that all matter consists of many, very small particles which are constantly moving or in a continual state of motion. The degree to which the particles move is determined by the amount of energy they have and their relationship to other particles.

What does the kinetic-molecular theory explain at least 3 things?

The simplest kinetic model is based on the assumptions that: (1) the gas is composed of a large number of identical molecules moving in random directions, separated by distances that are large compared with their size; (2) the molecules undergo perfectly elastic collisions (no energy loss) with each other and with the …

How does the kinetic theory of matter relate to heat transfer?

In kinetic theory, the molecular motion is responsible for this heat transfer as well. Collision of molecules of one system with another leads to transfer of energy from the more energetic molecule to the less energetic one.

What is the relationship between the kinetic energy of molecules in a solid and a liquid?

This explains why solids have a fixed volume and a fixed shape. If particles have enough kinetic energy to partly overcome the force of attraction between them, matter exists as a liquid. The particles can slide past one another but not pull apart completely.

How does kinetic molecular theory explain the relationship on the particles and the behavior of gases?

Kinetic Molecular Theory states that gas particles are in constant motion and exhibit perfectly elastic collisions. Kinetic Molecular Theory can be used to explain both Charles’ and Boyle’s Laws. The average kinetic energy of a collection of gas particles is directly proportional to absolute temperature only.

What does the kinetic theory explain quizlet?

Kinetic Theory. Explains how particles in matter behave by making three assumptions: 1) All matter is made of small particles. 2) These particles are in constant, random motion. 3) These particles are colliding with each other and the walls of their container. Assumption.

How do you explain the relationship of volume and temperature using kinetic molecular theory?

Any increase in the frequency of collisions with the walls must lead to an increase in the pressure of the gas. Thus, the pressure of a gas becomes larger as the volume of the gas becomes smaller. The average kinetic energy of the particles in a gas is proportional to the temperature of the gas.

How does kinetic theory fail to explain the behavior of real gases?

Kinetic theory or kinetic theory of gases attempts to explain overall properties of gases, such as pressure, temperature, or volume, by considering their molecular composition and motion. The theory basically states that pressure is not caused by molecules pushing each other away, like earlier scientists thought.

How are attractive forces related to the motion and the amount of kinetic energy of the particles?

If the kinetic energy is less than the attractive forces, a liquid or solid will form. The average kinetic energy of the particles in a gas is great enough to overcome the forces of attraction between them. The molecules of a gas move apart when they collide.

Why is it necessary to make assumptions while studying Behaviour of a gas?

Gases are compressible because gas molecules are so small compared to the volume of the gas. If the molecules took up more space, they couldn’t squish together as easily. We make this assumption because it makes the mathematics behind the model easier to follow and because gas molecules are really small.

How do intermolecular forces influence the properties of liquids?

As the intermolecular attraction increases, • The vapor pressure ( the pressure of the vapor that is in equilibrium with its liquid) decreases • The boiling point ( the temperature at which the vapor pressure becomes equal to the pressure exerted on the surface of the liquid) increases • Surface tension ( the …

How do intermolecular forces relate to solids liquids and gases?

Intermolecular forces are weaker attractions that hold molecules or noble gas particles close together when they are in a liquid or solid form. Gas particles have broken away from the intermolecular forces that hold liquids and solids together. An alternative name for intermolecular forces is the van der Waals forces.

How does the kinetic-molecular theory explain relatively high density in liquids?

According to the kinetic-molecular theory, liquids: a) have a relatively high density—the particles are close together – they’re only not in fixed positions as their solid relatives.

What is the importance of kinetic molecular theory of matter?

The kinetic theory of matter helps us understand why matter occurs in various stages (i.e. solid, liquid and gas) and how matter can change from one stage to the next. The kinetic theory of matter also enables one to consider other characteristics of matter.

What do you understand by kinetic theory of change of state?

The kinetic theory of matter states that all matter is made of small particles that are in random motion and that have space between them. This means that no matter what phase matter is in, it is made of separate, moving particles.

How would you explain the characteristics of a solid on the basis of the kinetic theory?

Answer: Solids have minimum kinetic energy due to least movement of particles. … Although the molecules can still vibrate, they cannot move from one part of the solid to another part. As a result, a solid does not easily change its shape or its volume.

What are the three main points of the kinetic theory as applied to a gas?

There are three main assumption of kinetic theory: (i) No energy is gained or lost when molecules collide. (ii)The molecules in a gas take up a negligible amount of space in relation to the container they occupy. (iii)The molecules are in constant, linear motion.

Which is a basic assumption of the kinetic theory?

The basic assumption of kinetic theory is that the measurable properties of gases, liquids, and solids reflect the combined actions of countless numbers of atoms and molecules. For example, the pressure exerted on the walls of a bicycle tire is produced by the impacts of an enormous number of air molecules.

What causes gas pressure kinetic theory?

The kinetic molecular theory can be used to explain each of the experimentally determined gas laws. The pressure of a gas results from collisions between the gas particles and the walls of the container. Each time a gas particle hits the wall, it exerts a force on the wall.

How is kinetic energy related to the particles of matter?

