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CHEM 131 > Exam 3 > Flashcards

Exam 3 Flashcards

1
Q

The force exerted per unit area by gas particles as they strike the surfaces around them

A

Gas Pressure

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2
Q

Higher gas concentration leads to this

A

Higher pressure

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3
Q

Greater volume leads to this

A

Lower pressure

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4
Q

An evacuated glass tube closed on one end with the open end placed in a pool of mercury
-Standard atmospheric pressure at sea level is 760mmHG

A

Barometer

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5
Q

A U-shaped tube partially filled with a liquid used to measure the pressure of a gas in a container

A

Manometer

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6
Q

Four key properties of gases

A

Pressure (P), volume (V), temperature (T), and amount (mol)

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7
Q

Temperature and amount are constant
-P1V1=P2V2
-As volume decreases, pressure increases and vice versa

A

Boyle’s Law

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8
Q

Amount and pressure remain constant
-Temperature must be in Kelvin
-V1/T1=V2/T2
-Constant pressure increases as temperature increases and vice versa

A

Charles’s Law

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9
Q

Pressure of a gas is directly proportional to its temperature
-P1/T1=P2/T2

A

Charles’s Law

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10
Q

Equal volumes of gas contain the same number of particles at the same temperature and pressure
-Only the number of particles matter
-V1/n1=V2/n2

A

Avogadro’s Law

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11
Q

A combination of the previous laws that summarizes the relationships expressed in all three
-PV=nRT
-P=pressure (atm), v=volume (L), t=temperature (K), n= moles of gas particles, R=ideal gas constant (0.08206Latm/molK)

A

Ideal gas Law

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12
Q

At STP, what is P and T?

A

P=1 atm
-T=0 degrees C or 273.2 K

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13
Q

What is the volume occupied by 1 mole of gas particles at STP?

A

22.4L

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14
Q

How to find molar mass from the mass of a gas sample and its volume at a known pressure and temperature

A

Molar mass= mass/Moles

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15
Q

P total= (n total)RT/V
-The moles of a component as divided by the total moles of a gas in a mixture
-P A=X aP total

A

Dalton’s Law of Partial Pressures

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16
Q

At STP, 1 mol is equal to how many L?

A

1mol=22.4L

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17
Q

Higher temperature means what?

A

Faster particles

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18
Q

-Particle collisions are completely elastic with each other or container walls
Interaction between gas particles is negligible (attractive or repulsive)

A

Kinetic Molecular Theory

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19
Q

-Decreasing Volume: less room for gas particles, more collisions with the container, higher pressure
-Increasing volume: more room for gas particles, fewer collisions with the container, lower pressure

A

KMT and Boyle’s LAw

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20
Q

-Increasing Temperature: gas particles move faster, more collisions with the container, volume must increase to maintain pressure
-Decreasing Temperature: gas particles move slower, fewer collisions with the container, volume must decrease to maintain pressure

A

KMT and Charles’s Law

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21
Q

Increasing Amount: more gas particles present, more collisions with the container, volume must increase to maintain pressure
-Decreasing Amount: fewer gas particles present, fewer collisions with the container, volume must decrease to maintain pressure

A

KMT and Avogadro’s Law

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22
Q

-Gas particles will all have the same kinetic energy at a given temperature
-The total pressure of collisions is the same

A

KMT and Dalton’s Law

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23
Q

The process of a collection of molecules spreading out from an area of high concentration to an area of low concentration

24
Q

The process by which a collection of molecules escapes through a small hole into a vacuum

25
For two different gases at the same temperature, the ration of their rates of effusion is given by the following equation: Rate A/Rate B = square root of M B/M A -The heavier gas will have a slower rate of effusion
Graham's Law of Effusion
26
What does ideal behavior assume? -Do not work under high pressure and/or low temperatures
-No attraction between gas particles -Gas particles take up no space
27
[P+a(n/V)squared]X[V-nb]=nRT
Van der Waals's Equation
28
The study of the relationships between chemistry and energy
Thermochemistry
29
The capacity to do work
Energy
30
A force acting over a distance -Energy=work=force*distance
Work
31
The flow of energy caused by a difference temperature
Heat
32
Energy that is stored in an object -Associated with position or composition -Stored in the structure of a compound
Potential Energy
33
Energy of motion or energy that is being transferred -Thermal energy: related to the temperature of a substance and the motion of its particles
Kinetic Energy
34
KE=1/2*mass*velocity
Units of kinetic energy
35
The amount of energy needed to raise the temperature of 1 gram of water by 1 degree C
Calorie (cal)
36
Energy cannot be created or destroyed, only converted from one form to another -First law of thermodynamics
Law of Conservation of Energy
37
The material or process with which we are studying the energy changes within
System
38
Everything with which the system can exchange energy
Surroundings
39
Delta E sys+Delta E surr=0
Amount of energy gained/lost by the system must be equal to the energy gained/lost by the surroundings
40
The sum of the kinetic and potential energies of all the particles that compose the system
Internal Energy
41
Delta E=E final-E initial -Delta E=E products-E reactants
Change in internal energy of a system
42
A function whose result only depends on the initial and final conditions, not on the process used
State Function
43
-Delta E sys is negative -Delta E surr is positive --Delta E sys equals Delta E surr
When energy flows out of a system it goes to the surroundings
44
-Delta E sys is positive -Delta E surr is negative -Delta E sys equals - Delta E surr
When energy flows into a system it comes from the surroundings
45
q=C*Delta T -q: heat -C: heat capacity of the object -Delta T: the change in temperature
Heat Capacity
46
What factors affect heat capacity?
-Amount of matter -The type of material
47
q=mass*Cs*Delta T Cs: specific heat capacity -Delta T: change in temperature
Specific Heat Capacity
48
q sys= -q surr
Thermal Energy Transfer
49
q m= -q w
Thermal Energy Transfer
50
w= -P Delta V -Convert to J using 1L*atm=101.3J
Pressure/Volume Work
51
q=mass*Cs* Delta T
Thermal Energy
52
w= -P delta V
Work
53
Delta E =q+w
Measuring Delta E
54
Delta E=q
Measuring Delta E for a process at constant volume
55
q sys= -q surr
Delta E is measured by observing how the reaction impacts the surroundings
56
A constant volume instrument used to measure Delta E for combustion reactions
Bomb Calorimeter

CHEM 131 (1 decks)

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