20 Gases Flashcards

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1
Q

Boyle’s law

A

States that for a fixed mass of gas at constant temperature

pV = constant

Measurements plotted as a graph of pressure against 1 / volume gives a straight line through the origin

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2
Q

Charles’ law

A

For a fixed mass of an ideal gas at constant pressure, its volume is directly proportional to its absolute temperature

V / T = constant

Work done = p 🔺v

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3
Q

Isobaric change

A

Any change at constant pressure

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4
Q

Isothermical

A

Any change at constant temperature

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5
Q

Pressure law

A

For a fixed mass of ideal gas at constant volume, its pressure is directly proportional to its absolute temperature

P / T = constant

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6
Q

Brownian motion

A

The random and unpredictable motion of a particle such as smoke particle caused by molecules of the surrounding substance colliding at random with the particle. Its discovery provided evidence for the existence of atoms

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7
Q

Avogadro constant

A

The number of atoms in 12g of the carbon istope 12 carbon is defined as a mole. The value is 6.02 x10^23

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8
Q

Pressure

A

Pressure of gas is the force per unit area that the gas exerts normally

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9
Q

Molarity

A

number of moles of a certain quality of a substance

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10
Q

ideal gas equation

A

Pv=nRT

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11
Q

molar gas constant

A

8.31

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12
Q

plot a graph of pV against T

A

line with the gradient = nR

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13
Q

Boltzmann constant (k)

A

molar gas constant divded by the avogardo number

1.38*10-23

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14
Q

Root mean square speed

A

square root of the mean value of the square of the molecular speeds.

Crms = [ C1^2 + C2^2 + Cn^2 / N ]^1/2

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15
Q

kinetic theory equation

A

pV=1/3Nm(crms)^2

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16
Q

mole

A

one mole of a substance consisting of identical particles is the quantity of substance that contains N particles of the substance

17
Q

molar mass

A

the mass of one mole of a substance

18
Q

ideal gas

A

a gas under conditions such that it obeys boyle’s law

19
Q

pressure law

A

for a fixed mass of an ideal gas at constant volume, its pressure is directly proportional to its absolute temperature

20
Q

kinetic energy

A

the energy of moving object due to its motion. for an object of mass m moving at speed v, it kinetic energy.

Ek = 1/2 mv^2

21
Q

kinetic energy of the molecules of an ideal gas

A

mean kinetic energy of a molecule of an ideal gas = 3/2KT

total kinetic energy of n moles of an ideal gas = 3/2 nRT

22
Q

kinetic theory of a gas

A

gas consists of identical point molecules which do not attract another
random motion
collided elastically

pV= 1/3 Nm (Crms)^2

23
Q

kinetic theory of gas equation

A

pV= 1/3 Nm (Crms)^2

24
Q

Pv = 1/3 Nmc^2

A
P= pressure on the side of the box
V = volume of the molecules in the box
N = number of particles in the box
M = mass of one particle
C^2 = mean square speed
25
Q

Random motion

A

When molecules are in a state of random motion they have a range of speeds and have no preferred direction of movement

Quality of a liquid and gas as described by kinetic energy

26
Q

State the assumptions used in the derivation pv= 1/3Nmc^2

A
Elastic collision
Intermolecular forces are negligible
Volume of molecules negligible
All molecules identical
Newtons laws of motion apply
27
Q

Describe how the motion of gas molecules can be used ti explain the pressure exerted by a gas on the walls of the container

A

Molecules are in constant random motion. When the molecules collide the walls exert a force on the molecules causing a change in momentum. The molecules exerts an force on the walls creating pressure

28
Q

what happens if the temperature of gas is increased

A

molecules move faster
root mean square increases
distribution curve becomes flatter and broader

29
Q

work done

A

pV

30
Q

average molecular kinetic energy

A

1/2 m(Crms)^2 = 3/2 KT = 3RT / 2N