As we heat a substance we give more thermal energy to the particles which is converted to kinetic energy and hence they move faster and further apart. If we continue heating, eventually a phase change occurs, but during such a process the temperature (and hence kinetic energy) remains constant.

What is the relationship of particle motion and kinetic energy?

With an increase in temperature, the particles gain kinetic energy and move faster. The actual average speed of the particles depends on their mass as well as the temperature – heavier particles move more slowly than lighter ones at the same temperature.

How does the kinetic molecular theory describe the temperature pressure volume and intermolecular interactions of an ideal gas?

The behavior of ideal gases is explained by the kinetic molecular theory of gases. Molecular motion, which leads to collisions between molecules and the container walls, explains pressure, and the large intermolecular distances in gases explain their high compressibility.

What most accurately explains relationships among the phases energy and mobility of matter?

What most accurately explains relationships among the phases, energy, and mobility of matter? Molecules making up water vapor have more energy and are more mobile than molecules making up ice. Which substance has the highest particle mobility?

What is the relationship between the kinetic energy of molecules in an object and object temperature?

What is the relationship between the kinetic energy of molecules in an object and the object’s temperature? As the temperature increases, the kinetic energy of the molecules increases. The kinetic energy always increases whether the temperature increases or decreases.

Which is an example of the kinetic molecular theory not holding true for a gas?

Which is an example of the kinetic-molecular theory not holding true for a gas? The attraction between particles causes a gas to condense at low temperatures.

What happens to the average kinetic energy of a gas when the particles of the gas collide against each other at a constant temperature and volume explain your answer?

The average kinetic energy of a gas when the particles of the gas collide against each other at a constant temperature and volume does not change….

Under which circumstances will kinetic molecular theory fail?

When a gas is compressed under high pressure, the gas is no longer mostly empty space, it fails when the gas condenses to a liquid.

How do intermolecular forces relate with the assumptions of the KMT?

In particular, KMT’s assumptions that intermolecular forces are negligible, and the volume of molecules is negligible, aren’t always valid. Real gas molecules do experience intermolecular forces. As pressure on a real gas increases and forces its molecules closer together, the molecules can attract one another.

How do intermolecular forces of attraction affect the properties of liquids and solids?

Intermolecular forces determine bulk properties, such as the melting points of solids and the boiling points of liquids. Liquids boil when the molecules have enough thermal energy to overcome the intermolecular attractive forces that hold them together, thereby forming bubbles of vapor within the liquid.

What is the relationship between the amount of space between particles and the state of the matter?

What is the relationship between the amount of space between particles and the state of the matter? The relationship between the amount of space between particles and the state of the matter is that they both can be in shapes of solid, liquid, and gas. What is the difference between evaporation and sublimation?

What do you understand by kinetic theory of gas?

The model, called the kinetic theory of gases, assumes that the molecules are very small relative to the distance between molecules. The molecules are in constant, random motion and frequently collide with each other and with the walls of any container.

What are the important postulates of kinetic theory of gases derive the equation for kinetic theory of gases?

Kinetic Theory of Gases and Gas Law

From the average kinetic energy equation, PV = 2NE_average/3, but E_average = k’T. Therefore, PV = 2Nk’T/3, this energy equation calculates the necessary deductions of gas law like Boyle’s, Charles’s, and Avogadro’s law.

How does kinetic molecular theory explain the behavior of gases?

The Kinetic-Molecular Theory Explains the Behavior of Gases, Part II. According to Graham’s law, the molecules of a gas are in rapid motion and the molecules themselves are small. The average distance between the molecules of a gas is large compared to the size of the molecules.

How does the kinetic molecular theory and intermolecular forces explain the different phase change?

The more kinetic energy particles have, the weaker these forces become. At certain temperatures, particles overcome enough intermolecular forces to experience a significant change in properties. At this point, a phase change occurs.

How do the intermolecular forces present on it interact with each other?

When two particles experience an intermolecular force, a positive (+) charge on one particle is attracted to the negative (-) on the other particles. When intermolecular forces are strong the atoms, molecules or ions are strongly attracted to each other, and draw closer together.

What does kinetic molecular theory explain about liquids?

The kinetic molecular theory suggests that the vapor pressure of a liquid depends on its temperature. As can be seen in the graph of kinetic energy versus number of molecules, the fraction of the molecules that have enough energy to escape from a liquid increases with the temperature of the liquid.

How does the kinetic molecular theory explain that liquids can diffuse?

According to the kinetic-molecular theory of liquids, the particles are not bound together in fixed positions, but move about constantly. This particle mobility explains why liquids and gases are referred to as fluids. A fluid is a substance that can flow and therefore take the shape of its container.

How do intermolecular forces affect the capillary action of liquids?

Capillary Action. Intermolecular forces also cause a phenomenon called capillary action, which is the tendency of a polar liquid to rise against gravity into a small-diameter tube (a capillary), as shown in Figure 11.4. 3. When a glass capillary is is placed in liquid water, water rises up into the capillary.

How do the intermolecular forces present relate to the size of the substance?

For any given chemical, intermolecular forces are highest in the solid state and smallest in the gaseous state. The bigger the molecule, the larger the electron cloud and, as a result, the more intermolecular force is possible.

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