phases of matter solidliquid gas visualize it! quiz

Phases of Matter

Solid Liquid Gas

Visualize it! Quiz

Heating/cooling curves:

Sublimation is when a solid goes directly to a gas without passing through the liquid phase.

Heat of fusion potential energy increases kinetic energy remains the same

Heat of vaporization potential energy increases kinetic energy remains the same

Answers to odd questions page 47-48

K = C + 273

C = K - 273

Answers to odd questions page 49

Q = M * C* Change in T

Heat of fusion is the amount of energy needed to melt one gram of ice into water at 0 degrees Celsius

343 J / g

Heat of vaporization is the amount of heat needed to evaporate 1 gram of water at 100 degrees Celsius

Hf = 2260 J /g

Answers to odd questions page 51 - 52

Ex: 25 grams of water are cooled from 20 oC to 10 oC What is the # of joules of heat energy released?

It involves a change in temp so use the formula

Q = M x C x (change in T)

M = 25 grams; C = 4.18 J/g x oC Change in T = 10

Answer = 1045 J

Ex: What are the total # of Joules needed to heat 150g of ice to water at

0 oC. No temp change and ice to water means heat of fusion.

Hf = 334 J/g ; Mass = 150 g Answer: 334J x 150 = 50100J

Ex : How many Joules of heat are needed to vaporize 100g of water to vapor at 100 oC. No temp. change and 100 oC.

Hv = 2260 J/g ; Mass = 100 g

Answer: 2260J x 100 = 22600 J

Kinetic Molecular TheoryPostulates of the Kinetic Molecular Theory of Gases

1. Gases consist of tiny particles (atoms or molecules) 2. These particles are so small, compared with the distances between

them, that the volume (size) of the individual particles can be assumed to be negligible (zero).

3. The particles are in constant random motion, colliding with the walls of the container.? These collisions with the walls cause the pressure exerted by the gas.

4. The particles are assumed not to attract or to repel each other. 5. The average kinetic energy of the gas particles is directly proportional

to the Kelvin temperature of the gas

Kinetic Theory and the Gas Laws

Dorin, Demmin, Gabel, Chemistry The Study of Matter ?, 3rd?Edition, 1990, page 323 (newer book)

A Gas Sample is Compressed

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 429

Boyle’s Law

Timberlake, Chemistry 7th?Edition, page 253

P vs. V (Boyle’s Data)

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 404

Boyle’s Law Illustrated

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 404

Charles?s Law

Timberlake, Chemistry 7th?Edition, page 259

Plots of V vs. T (Different Gases)

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 407

Ideal vs. Real Gases

No gas is ideal. As the temperature of a gas increases and the pressure on the gas decreases the gas acts more ideally.

Answers to odd questions page 54 - 56

Gas Mixtures and Dalton’s

Law

Dalton’s law states that the pressure of the total system is equal to the sum of all the partial pressures.

Filtration is used to separate Heterogeneous solutions.

Large particles which are not dissolved in the solution are easily separated using filters.

Heterogeneous Mixtures

Chromotography

Chromotography

Distillation

Separation of Homogeneous mixtures

Separates substances based on boiling points

Answers to Odd questions page 59