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Gen Chem > Exam III > Flashcards

Exam III Flashcards

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1
Q

What is ideal gas law?

A

PV = nRT; P=pressure, V=volume, n=# of mols, T=temp in Kelvin, R=0.0821

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2
Q

convert 760mmHg to torr, atm, psi, pascals

A

760 torr, 1 atm, 14.7 psi, 101,325 pascals

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3
Q

Which Gas Law? For a fixed amount of a gas at constant temp, the volume is inverse to the pressure

A

Boyle’s Law

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4
Q

What is Boyle’s Law?

A

P1V1 = P2V2

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5
Q

Which Gas Law? The volume of a fixed amount of gas at constant pressure is directly propotional to its temp in K

A

Charle’s Law

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6
Q

What is Charle’s Law?

A

V1/T1 = V2/T2

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7
Q

Which Gas Law? At a fixed temp and pressure, the volume of a gas is directly proportional to the # of mols of that gas

A

Avogadro’s Law

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8
Q

What is Avogadro’s Law?

A

v1/n1 = V2/n2

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9
Q

Which Gas Law? Relates pressure, volume, # of mols, temp all in one equation

A

Ideal gas low

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10
Q

What is General Gas Equation?

A

P1V1/T1 = P2V2/T2

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11
Q

Which Gas Low? The sum of the partial pressures exerted by each individual gas is the total pressure of the system

A

Dalton’s Law of Partial Pressures

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12
Q

What is Dalton’s Law of Partial Pressures?

A

Pt = P1 + P2 + P3?

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13
Q

Average Kinetic Energy is?

A

directly proportional to the temp of the system

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14
Q

What is Diffusion?

A

molecular movement of a gas going high consentration to lower

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15
Q

What is Effusion?

A

movement of gas through an opening

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16
Q

What is Graham’s Law?

A

rates of effusion of 2 different gases in inversely proportional to the square root of their molar masses

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17
Q

What is Polarity?

A

the tendency for a partial charge separation to occur within a molecule, either via lack of symmetry or via differences in electronegativity

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18
Q

What is intermolecular forces?

A

those in addition to bonds, that exist among different molecules

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19
Q

What is intramolecular forces?

A

those forces that exist within a molecule and help determine its preferred conformation

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20
Q

What is Dipole-Dipole interaction?

A

in polar compounds, the partially positive (delta+) end aligning itself with the partially negative (delta-) end of another molecule

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21
Q

What is Hydrogen Bonding?

A

the electrostatic attraction between polar molecules that occurs when a H atom bound to a highly electronegative atom such as FON

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22
Q

What is London Dispersion Forces?

A

The weakest intermolecular force. A temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.

23
Q

What are the forces acting among molecules called?

A

cohesion

24
Q

What are the forces acting between molecules and the surface of the container called?

A

adhesion

25
Q

What is the tendency of a liquid to rise in narrow tubes or to be drawn into small openings?

A

capillary action

26
Q

What is the phase? Change between liquid and gaseous states of matter

A

Vavorization/evaporation

27
Q

What is the pressure a liquid excerts on the atmosphere?

A

vapor pressure

28
Q

What is the pressure the atmosphere excerts on the liquid?

A

atmospheric pressure

29
Q

Increase atmospheric pressure = (increase/decrease) vapor pressure = (increase/decrease) boiling point

A

decrease VP, increase BP

30
Q

Increase temp = (increase/decrease) kinetic energy = (increase/decrease) vapor pressure

A

increase KE, increase VP

31
Q

Increase surface area of liquid = (increase/decrease) molecules intencity with atomospheric pressure = (increase/decrease) evaporative rate

A

increase MI, increase ER

32
Q

What is this phase change? Solid -> Liquid -> Gas

A

melting, evaporation

33
Q

What is this phase change? Gas -> Liquid -> Solid

A

condensation, freezing

34
Q

What is this phase change? Solid -> Gas

A

sublimation

35
Q

What is this phase change? Gas -> Solid

A

deposition

36
Q

What is Heating Curves?

A

graphically represent the phase changes for a substance

37
Q

What is Phase Diagram?

A

represents the conditions supporting different states of matter for a substance

38
Q

What is tha set of contions that supports all 3 states of matter (solid, liquids, and gas)?

A

triple point

39
Q

What is Covalent Solids?

A

have a network of covalent bonds throughout the crystal unit

40
Q

What is Ionic Solids?

A

contain gaseous cations and anions hold together in a matrix

41
Q

What is crystalline solids?

A

highly regular repeating network of atoms

42
Q

What is amorphous solid?

A

no order in the network of atoms

43
Q

What is the system? Neither heat nor matter is exhanged with the surroundings

A

isolated

44
Q

What is the system? Can exchange evergy, but not matter with the surroundings

A

closed

45
Q

What is the system? Exchanges both energy and matter with the surroundings

A

open

46
Q

Processes - conducted at some temp

A

isothermal

47
Q

Processes - conducted at some pressure

A

isobaric

48
Q

Processes - not heat exchange occurs

A

adiabatic

49
Q

stored energy

A

potential

50
Q

energy in motion

A

kinetic

51
Q

Derived from molecular motion, or temp of the system, also known as enthalpy

A

termal energy

52
Q

energy released as heat

A

friction

53
Q

1 calorie = ? Joules

A

4.184

54
Q

regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes

A

Hess’s Law

Gen Chem (1 decks)

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