Forms of Matter: Gases Flashcards

Unit Exam

1
Q

What are the properties of Gases

A
  1. Gases are compressible
    2.Gases expand as temperature is increased
    3.Gases have very low viscosity
  2. Gases have much lower densities then solids or liquids
  3. Gases are miscible
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2
Q

Explain the property “Gases are compressible”

A

The volume of a gas decreases dramatically when pressure is exerted on the gas because molecules are spaced further apart then liquids

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3
Q

Explain the property “ Gases expand as temperature is increased”

A

Only when pressure remains constant, and that is because molecules are moving faster and have more kinetic energy

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4
Q

Explain the property “ Gases have very low viscosity”

A

They have low resitant to flow

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5
Q

Explain the property “ Gases have much more lower densities then solids or liquids”

A

There is more space between particles.

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6
Q

Explain the peroperty “Gases are miscible”

A

They mix completely and evenly with eachother when put in the same container

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7
Q

What is the kinetic molecular theory(KMT)

A

It is a theory that provides a scientific moedel for explaining the behavior of gases

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8
Q

What is an ideal gase

A

A hypothetical gas that obeys all gas laws perfectly under all conditions

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9
Q

What is a real gas

A

real gases deviate from ideal gases under certain coniditons

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10
Q

One difference between ideal gases and real gases

A

Ideal gas molecules are very far apart, so the molecules sizes are negligible.
Real gases(under high pressures) the molecules are close together so their sizes are significant.

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11
Q

Another difference between ideal gases and real gases

A

Ideal gases are in constant straight line motion because no force exists between them. Realgases(as temperature decreases) molecules slow down, then at some point intermolecular attractions cause molecules to stick together then it turns into liquid.

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12
Q

Aother difference between ideal and real gases

A

Ideal gase molecules undergo perfect elastic collisions i which no energy is lost and the rebound happens quickly. During collision real gas molecules shape changes and rebound happens slower.(meaning pressure is less then ideal(

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13
Q

What is gas pressure

A

gas pressure is a measure of the force exerted by moving gas molecules per unit area.

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14
Q

What is atomispheric pressure

A

It is the force per unit are exrted by air on all objects

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15
Q

State the conversion units

A

760mmHg=1atm=101.325kPa

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16
Q

What is temperature

A

temperature is a measure of the normal amount of kinetic energy or particles. (the more the kinetic energy particles have the higher the temperature)

17
Q

What is absolute zero

A

Lowest possible temperature (0K, -273.15 degrees celcius)(theoretically this is the state in which all movement of kinetic energy is at zero)

18
Q

How do you go from celcius to Kelvin

A

Add 273.15 to celcius

19
Q

How do you go from Kelvin to celcius

A

Subtract 273.15 from kelvin

20
Q

What is STP

A

Standar temperature and pressure
Pressure-100kPa
temperature-273.15K(0 degreese celcius)

21
Q

What is SATP

A

Staandard ambient temperature and pressure
Pressure-100kPa
temperature-298.15K(25 degrees celcius)

22
Q

What is Gay-Lussac’s law of combining volumes

A

it is a law that states when measured at the same temperature and pressure, the volumes of gas reactants and profucts of chemical reactions are always in simpler ratios of whole numbers

23
Q

What is Boyles Law?

A

Boyles law is a law that states that as the pressure on a gas increases the volume of the gas decreases proportionally, provided that temperature and ehcmical amiunt stay constant.

24
Q

Explain boyles law

A

Increasing pressure causes volume to be smaller meaning molecules are closer together, and when they are closer together there is more frequent collisions between molecules increasing the pressure.(vice versa) less pressure– molecules further apart, volume increasing.

25
Q

WHat relationship do pressure and volume have

A

Inverse relationship

26
Q

What is the formula for boyles law

A

P(initial)V(initial)=P(final)V(final)

27
Q

What is charles law

A

Charles law states that as the temperature increases the volume increases proportionally, provided that the pressure and chemical amount remain constant

28
Q

What is the formula for charles law

A

V(initial)/T(initial)=V(final)/T(final)

29
Q

What type of relationship do volume and temperature have

A

They have a directly proportional relationship

30
Q

Avagadros law

A

According to avagadros law equal volumes of gasses at the same temperature and pressure contain equal numbers of moles, when avagadros number equals to 6.0x10^23mol

31
Q

What type of relationship do temperature and pressure have

A

they have a direct relationship

32
Q

SATP molar volume-

A

24.8L/mol

33
Q

STP molar volume

A

22.7L/mol

34
Q

What does comined gas law states

A

The combined gas law states that the product of the pressure and volume of a gas is proportional to its absolute temperature when the chemical amount remains constant.

35
Q

What is the ideal gas law

A

describes the interrelationship of pressure, temperature, volume and chemical amount of matter.

36
Q

equation for ideal gas law

A

PV=nRT
(v=L not any other unit)
(T= always in kelvin)