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Cell Structure Class > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Which of the following correctly reflects the relationship between the volume and the external pressure on a gas at constant temperature?

A
  1. As pressure decreases, volume will increase.

2. Pressure and volume are inversely prepositional.

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2
Q

How does a gas exert pressure?

A

The moving gas particles strike each other and the wall of the container, exerting a force.

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3
Q

Pressure =

A

Force/Area

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4
Q

The SI unit for pressure is?

A

The Pascal (pa)

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5
Q

Boyles Law?

A

states the at constant temperature, the volume occupied by a fixed amount of gas is inversely promotional to the applied pressure. This means that as the pressure on the gas increases, the volume will decrease.

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6
Q

Pressure decreases with ?

A

Altitude

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7
Q

Manometers

A

Used to measure the pressure of a gas in an experiment

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8
Q

Barometer

A

Uses Mercury to measure atmospheric pressure = 760mmHg.

Invented by Torricelli

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9
Q

Closed-end Manometer

A

a mercury-filled, curved tube is closed at one end and attached to a flask at the other. When the flask is evacuated, the mercury levels in the two arms of the tube are the same because no gas exerts pressure on either mercury surface. When a gas is in the flask, it pushes down the mercury level in the near arm, causing the level to rise in the far arm. The difference in column heights (Δh) equals the gas pressure.

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10
Q

Open-end Manometer

A

also consists of a curved tube filled with mercury, but one end of the tube is open to the atmosphere and the other is connected to the gas sample. The atmosphere pushes on one mercury surface, and the gas pushes on the other. Again, Δh equals the difference between two pressures. But, when using this type of manometer, we must measure the atmospheric pressure with a barometer and either add or subtract Δh from that value.

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11
Q

1 atm=

A

760 mmHg

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12
Q

1 torr=

A

1 mmHg

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13
Q

1 atm=

A

101.325 kPa

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14
Q

Charles’s Law

A

at constant pressure, the volume occupied by a fixed amount of gas is directly proportional to its absolute (Kelvin) temperature

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15
Q

Volume of 1 mole of an ideal gas at STP?

A

22.4L

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16
Q

0 Kelvin is equal to what C

A

-273.15 C

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17
Q

Avagadro’s Law

A

at fixed temperature and pressure, equal volumes of any ideal gas contain equal numbers (or moles) of particles.

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18
Q

STP

A

0C (273.15K) 1 atm (760 torr)

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19
Q

R the universal gas constant is equal to

A

0.0821 atm . L/ mol . K

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20
Q

Thermodynamics

A

the study of energy and its transformation

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21
Q

Thermochemistry

A

is a branch of thermodynamics that deals with the heat involved in chemical and physical changes.

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22
Q

1st Law of Thermodynamics

A

states that the total
energy of the universe is constant.
Esystem=-Euniverse

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23
Q

Units of Energy

A

J

24
Q

Density of a gas

A

mass/volume

(O2: 32g/22.4L=1.43g/L

25
Q

What is moles = to

A

mass/Molar mass
Pv=(m/M)RT
d=P(M)/RT

26
Q

The density of a gas is ____ _____ to the temperature

A

Inversely Proportional

27
Q

The density of a gas is ____ _____ to the pressure

A

directly proportional

28
Q

An alternative approach for finding the density of most simple gases, but at STP only, is to divide the molar mass by the standard molar volume, 22.4 L:

A

d=m/v

29
Q

Through another rearrangement of the ideal gas law, we can determine the molar mass of an unknown gas or a volatile liquid (one that is easily vaporized):

A

M=mRT/PV

30
Q

in a mixture of unreacting gases, the total pressure is the sum of the partial pressures of the individual gases:

A

Daltons Law of partial pressure

31
Q

Mole Fractions

A

Mole of N2/Total amount mole

nN2/nN2 + nH2 (mole fractions for N2 and H2

32
Q

If the total pressure is due to the total number of moles, the partial pressure of gas A is the total pressure multiplied by the _____?

A

Mole fraction

33
Q

Kinetic Molecular Theory

Postulate 1

A

Particle volume. A gas consists of a large collection of individual particles with empty space between them. The volume of each particle is so small compared with the volume of the whole sample that it is assumed to be zero; each particle is essentially a point of mass.

34
Q

Kinetic Molecular Theory

Postulate 2

A

Particle motion. The particles are in constant, random, straight-line motion, except when they collide with the container walls or with each other.

35
Q

Kinetic Molecular Theory

Postulate 3

A

Particle collisions. The collisions are elastic, which means that, like minute billiard balls on a frictionless billiards table, the colliding molecules exchange energy but do not lose any energy through friction. Thus, their total kinetic energy (Ek) is constant. Between collisions, the molecules do not influence each other by attractive or repulsive forces.

36
Q

Distribution of molecular speeds at 3 temperatures

A
  • the curves flatten and spread at higher temperatures

- the most probable speed (the peak of each curve) increases as the temperature increases.

37
Q

Mean free path of a gas particle

A

The average distance a gas particle travels between collisions (either with other particles or the wall)

38
Q

Diffusion

A

the movement of one gas through another

39
Q

Effusion

A

process of a gas escaping through a tiny hole

40
Q

Change in internal E

A 
∆E= E Final-E initial
∆E= E products - E reactants
41
Q

By releasing some energy in a transfer to the surroundings

A

E final < E initial

42
Q

By absorbing some energy in a transfer from the surroundings

A

E initial < E final

43
Q

∆E = q + w

A

The total change in a system’s internal energy is the sum of the energy transferred as heat and/or as work:

44
Q

Positive Energy

A

Energy transferred into the system is positive because the system ends up with more energy.

45
Q

Negative Energy

A

Energy transferred out from the system is negative, because the system ends up with less energy.

46
Q

For a system that transfers energy only as heat (q) and does no work (w = 0), we have

A

∆E = q

47
Q

For a system that transfers energy only as work, q = 0

A

∆E = w

48
Q

A _____ function is path independent, meaning that only the ____ and ____ conditions are needed to measure the net change that occurred.

A

state
initial
Final

49
Q

A change in ∆H (enthalpy) is equal to the change in heat (q) when the system is at constant ______.

A

Pressure

50
Q

All common Sulfates soluble except

A

CaSO4, SrSO4, BaSO4, AgSO4, PbSO4

51
Q

All common fluorides soluble except

A

PbF2, Flourides of group 2A

52
Q

All common Chlorides, bromides, and Iodides soluble excpet

A

Ag+, Pb2+, Cu+, Hg22+

53
Q

All common Nitrates, acetates, and percholrates soluble

A

no exceptions

NO3-, CH3C00-, CLO4-

54
Q

All common compounds of Group 1A soluble

A

no exceptions

55
Q

All common metal hydroxides are insoluble except

A

Group 1A hydroxides, Ca(OH)2, Sr(OH)2, and Ba(OH)2

56
Q

All common carbonates (CO2-3) and phosphates (PO34-) are insoluble except

A

carbonates and phosphates of Group 1A, and NH4+

57
Q

All common sulfides are insoluble except

A

Sulfides of Group 1A, and NH4+

Cell Structure Class (2 decks)

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