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Chemistry > Chapter 5- States Of Matter > Flashcards

Chapter 5- States Of Matter Flashcards

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0
Q

Variables that can be measured for real gases

A

Temperature
Pressure
Volume
Quantity (mass)

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1
Q

A model of the way that particles behave at the microscopic level

A

Ideal gas

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2
Q

Force per unit area. Measured with a barometer.

A

Pressure

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3
Q

1 atm=

A

760 mmHg
OR
760 torr

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4
Q

Provides a reasonable explanation of the behavior of gases.

A

Kinetic molecular theory of gases

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5
Q

Gases are made up of tiny atoms or molecules that are in constant, random motion.

A

Kinetic molecular theory of gases

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6
Q

The distance of separation among these atoms or molecules is very large in comparison to the size of the individual atoms or molecules— gas is mostly empty space.

A

Kinetic molecular theory of gases.

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7
Q

All the atoms and molecules behave independently. No attractive or repulsive forces exist between atoms or molecules in a gas.

A

Kinetic molecular theory of gases.

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8
Q

Atoms & molecules collide w/ each other & w/ the walls of the container w/o losing energy. The energy is transferred from one atom or molecule to another.

A

Kinetic molecular theory of gases

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9
Q

The average kinetic energy of the atoms or molecules increases or decreases in proportion to the absolute temperature.

A

Kinetic molecular theory of gases.

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10
Q

Temperature increase=

A

Energy increases

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11
Q

Temperature decreases=

A

Energy decreases.

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12
Q

Easily compressible

A

Property of gas

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13
Q

Expand to fill any available volume

A

Property of gas

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14
Q

Low density

A

Property of gas

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15
Q

Readily diffuse through each other

A

Property of gas

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16
Q

Exert pressure on their containers

A

Property of gas

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17
Q

Behave ideally at low pressures and high temperatures

A

Property of gas

18
Q

The volume of gas varies inversely with the pressure exerted by the gas if the number of miles and the temperature of the gas are held constant.

A

Boyle’s law

19
Q

PiVi=PfVf

A

Boyle’s law

20
Q

The volume of gas varies directly with the absolute temperature (K) if pressure and number of moles of gas are constant.

A

Charles’ law

21
Q

Vi/Ti = Vf/Tf

A

Charles’ law

22
Q

What is a good example of Boyle’s law?

A

Syringe

23
Q

What is a good example of Charles’ law?

A

Hot air balloons.

24
Q

Used when a sample of gas undergoes change involving volume, pressure, and temperature at the same time.

A

Combined gas law

25
Q

PiVi/Ti = PfVf/Tf

A

Combined gas law

26
Q

What two laws is the combined gas law made of?

A

Boyle’s and Charles’ laws

27
Q

The relationship between the volume and number of moles of a gas at constant temperature and pressure.

A

Avogadro’s law

28
Q

Equal volumes of any ideal gas contain the same number of moles if measures under the same conditions of temperature and pressure.

A

Avogadro’s law

29
Q

If there are more gas molecules, volume will increase

A

Avogadro’s law

30
Q

Vi/ni = Vf/nf

A

Avogadro’s law

31
Q

n=

A

Mol

32
Q

A combination of Boyle’s law, Charles’ law, and Avogadro’s law

A

Ideal gas law

33
Q

R= 0.0821 Latm/molK

A

Ideal gas law

34
Q

R=

A

0.0821 Latm/molK

35
Q

PV=nRT

A

Ideal gas law

36
Q

Units used in the ideal gas law

A

P-atm
V-liters
n-# of moles
T-Kelvin

37
Q

The volume occupied by 1 mol of any gas is referred to as its ___

A

Molar volume

38
Q

At standard temperature and pressure (STP), the molar volume of any gas is ____

A

22.4 L

39
Q

STP conditions

A 
T= 273 K
P= 1.00 atm
V= 22.4 L
40
Q

The density of gases at STP can be found using the formula ___

A

d= MW/V

41
Q

MW means what?

A

Molecular weight or molecular mass

42
Q

A mixture of gases exerts a pressure that is the sum of the pressures that each gas would exert if it were present alone under the same conditions.

A

Dalton’s law of partial pressure

43
Q

Pt= p1+p2+p3+….

A

Dalton’s law of partial pressure

Chemistry (3 decks)

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