Phase Change: solid to liquid Melting
water Most solids shrink in size when frozen. What substance is an exception and actually expands?
GAS Use the phase diagram below to answer the following question. Use the phase diagram below to answer the following question. What phase of matter would this substance be in at 90 C and 0.25atm? A B C
Heat energy is either absorbed or released What can cause a phase change of matter?
What phase of matter is “B”? A B C Temperature Pressure Liquid
________is the gas phase of a substance normally solid or liquid at room temperature Vapor
C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of C was decreased, the system would shift to the ________ C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of C was decreased, the system would shift to the ________ LEFT
Freezing occurs by the release of _____ energy
Describe a volatile liquid in terms of its rate of evaporation. Evaporates quickly
______ is the resistance of a liquid to flow Viscosity
What phase of matter is “A”? A B C Temperature Pressure Solid
A _____________ is a graph of pressure versus temperature that shows which phase a substance exists in under different conditions of temperature and pressure. Phase diagram
What is the normal boiling point of water? 100 C
Melting occurs by energy being ______. absorbed
Released Deposition occurs when energy is (absorbed OR released).
____________ is the temperature and pressure at which all 3 states of matter are at equilibrium Triple point
Phase Change: solid to gas Sublimation
The triple point of this substance occurs at: 5.2 atm & K
When a system at equilibrium is disturbed by application of a stress, it attains a new equilibrium position that minimizes the stress. This is known as ___________ Le Chatelier’s Principle
C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of CO was increased, the system would shift to the ________ C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of CO was increased, the system would shift to the ________ LEFT
_______ is the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature. Equilibrium vapor pressure
________ is the temperature at which equilibrium vapor pressure equals atmospheric pressure Boiling point
__________ is a dynamic condition in which two opposing physical or chemical changes occur at equal rates in a given closed system Equilibrium
____________ is the spontaneous mixing of two or more substances. Diffusion
When does a liquid boil? Equilibrium vapor pressure EQUALS atmospheric pressure
What is the most abundant liquid? Water
_____________ is the energy required to increase the surface area of a liquid by a given amount; results from an uneven distribution of attractive forces. Surface tension
List 2 examples of surface tension. Meniscus Droplets can form Objects float Capillary rise
List a volatile substance Rubbing alcohol Nail polish remover Gasoline hairspray
When energy is taken away from a substance, the particles would move __________ Slower
Phase Change: liquid to solid Freezing
What happens to the boiling point of liquids on top of Mt. Everest? WHY? Boiling point is lower B/c atmospheric pressure is lower
C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 O was increased, the system would shift to the ________ C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 O was increased, the system would shift to the ________ Right
How does a substance evaporate, if equilibrium vapor pressure is LOW? WHY? SLOWLY! B/c there are STRONG IM forces and requires MORE kinetic energy to become a vapor
Describe a liquid in terms of particle spacing. Particles are packed relatively closely together
Describe a liquid in terms of particle motion. Particles vibrate around MOVING points
Water, olive Oil, Tree Sap Arrange the following in order of increasing viscosity at room temperature: tree sap, water, olive oil.
C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 was decreased, the system would shift to the ________ C(s) + H 2 O(g) CO(g) + H 2 (g) If the concentration of H 2 was decreased, the system would shift to the ________ RIGHT
Phase Change: gas to liquid Condensation
Describe the general volume of a liquid and use KMT to explain. Definite VOLUME- b/c particles are close together
Describe the general shape of a liquid and use KMT to explain. NO Definite SHAPE- b/c particles vibrate around moving points
Describe a liquid-vapor system at equilibrium. The number of particles vaporizing is EQUAL to the number of particles condensing
Unequal distribution of charge (oxygen is partially negative while hydrogen is partially positive) Why water is considered a polar molecule?
Phase Change: gas to solid Deposition
Both have particles changing from a liquid to a gas (vaporization) How are boiling and evaporation alike?
Phase Change: liquid to gas Vaporization
Temp. remains constant (does not change!) What happens to the temperature of substance during a phase change?
Phase change __________ is the transitioning from one state of matter to another.
Solid Use the phase diagram below to answer the following question. Use the phase diagram below to answer the following question. What phase of matter would this substance be in at 10 C and 1.0atm? A B C
Evaporation ONLY takes place at the surface and boiling vaporization is throughout liquid Heat is needed for boiling to occur and not for evaporation How are boiling and evaporation different? List one difference
RELEASED Condensation occurs when energy is (absorbed OR released).
What phase of matter is “C”? A B C Temperature Pressure Gas
What is the difference between the IM forces during melting and freezing? Melting = Less IM forces b/c more particle collisions Freezing = MORE IM forces b/c particles are moving slower
Using KMT, explain the evaporation rate of a volatile liquid. Quick evaporation rate. ◦ Has weak IM forces between particles so it requires LESS kinetic energy to become a vapor
Using KMT, explain the evaporation rate of a nonvolatile liquid. Slow evaporation rate ◦ Has strong IM forces between particles so it requires MORE kinetic energy to become a vapor
Rubbing Alcohol – it evaporates quickly b/c there is WEAK IM forces between the particles Which would you expect to be more volatile, water or rubbing alcohol? Explain.
B/c of the hydrogen bonding- the arrangement of the molecules in the solid crystalline structure take up more space, yet have the same mass; making ice less dense than liquid water. Explain why the solid state of water (ice) is less dense than the liquid state.
When energy is added to a substance, the particles would move ___________ Faster
Energy exchanges are not changes in kinetic energy – so temperature remains constant. ◦ Heat energy is used to change the IM forces between the molecules Explain why the temperature remains constant during a phase change.
FALSE they are the same = 0°C TRUE or FALSE: The temperature at which a substance freezes is lower than the temperature at which it melts. Why?