The weaker the intermolecular forces, the easier the liquid evaporates. Higher vapor pressure the faster it evaporates. Thus, the weaker the attractive forces, the higher the vapor pressure and vice versa.
When the temperature of a gas increases, the Kinetic Energy of the particles increases. This means that they move faster and apply a greater force when they collide with the walls of the container. As pressure is the force per unit area on the container, the pressure increases. This is Gay-Lussac's "Pressure Temperature" Law: "P = kT".
The particles in a liquid are very close together, so an increase in pressure cannot push them any closer. The particles in a gas are widely spaced, so they can easily be forced closer together. Gases are compressible, liquids are not.
warm air particles slowly pass heat energy to all the other air particles
According to Charles law, when pressure is kept constant,the volume of a given mass of gas is directly proportional to the absolute temperature.The given mass of gas starts to rise with the rise in temperature and reduces with reduction in temperature.
The particles of a liquid move from one place to another although they are close together. Because of this, a liquid changes shape depending on the container they are put in. It does not have a fixed shape. The volume of a liquid is fixed; it can be measured.
Explain the consumer equilibrium with the help of indifference curve?
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The equilibrium price exists when at that price supply and demand for a product are equal. Apparently at that price level everybody is happy and as long as nothing changes there will be no pressure. If it would arise because of an increase in eithersupply or demand, the price would no longer be an equilibrium price and it would shift to another - higher or lower - level.
madarchode machudda
illustrate and explain e the consumer equilibrium ender cardinalist and ordinalist?
The gas particles will spread out to encompass the entire volume of the container. The particles are constantly in motion and will run into the walls of the container creating pressure (basically). If heated, the particles will move faster, and slower if cooled.
Chemical equilibrium shifts to favor products when the concentration of products is decreased or the concentration of reactants is increased. This can be achieved by removing some of the product or adding more reactant to the system. Le Chatelier's principle states that a system at equilibrium will respond to changes in concentration, pressure, or temperature by shifting in a direction that helps restore equilibrium.
A syringe demonstrates the relationship between pressure and volume. When you pull the plunger, the volume inside the syringe increases, causing the pressure to decrease. This is because the air particles inside the syringe become more spread out, resulting in lower pressure.
Bernoulli's principle explains that as the speed of a fluid increases, its pressure decreases. This is because the faster-moving fluid particles have less time to exert pressure on the surrounding surfaces, resulting in lower pressure.
The air particles are closer together creating more pressure inside a ballon or tired and makes it expand
The particle model of matter describes matter as being made up of tiny particles (atoms and molecules) that are in constant motion. Changes in temperature or pressure affect the motion of these particles. With an increase in temperature, the particles move faster, leading to a change in state (e.g., solid to liquid to gas). Changes in pressure can also affect the arrangement and movement of particles, causing changes in state.
The kinetic theory explains Brownian motion as the random movement of particles in a fluid due to collisions with other particles. These collisions transfer momentum, causing the particles to move in random directions. This continuous bombardment of particles is responsible for the erratic, unpredictable motion observed in Brownian particles.