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Chem 112 > Chapter 5 > Flashcards

Chapter 5 Flashcards

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1
Q

What is pressure?

A

The result of the collisions between atoms or molecules in a gas and the surfaces around them

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2
Q

What is the formula for finding pressure?

A

Pressure=Force/Area of surface in which particles collide

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3
Q

What device is used to measure pressure in millimeter of mercury (1 mmHg or 1 torr)

A

Barometer

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4
Q

What does one average pressure at sea level (atmosphere, atm) equal in mmHG or torr?

A

1 atm= 760 mmHg

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5
Q

What is one pascal or newton per square meter equal to in atm? (Pa, N/m2)

A

1 atm= 101 325 Pa

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6
Q

What is one atm in psi?

A

1 atm=14.7 psi

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7
Q

What are the four basic physical properties of gas?

A

Pressure P
Volume V
Temperature T
Moles n

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8
Q

What is Boyle’s law about volume and pressure?

A

Volume and pressure have an inverse relationship

V=constant/P

P1V1=constant=P2V2

P1V1=P2V2

AS LONG AS TEMPERATURE AND MOLES ARE CONSTANT

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9
Q

What does Charles law on volume and temperature state and what formula does it give?

A

States that volume and temperature have direct proportionality
V=constant x T

V1/T1=V2/T2

AS LONG AS PRESSURE AND AMOUNT OF MOLES ARE CONSTANT

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10
Q

What is avogadros law on volume and number of moles and what equation does it give us?

A

Linear relationship between volume and number of moles
V= constant x n

V1/n1=V2/n2

AS LOMG AS PRESSURE AND TEMPERATURE STAY CONSTANT

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11
Q

What is an example of avogadros law in real life?

A

Inflating a balloon
Which each exhale you add more gas particles inside the balloon increasing its volume
You can use avogadros law to calculate the volume of a gas following a change in the amount of gas

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12
Q

What equation does the ideal gas law give us?

A

Putting everything together we get
V= constant (nT/P)

V= RnT/P

PV= nRT

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13
Q

What is gay-lussac’s law and what equation does it give us?

A

P= constant x T

P1/T1=P2/T2

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14
Q

What is the difference between total pressure and gauge pressure?

A

Gauge pressure is the difference between the total pressure and atmospheric pressure

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15
Q

What is molar volume?

What is volume at STP?

A

The volume occupied by one mole of a substance

STP- 273.15 K and 1.00 atm
Standard temperature and pressure

22.4L

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16
Q

What is the formula for density with a gas under standard temperature and pressure?

A

Density= molar mass/ molar volume (22.4L)

The density of a gas is directly proportional to its molar mass

D= PM(molar mass)/RT

17
Q

What is partial pressure (Pn)?

What is it’s formula?

A

Partial pressure is the pressure due to any individual component in a gas mixture

Pn=nn(RT/V)

18
Q

How can you find the total pressure in a mixture of gases?

A

Ptotal=(n1+n2+n3+…)(RT/V)

19
Q

How can we find the mole fraction (Xa) of a mixture of gases? How can we use the mole fraction in an equation the find the partial pressure?

A

Xa=na/ntotal

Pa=XaPtotal

20
Q

How do scientists collect gas?

A

They set up an apparatus for the displacement of water, they force the gas into a device with water so the gas bubbles through it into a flask where it is trapped

21
Q

What is vapour pressure? How does vapour pressure change with temperature?

A

The partial pressure of water in the resulting mixture after gas has been displaced when collecting gas

Temperature goes up, vapour pressure goes up

22
Q

How do we use stoichemetry in gases? What equation etc

A

Find numbers of moles using
n=PV/RT
Use mole ratiosi

23
Q

What are the three points of the kinetic molecular theory?

A
  1. The size of a particle is negligibly small- assumes particles occupy no volume
  2. The average kinetic energy of a particle is proportional to the temperature in kelvin’s
  3. The collision of one particle with another (or with walls) is completely elastic- means when particles collide they may exchange energy and but there is no loss of energy
24
Q

What equation shows that the kinetic energy of a particle depends on its mass and velocity? How do light particles travel in difference of speed of heavier ones at a given temp?

A

KE=1/2mv^2

In a gas mixture at a given temperature, lighter particles travel faster (on average) than heavier ones

25
Q

When are the two instances that gases behave ideally? (Both instances must be true)

A

A. The volume of the gas particles is negligible compared to the space between them
B. The forces between the gas particles are not significant

26
Q

When does the finite volume of gas particles become important?

A

It becomes important at high pressure, when the particles themselves occupy a significant portion of the total gas volume

27
Q

What is the corrected ideal gas equation for real gases?

A

V=nRT/p + nb
Where n is the number of moles and b is a constant that depends on the gas

(V-nb) = nRT/P

28
Q

What are intermolecular forces?

A

The attractions between the atoms or molecules in a gas
They are small and therefore do not matter much at low pressure
Don’t matter at high temps either because the molecules have a lot of kinetic energy

29
Q

What is the corrected ideal gas equation for intermolecular forces?

A

P=nRT/V - a(n/V)^2

Where a is a constant that depends on the gas

30
Q

What is Van der Waals equation?

A

The equation that describes non ideal gas behaviour

(P+a(n/V)^2) x (V-nb) = nRT

Chem 112 (11 decks)

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