Unit 3 chemistry

Melting: From a solid to a liquid ; heat is added

Solidification: From a liquid to a solid; heat is removed; also called fusion

Sublimation: From a solid to a Gas

Depositions: Gas to Solid phase change

Evaporation: Liquid to gas; heat added

Definition:

Specific heat capacity

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They're Forces that act between stable molecules

Solid: Strong IMF, so low entropy

Liquid: Moderate IMF, so moderate entropy

Gas: Low IMF, so high Entropy

equation Q=mc^t

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Q: heat energy (Joules or calories)

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M: mass (g)

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C: Specific heat capacity

How mush energy it takes to heat up one gram of a substance by one degree Celsius

Specific heat: The higher the specific heat, the more energy is needed to heat up the substance/ Lower the specific heat= the less energy is needed

^t: Change in Temperature (Celsius)

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Temperature: Average Kinetic energy of particles in a substance

Hotter substances having faster moving particles

Units for temperature: Celsius does not work for gas laws so Kelvins should be used K= Celsius + 273

Liquid

Indefinite Shape, Definite Volume, Less Organized

Solid

Gas

Indefinite Shape, Indefinite Volume, Very Disorganized

Plasma

A Gas heated up so intensely that the electrons break away from their distinct atoms

In order from Solids to a Gas is the Increase in Entropy and Kinetic Energy

Entropy: How much "Chaos" in the molecules of a substance

Atmospheres (ATM): Normal atmospheric pressure is one atm

KiloPascals (kPa): The normal atmospheric pressure for this is 101.325 kPa

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Definition: the amount of space a gas takes up; measured in Liters (L) for gases; possibly measured in mL; 1L=1000 mL

Particles have no volume

Particles have no intermolecular forces

Particles are in constant motion and travel randomly in straight lines, bouncing off one another

Boyles Law: As pressure increases, volume decreases; P1 V1= P2V2

Charle's Law: As gas temperature increases, Volume increases; equation is V1/T1= V2/T2

Combined gas law: It is a combination of Boyle's and Charles' law, where one of the values does not always have to e constant, so you may use any variables

Dalton's Laws of partial pressure: If you have a mixture of gases, the total pressure is the sum is all the pressures of each gas; P total= (P1+P2+........)

Critical pressure: occurs at 218 atm in water

Normal freezing point: 32 degrees fahrenheit or 273.15 Kelvin

Triple point: It is that temperature and pressure at which the sublimation curve, fusion curve and the vaporization curve meet. or the temperature and pressure at which the solid, liquid, and vapor phases of a pure substance can coexist in equilibrium.

Normal boiling point: It's the temperature at which a liquid boils at 1 atmosphere of pressure.

Critical point: the point on the phase diagram at which both the liquid and gas phases of a substance have the same density, which means they are indistinguishable.

Pressure (atm or kPa)

Volume: (L or mL)

Number of Moles of the gas (mol or Mole)

R: Gas constant

Temperature (k)