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Chemistry 20 > Chapter 4: Textbook > Flashcards

Chapter 4: Textbook Flashcards

1
Q

How is force affected when exerted on a larger area?

A

The pressure is lower

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2
Q

How is force affected when exerted on a smaller area?

A

The pressure is higher

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3
Q

What is pressure?

A

The force per unit area

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4
Q

What kind of force is measured by gases?

A

The force exerted by moving molecules as they collide with objects in the path, particularly the walls of their container

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5
Q

What is the unit for pressure?

A

(Pa) Pascals

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6
Q

What is force measured in?

A

(N) Newtons

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7
Q

What does one Pascal measure?

A

The force of 1 N on an area of 1 Meter squared. 1 Pa = 1 N/m2

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8
Q

What is atmospheric pressure and the pressure of other gasses measured in?

A

Kilopascals (kPa)

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9
Q

What is a kPa?

A

1000 Pa or 1kN/m2 exactly

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10
Q

What is atmospheric pressure?

A

The force per unit area exerted by air on all objects

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11
Q

What is the atmospheric pressure at sea level?

A

About 101 kPa or

101.325 kPa exactly

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12
Q

What basis do scientists use to describe one standard atmosphere ( 1 atm)?

A

The atmospheric pressure at sea level 101.325 kPa

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13
Q

What were the previous standards for work with gases?

A

A temperature of 0 and a pressure of 1 atm/101.325 kPa

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14
Q

What conditions were known as Standard Temperature and Pressure (STP)?

A

0 degrees and 1 atm/101.325 kPa

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15
Q

What is the new standard for reporting the properties of substances called?

A

Standard Ambient Temperature and Pressure (SATP)

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16
Q

What are the definitions of Standard Ambient Temperature and Pressure (SATP)?

A

25 degrees and 100 kPa

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17
Q

How did Evangelista Torricelli accidentally invent a way for measuring atmospheric pressure?

A

He flipped over a glass tube filled with mercury into a tub filled with mercury and noticed how the mercury level change from day to day. This was called a Mercury Barometer

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18
Q

What did standard pressure used to be defined as?

A

760 Torr or 760mm Hg in honor Torricelli

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19
Q

What is 760 mm Hg equal to?

A

1 atm or 101.325 kPa

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20
Q

What happens to gases as pressure increases?

A

Their volume decreses

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21
Q

What happens to gases as pressure decreases?

A

The volume decreases

22
Q

What is the mathematical equations to represent Pressure and volume in gases?

A

PV = k

23
Q

What is Boyle’s Law?

A

As pressure on a gas increases, the volume of gas decreases proportionally, provided the temperature and chemical amount of gas remains constant

24
Q

What is the equation to represent Boyle’s law?

A

P1 x V1 = P2 x V2

So basically PV = A constant

25
Q

What did Jacques Charles discover?

A

The relationship between temperature and volume of gas

26
Q

What is absolute 0?

A

0 Kelvins = -273 The lowest possible temperature

27
Q

What is the basis for the Absolute or Kelvin temperature Scale?

A

Absolute 0

28
Q

How do convert Celcius to Kelvin?

A

You add 273

29
Q

What is the STP for Kelvin?

A

273.15 Kelvin

30
Q

What is the SATP for Kelvin?

A

298.15 Kelvin

31
Q

What is the boiling point of water in Kelvin?

A

273 K

32
Q

What is the freezing point of water in Kelvin?

A

273 K

33
Q

What is Charles law?

A

As the temperature of a gas increases, the volume of the gas increases proportionally, provided that the pressure and chemical amount of gas remain constant

34
Q

What is the mathematical relationship the represents Charles law?

A

V1/T1 = V2/T2

so basically V/T = a constant

35
Q

What are thermocouples best for?

A

High temperatures such as ovens

36
Q

What are thermistors best suited for?

A

Low temperatures such as the home

37
Q

What is the combined gas law?

A

The product of the pressure and volume of a gas sample is proportional to its absolute temperature in Kelvin.

38
Q

What is the equation for the combined gas law?

A

PV/T= A constant (k) which means k is a constant as long as the amount of gas does not change

39
Q

What does kinetic molecular theory explain?

A

Why gases, unlike solids and liquids, are compressible

40
Q

Describe kinetic molecular theory as it pertains to solid, liquids and gas?

A

In solids the distance between its molecules are about the same size of it molecules. In liquids the spaces are slightly greater. In gases the distances are about 20 - 30 times greater.
If most of the volume of gases are empty space then it should be possible to force the molecules together

41
Q

How will gases be affected if a volume of a container is reduced?

A

Gas molecules will move a shorter distance before colliding with the walls of a container. Since they collide with the walls more frequently, there will be increased pressure on the container

42
Q

What is the pressure of gas relating to its container?

A

Basically pressure exerted by a gas is the total force of the collisions between the gas molecules and the walls distributed over an area of the container wall.

43
Q

How does kinetic Molecular theory explain Charles law?

A

An increase in temperature represents an increase in average kinetic energy and therefore the average speed of the entities’ motion. In a container where pressure can be kept constant, faster moving molecules with collide more frequently with container walls. Thus the volume of gas increases with temperature

44
Q

What is the law of combining volumes/Gay-Lussac’s law?

A

When measures at the same temperature and pressure, volumes of gaseous reactants and products of chemical reactions are always in simple ratios of whole numbers

45
Q

What was Avogadro’s Theory?

A

Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules

46
Q

What is Molar Volume?

A

The volume that one mole of gas occupies at a specified temperature and pressure. That means molar volume is the same for all gases at the same temperature and pressure

47
Q

What is the molar volume of gas at SATP?

A

24.8 L/mol

48
Q

What is the molar volume of gas at STP?

A

22.4 L/mol

49
Q

What is the symbol for molar volume?

A

Vm

50
Q

What is an ideal gas?

A

A hypothetical gas that obeys all the gas laws perfectly under all conditions. It does not condense into liquid when cooled. And graphs of it are perfectly straight lines

51
Q

What are the assumptions for ideal gasses?

A
  • The gas molecules are very far apart, so their size is negligible
  • They are in constant, random straight line motion
  • they go through collisions in which no energy is lost
52
Q

What is the equation for the ideal gas law?

A

PV = nRT

Chemistry 20 (10 decks)

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