Calorimetry: n this video Paul Andersen describes the history of calorimetry and explains how it can be used to measure energy changes in a system. The specific heat of water is well established and so as a system releases or absorbs energy from a surrounding water bath it can be measured. Calorimeters can be used to measure the specific heat capacity of a substance as well as the enthalpy of fusion, vaporization, and reaction.

Calorimetry: n this video Paul Andersen describes the history of calorimetry and explains how it can be used to measure energy changes in a system. The specific heat of water is well established and so as a system releases or absorbs energy from a surrounding water bath it can be measured. Calorimeters can be used to measure the specific heat capacity of a substance as well as the enthalpy of fusion, vaporization, and reaction.

Sublimation: the transition of a substance directly from the solid to the gas phase without passing through an intermediate liquid phase; an endothermic phase transition that occurs at temps and pressures below a substance's triple point in its phase diagram; reverse is desublimation or deposition; as you observe an ice crystal in freezing air, an occasional molecule will gain enough energy to break away from its neighbors and enter into the air above

Sublimation: the transition of a substance directly from the solid to the gas phase without passing through an intermediate liquid phase; an endothermic phase transition that occurs at temps and pressures below a substance's triple point in its phase diagram; reverse is desublimation or deposition; as you observe an ice crystal in freezing air, an occasional molecule will gain enough energy to break away from its neighbors and enter into the air above

Energy Changing Processes: In this video Paul Andersen explains how energy can enter and leave a system. The amount of energy a substance can receive through heating or lose through cooling is measured using the specific heat capacity. Phase changing energy from solid to liquid is known as the enthalpy of fusion and phase-changing energy from a liquid to a gas is known as the enthalpy of vaporization. The energy leaving or entering a chemical reaction is the enthalpy of reaction.

Energy Changing Processes: In this video Paul Andersen explains how energy can enter and leave a system. The amount of energy a substance can receive through heating or lose through cooling is measured using the specific heat capacity. Phase changing energy from solid to liquid is known as the enthalpy of fusion and phase-changing energy from a liquid to a gas is known as the enthalpy of vaporization. The energy leaving or entering a chemical reaction is the enthalpy of reaction.

What are the phase changes? Phase changes going toward decreasing enthalpy of system are exothermic and have -ΔH and -ΔS. Sublimation>vaporization>fusion for changes in enthalpy and entropy.

What are the phase changes? Phase changes going toward decreasing enthalpy of system are exothermic and have -ΔH and -ΔS. Sublimation>vaporization>fusion for changes in enthalpy and entropy.

Chemistry in everyday life Have you ever wondered why chemistry is so important? Why do we study chemistry?  We all are made of chemicals and everything around us is made of chemicals. Everything we hear, see, smell, taste, and touch involves chemistry and chemicals (matter). Hearing, seeing, tasting, and touching all involve intricate series of chemical reactions and interactions in our body

Chemistry in everyday life Have you ever wondered why chemistry is so important? Why do we study chemistry? We all are made of chemicals and everything around us is made of chemicals. Everything we hear, see, smell, taste, and touch involves chemistry and chemicals (matter). Hearing, seeing, tasting, and touching all involve intricate series of chemical reactions and interactions in our body

This is a periodic table in which the elements are ordered by the energy level of their subshells and by the number of electrons in their outer subshell.  This layout makes it easier to understand how the properties of all elements relate to the orbital structure of the atom.  The table maintains periodicity, and gives the electron configurations required in modern chemistry but missing from the traditional table.

This is a periodic table in which the elements are ordered by the energy level of their subshells and by the number of electrons in their outer subshell. This layout makes it easier to understand how the properties of all elements relate to the orbital structure of the atom. The table maintains periodicity, and gives the electron configurations required in modern chemistry but missing from the traditional table.

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