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Chem > Ch 11 Section 2 > Flashcards

Ch 11 Section 2 Flashcards

1
Q

Robert Boyle discovered that gas pressure and volume are

A

related mathematically

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2
Q

the observations of Boyle and others led to the development of the

A

gas laws

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3
Q

the gas laws are simple mathematical relationships between the

A

volume, temperature, pressure, and amount of a gas

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4
Q

Robert Boyle discovered that doubling the pressure on a sample of gas at constant temperature reduces its

A

volume by one-half

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5
Q

reducing the pressure on a gas by one-half allows the volume of the gas to

A

double

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6
Q

the pressure of a gas is caused by moving molecules hitting the

A

container walls

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7
Q

if volume of container is decreased but same number of gas molecules is present at the same temperature then there will be more molecules per

A

unit volume

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8
Q

the number of collisions with a given unit of wall area per unit time will …. and therefore…

A

increase as a result; pressure will also increase

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9
Q

plotting values of volume versus pressure for a gas at constant temperature gives a

A

curve

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10
Q

the general-volume pressure relationship illustrated is called

A

boyle’s law

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11
Q

boyle’s law states that the volume of a fixed mass of gas varies inversely with the pressure at

A

constant temperature

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12
Q

Boyle’s la can be expressed as : PV=

A

k

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13
Q

P is

A

pressure

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14
Q

V is

A

volume

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15
Q

k is a

A

constant

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16
Q

Since P and V vary inversely, their product remains the

A

same

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17
Q

because two quantities that are equal to the same thing are equal to each other, the relationship between changes of pressure and volume can be expressed as: P1V1 =

A

P2V2

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18
Q

P1 and V1 are

A

initial conditions

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19
Q

P2 and P2 are a

A

different set of conditions

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20
Q

given three of the four values P1, V1, P2, and V2, you can use this equation to calculate the fourth value for a

A

system at constant temperature

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21
Q

if pressure is constant, gases expand when

A

heated

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22
Q

when temperature increases, the volume of a fixed number of gas molecules must increase if the pressure is to

A

stay constant

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23
Q

at the higher temperature, the gas molecules move

A

faster

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24
Q

they collide with the walls of the container more frequently and with more

A

force

25
Q

the volume of a flexible container must then increase in order for the pressure to

A

remain the same

26
Q

the quantitative relationship between volume and temperature was discovered by the French scientist

A

Jacques charles in 1787

27
Q

Charles’s experiments showed that all gases expand to the same extent when heated through the

A

same temperature interval

28
Q

charles found that the volume changes by 1/273 of the original volume for each

A

celsius degree, at constant pressure and initial temp of 0 degrees celsius

29
Q

the same regularity of volume change occurs if a gas is cooled at

A

constant pressure

30
Q

the kelvin temperature scale is a scale that starts at a temperature corresponding to

A

-273.15 degrees celsius

31
Q

-273.15 degrees celsius is the lowest one

A

possible

32
Q

the temperature -273.15 degrees celsius is referred to as absolute zero and is given a value of

A

zero in the Kelvin scale

33
Q

K =

A

273.15 + degrees C

34
Q

gas volume and kelvin temperature are

A

directly proportional to each other at constant pressure

35
Q

charles’s law states that the volume of a fixed mass of gas at constant pressure varies directly with the

A

Kelvin temperature

36
Q

charles’s law:
V =
k=

A

V = kT

V/T= k

37
Q

the value of T is the

A

kelvin temperature

38
Q

The ratio V/T for any set of volume-temperature values always equals the same

A

k

39
Q

the form of charles’s law that can be applied directly to most volume temperature problems involving gases is:

A

V1/ T1 = V2/ T2

40
Q

V1 and T1 represent

A

initial conditions

41
Q

V2 and T2 represent a

A

different set of conditions

42
Q

when 3 of the 4 values T1, V1, T2, and V2 are known, the equation can be used to calculate the fourth value for a

A

system at constant pressure

43
Q

the energy and frequency of collisions depend on the average

A

kinetic energy of molecules

44
Q

for a fixed quantity of gas at constant volume, the pressure should be directly proportional to the

A

Kelvin temperature, which depends directly on average kinetic energy

45
Q

for every kelvin of temperature change, the pressure of a confined gas changes by

A

1/273 of the pressure at 0 degrees C

46
Q

Gay-Lussac’s law: the pressure of a fixed mass of gas at constant volume varies

A

directly with the Kelvin temperature

47
Q

Gay-Lussac’s law is expressed as :
P =
k=

A

P = kT

P/T= k

48
Q

in gay lussac’s law k is constant that depends on the

A

quantity of gas and volume

49
Q

for given mass of gas at constant volume, the ratio P/T is the same for any set of

A

pressure-temperature values

50
Q

unknown values can be found using the following form of gay-lussac’s law:

A

P1/ T1 = P2/ T2

51
Q

a gas sample often undergoes changes in temperature, pressure, and volume all at the

A

same time

52
Q

the combined law expresses the relationship between

A

pressure, volume, and temperature of a fixed amount of gas

53
Q

combined gas law: k=

A

PV/ T

54
Q

in combined gas law, k depends on the

A

amount of gas

55
Q

combined gas law can also be written as:

A

P1V1/ T1 = P2V2/ T2

56
Q

each of the gas laws can be obtained from the combined gas law when the

A

proper variable is constant

57
Q

boyle’s law is obtained from the combined gas law when

A

temperature is constant

58
Q

because T1 = T2, T1 and T2 will canel out on both sides of the combined gas law equation, giving

A

Boyle’s law

Chem (54 decks)

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